Question 1

When baking soda is heated it decomposes according to the following reaction: 2 NaHCO₃(s)⇌ Na₂CO₃(s)+ H₂O(g)+ CO₂(g) If sufficient baking soda is placed in a container and heated to 90°C,the total pressure of the gases is 0.5451 atm.What is the value of K_p at that temperature?

Accepted Answer

The correct answer is A.The equilibrium constant, Kp, is given by the expression:Kp = (P(CO2) * P(H2O)) / P(NaHCO3)^2At 90°C, the total pressure of the gases is 0.5451 atm. Since the reaction produces equal moles of CO2 and H2O, the partial pressure of each gas is 0.5451 atm / 2 = 0.27255 atm.The partial pressure of NaHCO3 is not given, but it can be assumed to be negligible compared to the partial pressures of the gases. Therefore, we can approximate Kp as:Kp ≈ (0.27255 atm * 0.27255 atm) / (1 atm)^2 = 0.07428Therefore, the value of Kp at 90°C is approximately 0.07428.

Question 2

At a certain temperature the equilibrium constant,K_c,equals 0.11 for the reaction: 2 ICl(g)⇌ I₂(g)+ Cl₂(g). What is the equilibrium concentration of ICl if 0.75 mol of I₂ and 0.75 mol of Cl₂ are initially mixed in a 2.0-L flask?

Accepted Answer

First, we need to use the equilibrium constant equation to set up an expression for the equilibrium concentration of ICl: K_c = [I₂][Cl₂]/[ICl]2 We can plug in the initial concentrations to solve for the equilibrium concentration of ICl: 0.11 = (0.75 mol/L)2 / x2 x2 = (0.75 mol/L)2 / 0.11 x = 0.45 mol/L So the equilibrium concentration of ICl is 0.45 M.

Question 3

For acid solutions of the same molarity acid strength is proportional to the equilibrium concentration of H₃O⁺.For equimolar solutions of acids,which equilibrium expression below corresponds to the strongest acid?

Accepted Answer

The answer of For acid solutions of the same molarity...

Question 4

Cyclohexane (C₆H₁₂)undergoes a molecular rearrangement in the presence of AlCl₃ to form methylcyclopentane (CH₃C₅H₉)according to the equation: C₆H₁₂ ⇌ CH₃C₅H₉ If K_c = 0.143 at 25°C for this reaction,find the equilibrium concentrations of C₆H₁₂ and CH₃C₅H₉ if the initial concentrations are 0.200 M and 0.100 M,respectively.

Accepted Answer

The answer of Cyclohexane (C₆H₁₂)undergoes a molecular rearrangement in the...

Question 5

Oxalic acid can donate two protons to water in successive reactions: (1)H₂C₂O₄(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ HC₂O₄^-(aq) (2)HC₂O₄^-(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ C₂O₄^2-(aq) If K_c1 = 5.9 × 10^-2 and K_c2 = 6.4 × 10^-5 at 25°C,what is the value of K_c for reaction (3)? (3)H₂C₂O₄(aq)+ 2 H₂O(l)⇌ 2 H₃O⁺(aq)+ C₂O₄^2-(aq)

Accepted Answer

The overall equilibrium constant $K_c$ for reaction (3) is the product of the equilibrium constants for reactions (1) and (2), i.e., $K_{c1} \times K_{c2} = 5.9 \times 10^{-2} \times 6.4 \times 10^{-5} = 3.776 \times 10^{-6}$, which is approximately $3.8 \times 10^{-6}$.

Question 6

Ammonium carbamate can dissociate into gases at 25°C according to the reaction: NH₂COONH₄(s)⇌ 2 NH₃(g)+ CO₂(g) If sufficient ammonium carbamate is sealed in a flask,the total pressure will be 0.117 atm at equilibrium.What is the value of K_p at 25°C?

Accepted Answer

The equilibrium expression for the dissociation of ammonium carbamate into gases is given by $K_p = \frac{P_{NH_3}^2 \cdot P_{CO_2}}{P_{solid}}$. Since the pressure of the solid is constant and not included in the $K_p$ expression, we can simplify the expression to $K_p = P_{NH_3}^2 \cdot P_{CO_2}$. At equilibrium, the total pressure ($P_{total}$) is the sum of the partial pressures of $NH_3$ and $CO_2$. Given that $2NH_3$ and $1CO_2$ are produced, for every mole of ammonium carbamate that dissociates, the ratio of $NH_3$ to $CO_2$ will be 2:1. Therefore, if $x$ is the partial pressure of $CO_2$, then $2x$ will be the partial pressure of $NH_3$, making $P_{total} = 3x = 0.117$ atm. Solving for $x$ gives $x = 0.039$ atm. Substituting these values into the $K_p$ expression gives $K_p = (2x)^2 \cdot x = (2 \cdot 0.039)^2 \cdot 0.039 = 2.37 \times 10^{-4}$.

Question 7

Gaseous hydrogen bromide decomposes at elevated temperatures according to the following equation: . At a certain temperature a 2.00 L flask is initially filled only with 0.600 mol of HBr.What is the value of K_c at that temperature if the flask contains 0.104 mol of H₂ at equilibrium?

Accepted Answer

The answer of Gaseous hydrogen bromide decomposes at elevated temperatures...

Question 8

Salt solubilities can be compared by the concentration of cation formed when the salt dissolves in the general reaction: M_aX_b(s)⇌ a M^b+(aq)+ b X^a-(aq).Given the following salts and their equilibrium constants for the reaction above at 25°C,which salt is the least soluble?

Accepted Answer

The least soluble salt is the one with the lowest solubility product constant (Ksp). AgCl has the lowest Ksp value (1.8 × 10^-10), indicating it is the least soluble among the given options.

Question 9

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the reaction: PCl₅(g)⇌ PCl₃(g)+ Cl₂(g) At 250°C,0.250 M PCl₅ is added to a flask.If K_c = 1.80,what are the equilibrium concentrations of each gas?

Accepted Answer

First, we need to set up the equilibrium expression and the ICE table:

Equilibrium expression:

Kc = [PCl5] / ([PCl3] * [Cl2])

ICE table:

PCL5  <----> PCL3    +   Cl2
I           0.250                   0                         0
C          0.250 – x                 x                         x
E         0.250 – x                 x                         x

We can substitute the equilibrium concentrations into the equilibrium expression and solve for x:

1.80 = (x)(x) / (0.250 – x)

Then, we can solve for x using the quadratic formula:

x = 0.222 M

Therefore, the equilibrium concentrations are:

[PCl5] = 0.250 – x = 0.0280 M 
[PCl3] = x = 0.222 M 
[Cl2] = x = 0.222 M

The only answer choice that matches this is A.

Question 10

The equilibrium constant K_cfor the reaction HF(aq)+ H₂O(l)⇌ H₃O⁺(aq)+F^-(aq)is 3.5 × 10^-4.What is the equilibrium concentration of H₃O⁺ if the initial concentration of HF is 1.0 M?

Accepted Answer

The equilibrium constant expression for the given reaction is: K_c=([H₃O⁺][F^-])/([HF][H₂O]) Given K_c=3.5 × 10^-4 Initial concentration of HF = 1.0 M Assume the equilibrium concentration of H₃O⁺ to be x Since HF and H₂O are reactants, their concentrations are not changed when the reaction reaches equilibrium. Therefore, their concentrations will be equal to their initial concentrations, which are 1.0 M and 1.0 M, respectively. Substituting the given and assumed values in the equilibrium constant expression, we get: 3.5 × 10^-4=([x][F^-])/([1.0][1.0]) x = (3.5 × 10^-4)(1.0)/(1.0)= 3.5 × 10^-4 M Therefore, the equilibrium concentration of H₃O⁺ is 1.9 × 10^-2 M. (C)

Question 11

Consider the reaction HCO₃^- (aq)+ H₂O (l)⇌ CO₃^-2 (aq)+ H₃O+ (aq) The K_eq for this reaction is 5.6 × 10^-11.Describe what will happen to the reaction if the concentration of each reactant is [HCO₃^-] = 5.6 × 10^-11[H₃O⁺] = 1.2 × 10^-11[CO₃^-] = 5.6 × 10^-11

Accepted Answer

The answer of Consider the reaction HCO₃^- (aq)+ H₂O (l)⇌...

Question 12

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0015 M O₂.At this temperature,K_c,equals 1.4 × 10² for the reaction: 2 CO(g)+ O₂(g)⇌ 2 CO₂(g). What is the equilibrium concentration of CO?

Accepted Answer

The equilibrium constant $K_c$ for the reaction $2 CO(g) + O_2(g) \rightleftharpoons 2 CO_2(g)$ is given by $K_c = \frac{[CO_2]^2}{[CO]^2[O_2]}$. Given $K_c = 1.4 \times 10^{12}$, $[CO_2] = 0.0010$ M, and $[O_2] = 0.0015$ M, we can solve for $[CO]$. Rearranging the equation for $K_c$, we get $[CO] = \sqrt{\frac{[CO_2]^2}{K_c[O_2]}}$. Plugging in the given values, $[CO] = \sqrt{\frac{(0.0010)^2}{1.4 \times 10^{12} \times 0.0015}} = 2.2 \times 10^{-3}$ M.

Question 13

K_p is equal to 48.70 at 731 K for the reaction: H₂(g)+ I₂(g)⇌ 2 HI(g).Initially the mixture contains 0.08592 atm each of H₂ and I₂ and 1.0000 atm of HI.What is the pressure of HI at equilibrium?

Accepted Answer

The answer of K_p is equal to 48.70 at 731...

Question 14

At a certain temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g)+ O₂(g)⇌ 2 CO₂(g). If a 2.50-L flask contains 0.400 mol of CO₂ and 0.100 mol of O₂ at equilibrium,how many moles of CO are also present in the flask?

Accepted Answer

To find the moles of CO, use the equilibrium expression: Kc = [CO2]^2 / ([CO]^2[O2]). Calculate concentrations: [CO2] = 0.400 mol / 2.50 L, [O2] = 0.100 mol / 2.50 L. Solve for [CO] using Kc = 1.4 × 10^2.

Question 15

The solubility of 1:1 salts is measured by the equilibrium constant for the general reaction: MX(s)= Mⁿ⁺(aq)+ X^n-(aq).Given the following salts and their equilibrium constants for the reaction above at 25°C,which salt is the least soluble?

Accepted Answer

The solubility of a salt is inversely related to the value of its equilibrium constant. The salt with the smallest equilibrium constant is the least soluble. SrCO3 has the smallest equilibrium constant (5.6 × 10^-10), making it the least soluble.

Question 16

The equilibrium constant,K_p,equals 3.40 for the isomerization reaction: cis-2-butene ⇌ trans-2-butene. If a flask initially contains 0.250 atm of cis-2-butene and 0.125 atm of trans-2-butene,what is the equilibrium pressure of each gas?

Accepted Answer

The answer of The equilibrium constant,K_p,equals 3.40 for the isomerization...

Question 17

The esterification of acetic acid and ethanol is given by the reaction below: C₂H₅OH(aq)+ CH₃COOH(aq)⇌ CH₃COOC₂H₅(aq)+ H₂O(l) When 1.00 mol of ethanol was mixed with 2.00 mol of acid in a 1.00 L flask,0.86 mol of ester was formed at room temperature.What is the value of the equilibrium constant,K_c?

Accepted Answer

The balanced chemical equation for the reaction is:
CH3CH2OH + CH3COOH ⇌ CH3COOCH2CH3 + H2O

The equilibrium constant expression is given by:
Kc = ([CH3COOCH2CH3] / [CH3CH2OH] [CH3COOH])

At equilibrium, the concentration of ethanol is (1 - 0.86) = 0.14 mol/L, the concentration of acetic acid is (2 - 0.86) = 1.14 mol/L, and the concentration of ester is 0.86 mol/L.

Substituting the values into the equilibrium constant expression, we get:
Kc = (0.86 / (0.14 x 1.14))
Kc = 5.351

Therefore, the value of the equilibrium constant is 5.4 (rounded to one significant figure).

The correct answer is D.

Question 18

The following two isomers of C₃H₇NO exist in equilibrium with each other in solution: If K_c = 0.57 at 25°C and the initial concentration of the reactant is 0.50 M and the product is 0.70 M,what are the concentrations at equilibrium?

Accepted Answer

The answer of The following two isomers of C₃H₇NO exist...

Question 19

Acids donate protons to water according to the general equation: HA(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ A^-(aq) Consider the following acids and their equilibrium constants for reaction with water at 25°C.If all the acids have the same initial concentration,which is the strongest acid (i.e.which donates the most protons to water)?

Accepted Answer

HIOS3 has the highest equilibrium constant (Ka = 1.7 × 10^-1), indicating it donates the most protons to water, making it the strongest acid among the options.

Question 20

For the isomerization reaction: butane ⇌ isobutane K_p equals 25 at 500°C.If the initial pressures of butane and isobutane are 10.atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

Accepted Answer

First, we can set up an ICE table to represent the reaction:
Initial:   10 atm        0 atm
Change:   -x              +x
Equilibrium: 10-x      x
Using the equilibrium constant expression, we can set up the equation:
25 = (x)/(10-x)
Solving for x, we get x = 0.38 atm. 
Substituting x back into our ICE table, we get the equilibrium pressures to be:
P(butane) = 10 - x = 9.62 atm, and 
P(isobutane) = x = 0.38 atm. 
Thus, the answer is A.

Quiz 14: Chemical Equilibrium

When baking soda is heated it decomposes according to the following reaction: 2 NaHCO₃(s) ⇌ Na₂CO₃(s) + H₂O(g) + CO₂(g) If sufficient baking soda is placed in a container and heated to 90°C,the total pressure of the gases is 0.5451 atm.What is the value of K_p at that temperature?

At a certain temperature the equilibrium constant,K_c,equals 0.11 for the reaction: 2 ICl(g) ⇌ I₂(g) + Cl₂(g) . What is the equilibrium concentration of ICl if 0.75 mol of I₂ and 0.75 mol of Cl₂ are initially mixed in a 2.0-L flask?

For acid solutions of the same molarity acid strength is proportional to the equilibrium concentration of H₃O⁺.For equimolar solutions of acids,which equilibrium expression below corresponds to the strongest acid?

Ammonium carbamate can dissociate into gases at 25°C according to the reaction: NH₂COONH₄(s) ⇌ 2 NH₃(g) + CO₂(g) If sufficient ammonium carbamate is sealed in a flask,the total pressure will be 0.117 atm at equilibrium.What is the value of K_p at 25°C?

Gaseous hydrogen bromide decomposes at elevated temperatures according to the following equation: . At a certain temperature a 2.00 L flask is initially filled only with 0.600 mol of HBr.What is the value of K_c at that temperature if the flask contains 0.104 mol of H₂ at equilibrium?

Salt solubilities can be compared by the concentration of cation formed when the salt dissolves in the general reaction: M_aX_b(s) ⇌ a M^b+(aq) + b X^a-(aq) .Given the following salts and their equilibrium constants for the reaction above at 25°C,which salt is the least soluble?

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the reaction: PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) At 250°C,0.250 M PCl₅ is added to a flask.If K_c = 1.80,what are the equilibrium concentrations of each gas?

The equilibrium constant K_cfor the reaction HF(aq) + H₂O(l) ⇌ H₃O⁺(aq) +F^-(aq) is 3.5 × 10^-4.What is the equilibrium concentration of H₃O⁺ if the initial concentration of HF is 1.0 M?

Consider the reaction HCO₃^- (aq) + H₂O (l) ⇌ CO₃^-2 (aq) + H₃O+ (aq) The K_eq for this reaction is 5.6 × 10^-11.Describe what will happen to the reaction if the concentration of each reactant is [HCO₃^-] = 5.6 × 10^-11[H₃O⁺] = 1.2 × 10^-11[CO₃^-] = 5.6 × 10^-11

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0015 M O₂.At this temperature,K_c,equals 1.4 × 10² for the reaction: 2 CO(g) + O₂(g) ⇌ 2 CO₂(g) . What is the equilibrium concentration of CO?

K_p is equal to 48.70 at 731 K for the reaction: H₂(g) + I₂(g) ⇌ 2 HI(g) .Initially the mixture contains 0.08592 atm each of H₂ and I₂ and 1.0000 atm of HI.What is the pressure of HI at equilibrium?

At a certain temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g) + O₂(g) ⇌ 2 CO₂(g) . If a 2.50-L flask contains 0.400 mol of CO₂ and 0.100 mol of O₂ at equilibrium,how many moles of CO are also present in the flask?

The solubility of 1:1 salts is measured by the equilibrium constant for the general reaction: MX(s) = Mⁿ⁺(aq) + X^n-(aq) .Given the following salts and their equilibrium constants for the reaction above at 25°C,which salt is the least soluble?

The equilibrium constant,K_p,equals 3.40 for the isomerization reaction: cis-2-butene ⇌ trans-2-butene. If a flask initially contains 0.250 atm of cis-2-butene and 0.125 atm of trans-2-butene,what is the equilibrium pressure of each gas?

The following two isomers of C₃H₇NO exist in equilibrium with each other in solution: If K_c = 0.57 at 25°C and the initial concentration of the reactant is 0.50 M and the product is 0.70 M,what are the concentrations at equilibrium?

For the isomerization reaction: butane ⇌ isobutane K_p equals 25 at 500°C.If the initial pressures of butane and isobutane are 10.atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

Quiz 14: Chemical Equilibrium

When baking soda is heated it decomposes according to the following reaction: 2 NaHCO3(s) ⇌ Na2CO3(s) + H2O(g) + CO2(g) If sufficient baking soda is placed in a container and heated to 90°C,the total pressure of the gases is 0.5451 atm.What is the value of Kp at that temperature?

At a certain temperature the equilibrium constant,Kc,equals 0.11 for the reaction: 2 ICl(g) ⇌ I2(g) + Cl2(g) . What is the equilibrium concentration of ICl if 0.75 mol of I2 and 0.75 mol of Cl2 are initially mixed in a 2.0-L flask?

For acid solutions of the same molarity acid strength is proportional to the equilibrium concentration of H3O+.For equimolar solutions of acids,which equilibrium expression below corresponds to the strongest acid?

Ammonium carbamate can dissociate into gases at 25°C according to the reaction: NH2COONH4(s) ⇌ 2 NH3(g) + CO2(g) If sufficient ammonium carbamate is sealed in a flask,the total pressure will be 0.117 atm at equilibrium.What is the value of Kp at 25°C?

Gaseous hydrogen bromide decomposes at elevated temperatures according to the following equation: . At a certain temperature a 2.00 L flask is initially filled only with 0.600 mol of HBr.What is the value of Kc at that temperature if the flask contains 0.104 mol of H2 at equilibrium?

Salt solubilities can be compared by the concentration of cation formed when the salt dissolves in the general reaction: MaXb(s) ⇌ a Mb+(aq) + b Xa-(aq) .Given the following salts and their equilibrium constants for the reaction above at 25°C,which salt is the least soluble?

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the reaction: PCl5(g) ⇌ PCl3(g) + Cl2(g) At 250°C,0.250 M PCl5 is added to a flask.If Kc = 1.80,what are the equilibrium concentrations of each gas?

The equilibrium constant Kc for the reaction HF(aq) + H2O(l) ⇌ H3O+(aq) +F-(aq) is 3.5 × 10-4.What is the equilibrium concentration of H3O+ if the initial concentration of HF is 1.0 M?

Consider the reaction HCO3- (aq) + H2O (l) ⇌ CO3-2 (aq) + H3O+ (aq) The Keq for this reaction is 5.6 × 10-11.Describe what will happen to the reaction if the concentration of each reactant is [HCO3-] = 5.6 × 10-11 [H3O+] = 1.2 × 10-11 [CO3-] = 5.6 × 10-11

An equilibrium mixture of CO,O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 0.0015 M O2.At this temperature,Kc,equals 1.4 × 102 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g) . What is the equilibrium concentration of CO?

Kp is equal to 48.70 at 731 K for the reaction: H2(g) + I2(g) ⇌ 2 HI(g) .Initially the mixture contains 0.08592 atm each of H2 and I2 and 1.0000 atm of HI.What is the pressure of HI at equilibrium?

At a certain temperature,Kc equals 1.4 × 102 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g) . If a 2.50-L flask contains 0.400 mol of CO2 and 0.100 mol of O2 at equilibrium,how many moles of CO are also present in the flask?

The solubility of 1:1 salts is measured by the equilibrium constant for the general reaction: MX(s) = Mn+(aq) + Xn-(aq) .Given the following salts and their equilibrium constants for the reaction above at 25°C,which salt is the least soluble?

The equilibrium constant,Kp,equals 3.40 for the isomerization reaction: cis-2-butene ⇌ trans-2-butene. If a flask initially contains 0.250 atm of cis-2-butene and 0.125 atm of trans-2-butene,what is the equilibrium pressure of each gas?

The following two isomers of C3H7NO exist in equilibrium with each other in solution: If Kc = 0.57 at 25°C and the initial concentration of the reactant is 0.50 M and the product is 0.70 M,what are the concentrations at equilibrium?

For the isomerization reaction: butane ⇌ isobutane Kp equals 25 at 500°C.If the initial pressures of butane and isobutane are 10.atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?

When baking soda is heated it decomposes according to the following reaction: 2 NaHCO₃(s) ⇌ Na₂CO₃(s) + H₂O(g) + CO₂(g) If sufficient baking soda is placed in a container and heated to 90°C,the total pressure of the gases is 0.5451 atm.What is the value of K_p at that temperature?

At a certain temperature the equilibrium constant,K_c,equals 0.11 for the reaction: 2 ICl(g) ⇌ I₂(g) + Cl₂(g) . What is the equilibrium concentration of ICl if 0.75 mol of I₂ and 0.75 mol of Cl₂ are initially mixed in a 2.0-L flask?

For acid solutions of the same molarity acid strength is proportional to the equilibrium concentration of H₃O⁺.For equimolar solutions of acids,which equilibrium expression below corresponds to the strongest acid?

Ammonium carbamate can dissociate into gases at 25°C according to the reaction: NH₂COONH₄(s) ⇌ 2 NH₃(g) + CO₂(g) If sufficient ammonium carbamate is sealed in a flask,the total pressure will be 0.117 atm at equilibrium.What is the value of K_p at 25°C?

Gaseous hydrogen bromide decomposes at elevated temperatures according to the following equation: . At a certain temperature a 2.00 L flask is initially filled only with 0.600 mol of HBr.What is the value of K_c at that temperature if the flask contains 0.104 mol of H₂ at equilibrium?

Salt solubilities can be compared by the concentration of cation formed when the salt dissolves in the general reaction: M_aX_b(s) ⇌ a M^b+(aq) + b X^a-(aq) .Given the following salts and their equilibrium constants for the reaction above at 25°C,which salt is the least soluble?

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the reaction: PCl₅(g) ⇌ PCl₃(g) + Cl₂(g) At 250°C,0.250 M PCl₅ is added to a flask.If K_c = 1.80,what are the equilibrium concentrations of each gas?

The equilibrium constant K_cfor the reaction HF(aq) + H₂O(l) ⇌ H₃O⁺(aq) +F^-(aq) is 3.5 × 10^-4.What is the equilibrium concentration of H₃O⁺ if the initial concentration of HF is 1.0 M?

Consider the reaction HCO₃^- (aq) + H₂O (l) ⇌ CO₃^-2 (aq) + H₃O+ (aq) The K_eq for this reaction is 5.6 × 10^-11.Describe what will happen to the reaction if the concentration of each reactant is [HCO₃^-] = 5.6 × 10^-11[H₃O⁺] = 1.2 × 10^-11[CO₃^-] = 5.6 × 10^-11

An equilibrium mixture of CO,O₂ and CO₂ at a certain temperature contains 0.0010 M CO₂ and 0.0015 M O₂.At this temperature,K_c,equals 1.4 × 10² for the reaction: 2 CO(g) + O₂(g) ⇌ 2 CO₂(g) . What is the equilibrium concentration of CO?

K_p is equal to 48.70 at 731 K for the reaction: H₂(g) + I₂(g) ⇌ 2 HI(g) .Initially the mixture contains 0.08592 atm each of H₂ and I₂ and 1.0000 atm of HI.What is the pressure of HI at equilibrium?

At a certain temperature,K_c equals 1.4 × 10² for the reaction: 2 CO(g) + O₂(g) ⇌ 2 CO₂(g) . If a 2.50-L flask contains 0.400 mol of CO₂ and 0.100 mol of O₂ at equilibrium,how many moles of CO are also present in the flask?

The solubility of 1:1 salts is measured by the equilibrium constant for the general reaction: MX(s) = Mⁿ⁺(aq) + X^n-(aq) .Given the following salts and their equilibrium constants for the reaction above at 25°C,which salt is the least soluble?

The equilibrium constant,K_p,equals 3.40 for the isomerization reaction: cis-2-butene ⇌ trans-2-butene. If a flask initially contains 0.250 atm of cis-2-butene and 0.125 atm of trans-2-butene,what is the equilibrium pressure of each gas?

The following two isomers of C₃H₇NO exist in equilibrium with each other in solution: If K_c = 0.57 at 25°C and the initial concentration of the reactant is 0.50 M and the product is 0.70 M,what are the concentrations at equilibrium?

For the isomerization reaction: butane ⇌ isobutane K_p equals 25 at 500°C.If the initial pressures of butane and isobutane are 10.atm and 0.0 atm,respectively,what are the pressures of the two gases at equilibrium?