Question 1

Picture (1)represents an equilibrium mixture of solid CaCOS1U1B13S1U1B0,solid CaO,and gaseous COS1U1B12S1U1B0,obtained as a result of the endothermic decomposition of CaCOS1U1B13S1U1B0. 
-Which picture (2)-(4)represents the equilibrium mixture when more solid CaO is added?

Accepted Answer

The answer of Picture (1)represents an equilibrium mixture of solid...

Question 2

Nitric oxide reacts with oxygen to form nitrogen dioxide: 2 NO(g)+ O₂(g)⇌ 2 NO₂(g) What is K_c for the forward reaction if the equilibrium concentration of NO is 0.200 M,O₂ is 0.100 M,and NO₂ is 0.200 M at 25°C?

Accepted Answer

K_c is calculated using the equation: K_c = [NO₂]^2 / ([NO]^2 [O₂]) Substituting the given values: K_c = (0.2 M)^2 / [(0.2 M)^2 x (0.1 M)] K_c = 10.0 Therefore, the best choice is D.

Question 3

Picture (1)represents an equilibrium mixture of solid CaCOS1U1B13S1U1B0,solid CaO,and gaseous COS1U1B12S1U1B0,obtained as a result of the endothermic decomposition of CaCOS1U1B13S1U1B0. -Which picture (2)-(4)represents the equilibrium mixture when more solid CaCO₃ is added?

Accepted Answer

The answer of Picture (1)represents an equilibrium mixture of solid...

Question 4

The equilibrium constant,K_p,equals 3.40 at 25°C for the isomerization reaction: cis-2-butene ⇌ trans-2-butene. If a flask initially contains 3.00 atm of each gas,in what direction will the system shift to reach equilibrium?

Accepted Answer

Since the equilibrium constant (K) is greater than 1, it indicates that the system favors the product (trans-2-butene). Therefore, the system will shift to the right to reach equilibrium, meaning that more cis-2-butene will be converted to trans-2-butene until the concentrations reach an equilibrium state.

Question 5

The decomposition of ammonia is: 2 NH₃(g)⇌ N₂(g)+ 3 H₂(g).If the partial pressure of ammonia is 1.60 × 10^-3 atm and the partial pressures of N₂ and H₂ are each 0.250 atm at equilibrium,what is the value for K_c at 400°C for the forward reaction?

Accepted Answer

The answer of The decomposition of ammonia is: 2 NH₃(g)⇌...

Question 6

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO₂(g)+ O₂(g)⇌ 2 SO₃(g). If initial concentrations are [SO₂] = 3.60 M,[O₂] = 0.45 M,and [SO₃] = 5.40 M,the system is

Accepted Answer

The answer of The equilibrium constant is equal to 5.00...

Question 7

At some temperature,a 4.0 L flask is found to contain 10.0 mol of CO₂,8.0 mol of C,and 10.0 mol of CO,at equilibrium.What is the value of the equilibrium constant,K_c,for this reaction?

Accepted Answer

The answer of At some temperature,a 4.0 L flask is...

Question 8

For which one of the following reactions will K_c = K_p?

Accepted Answer

For Kc to equal Kp, the change in the number of moles of gas (Δn) must be zero. In reaction B, Δn = 1 - 1 = 0.

Question 9

Picture (1)represents an equilibrium mixture of solid CaCOS1U1B13S1U1B0,solid CaO,and gaseous COS1U1B12S1U1B0,obtained as a result of the endothermic decomposition of CaCOS1U1B13S1U1B0. 
-Which picture (2)-(4)represents the equilibrium mixture when a catalyst is added?

Accepted Answer

The answer of Picture (1)represents an equilibrium mixture of solid...

Question 10

Write the equilibrium equation for the reverse reaction: 4 CH₄ (g)+ 6 O₂ (g)⇌ 4 CO (g)+ 8 H₂O (g)

Accepted Answer

The answer of Write the equilibrium equation for the reverse...

Question 11

Which equilibrium below is homogeneous?

Accepted Answer

A homogeneous equilibrium involves reactants and products in the same phase. In option D, all substances are gases, making it a homogeneous equilibrium.

Question 12

Picture (1)represents an equilibrium mixture of solid CaCOS1U1B13S1U1B0,solid CaO,and gaseous COS1U1B12S1U1B0,obtained as a result of the endothermic decomposition of CaCOS1U1B13S1U1B0. 
-Which picture (2)-(4)represents the equilibrium mixture at a higher temperature?

Accepted Answer

Picture (4) likely represents the equilibrium mixture at a higher temperature if it shows an increased concentration of products for an endothermic reaction or decreased concentration of products for an exothermic reaction, according to Le Chatelier's principle. This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change. For an endothermic reaction, increasing the temperature shifts the equilibrium to the right (producing more products), while for an exothermic reaction, it shifts the equilibrium to the left (producing more reactants).

Question 13

Write the equilibrium equation for the forward reaction: 4 CH₄ (g)+ 6 O₂ (g)⇌ 4 CO (g)+ 8 H₂O (g)

Accepted Answer

The answer of Write the equilibrium equation for the forward...

Question 14

Picture (1)represents an equilibrium mixture of solid CaCOS1U1B13S1U1B0,solid CaO,and gaseous COS1U1B12S1U1B0,obtained as a result of the endothermic decomposition of CaCOS1U1B13S1U1B0. -Which picture (2)-(4)represents the equilibrium mixture after addition of four more CO₂ molecules?

Accepted Answer

The answer of Picture (1)represents an equilibrium mixture of solid...

Question 15

K_c is 1.67 × 10²⁰ at 25°C for the formation of iron(III)oxalate complex ion: Fe³⁺(aq)+ 3 C₂O₄^2-(aq)⇌ [Fe(C₂O₄)₃]^3-(aq). If 0.0400 M Fe³⁺ is initially mixed with 1.00 M oxalate ion,what is the concentration of Fe³⁺ ion at equilibrium?

Accepted Answer

The equilibrium constant Kc is very large, indicating the reaction strongly favors the formation of the complex ion. Therefore, almost all Fe3+ will be converted to the complex ion, leaving a very small concentration of Fe3+ at equilibrium.

Question 16

If K_c = 0.600,and K_p = 359 for a hypothetical reaction,which of the equations below could represent the reaction at 25°C?

Accepted Answer

The relationship between Kc and Kp is given by Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas. For Kp to be much larger than Kc, Δn should be positive. In option A, Δn = 6 - 4 = 2, which is positive.

Question 17

If K_c equals 0.110 at 25°C for the reaction: N₂O₄(g)⇌ 2 NO₂(g),what is K_c for the reaction: 6NO₂(g)⇌ 3 N₂O₄(g)?

Accepted Answer

For the reverse reaction, the equilibrium constant $K_{c}$ is the reciprocal of the original reaction. Given the stoichiometry of the reverse reaction is multiplied by 3 (from 2 N2O(g) to 6 N2O(g)), the new $K_{c}$ is the reciprocal of the original $K_{c}$ raised to the power of 3. Therefore, $K_{c} = (1/0.110)^3 = 1/(0.110)^3 = 751$.

Question 18

Picture (1)represents an equilibrium mixture of solid CaCOS1U1B13S1U1B0,solid CaO,and gaseous COS1U1B12S1U1B0,obtained as a result of the endothermic decomposition of CaCOS1U1B13S1U1B0. -For the reaction: N₂(g)+ 2 O₂(g)⇌ 2 NO₂(g),K_c = 8.3 × 10^-10 at 25°C.What is the concentration of N₂ gas at equilibrium when the concentration of NO₂ is twice the concentration of O₂ gas?

Accepted Answer

Let's assume that the initial concentration of OS1U1B12S1U1B0 is x M. Then, the initial concentration of NOS1U1B12S1U1B0 is 2x M. The initial concentration of NS1U1B12S1U1B0 is 0 M (since it is not given).

At equilibrium, let's assume that the concentration of NS1U1B12S1U1B0 is y M. Then, the concentration of OS1U1B12S1U1B0 becomes (x - 2y) M and the concentration of NOS1U1B12S1U1B0 becomes (2x + y) M.

We can now use the equilibrium constant expression to find the concentration of NS1U1B12S1U1B0:

KS1U1B1cS1U1B0 = [NOS1U1B12S1U1B0]2 / ([NS1U1B12S1U1B0][OS1U1B12S1U1B0]2)
8.3 × 10S1U1P1-10S1S1P0 = (2x + y)2 / (y(x - 2y)2)

Simplifying this expression and rearranging, we get:

y3 - 4xy2 + 4x2y - 8.3 × 10S1U1P1-10S1S1P0yx2 = 0

This is a cubic equation in y, and we can solve it using the cubic formula or numerical methods. However, in this case, the answer choices are all in some multiple of 10S1U1P19S1S1P0 M, which suggests that the problem can be solved using estimates.

Since the equilibrium constant is very small (10S1U1P1-10S1S1P0), we can assume that the concentration of NS1U1B12S1U1B0 is very small compared to the concentrations of OS1U1B12S1U1B0 and NOS1U1B12S1U1B0. This means that we can approximate:

y << x
y << 2x

With these approximations, we can simplify the cubic equation to:

- 8.3 × 10S1U1P1-10S1S1P0x2 ≈ 0

Solving for x, we get:

x ≈ √(8.3 × 10S1U1P1-10S1S1P0) ≈ 9.12 × 10S1U1P-6S1S1P0 M

Using this value of x, we can find y:

KS1U1B1cS1U1B0 = (2x + y)2 / (y(x - 2y)2)
8.3 × 10S1U1P1-10S1S1P0 ≈ (2x)2 / (y(x - 2y)2)
y(x - 2y)2 ≈ (2x)2 / 8.3 × 10S1U1P1-10S1S1P0
y(x2 - 4xy + 4y2) ≈ (2x)2 / 8.3 × 10S1U1P1-10S1S1P0
y(16x2) ≈ (2x)2 / 8.3 × 10S1U1P1-10S1S1P0
y ≈ (2x)2 / (16x2 × 8.3 × 10S1U1P1-10S1S1P0)
y ≈ 4.8 × 10S1U1P19S1S1P0 M

Therefore, the answer is D: 4.8 × 10S1U1P19S1S1P0 M.

Question 19

The decomposition of ammonia is: 2 NH₃(g)= N₂(g)+ 3 H₂(g).If K_p is 1.5 × 10³ at 400°C,what is the partial pressure of ammonia at equilibrium when N₂ is 0.40 atm and H₂ is 0.15 atm?

Accepted Answer

Using the equilibrium expression: K_p = (PH₂)3(PN₂) / (PNH₃)2 Substituting the values, we get: 1.5 × 10³ = (0.15)3(0.40) / (PNH₃)2 PNH₃ = 9.5 × 10^-4 atm

Question 20

Cyclohexane (C₆H₁₂)undergoes a molecular rearrangement in the presence of AlCl₃ to form methylcyclopentane (MCP)according to the equation: C₆H₁₂ ⇌ MCP If K_c = 0.143 at 25°C for this reaction,predict the direction in which the system will shift if the initial concentrations of C₆H₁₂ and MCP are 0.800 M and 0.400 M,respectively.The system

Accepted Answer

Since Kc is less than 1, the reaction favors the reactant side. Therefore, the system will shift left in order to reach equilibrium, resulting in an increase in the concentration of cyclohexane and a decrease in the concentration of methylcyclopentane.

Quiz 14: Chemical Equilibrium

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture when more solid CaO is added?

Nitric oxide reacts with oxygen to form nitrogen dioxide: 2 NO(g) + O₂(g) ⇌ 2 NO₂(g) What is K_c for the forward reaction if the equilibrium concentration of NO is 0.200 M,O₂ is 0.100 M,and NO₂ is 0.200 M at 25°C?

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture when more solid CaCO₃ is added?

The equilibrium constant,K_p,equals 3.40 at 25°C for the isomerization reaction: cis-2-butene ⇌ trans-2-butene. If a flask initially contains 3.00 atm of each gas,in what direction will the system shift to reach equilibrium?

The decomposition of ammonia is: 2 NH₃(g) ⇌ N₂(g) + 3 H₂(g) .If the partial pressure of ammonia is 1.60 × 10^-3 atm and the partial pressures of N₂ and H₂ are each 0.250 atm at equilibrium,what is the value for K_c at 400°C for the forward reaction?

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) . If initial concentrations are [SO₂] = 3.60 M,[O₂] = 0.45 M,and [SO₃] = 5.40 M,the system is

At some temperature,a 4.0 L flask is found to contain 10.0 mol of CO₂,8.0 mol of C,and 10.0 mol of CO,at equilibrium.What is the value of the equilibrium constant,K_c,for this reaction?

For which one of the following reactions will K_c = K_p?

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture when a catalyst is added?

Write the equilibrium equation for the reverse reaction: 4 CH₄ (g) + 6 O₂ (g) ⇌ 4 CO (g) + 8 H₂O (g)

Which equilibrium below is homogeneous?

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture at a higher temperature?

Write the equilibrium equation for the forward reaction: 4 CH₄ (g) + 6 O₂ (g) ⇌ 4 CO (g) + 8 H₂O (g)

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture after addition of four more CO₂ molecules?

K_c is 1.67 × 10²⁰ at 25°C for the formation of iron(III) oxalate complex ion: Fe³⁺(aq) + 3 C₂O₄^2-(aq) ⇌ [Fe(C₂O₄) ₃]^3-(aq) . If 0.0400 M Fe³⁺ is initially mixed with 1.00 M oxalate ion,what is the concentration of Fe³⁺ ion at equilibrium?

If K_c = 0.600,and K_p = 359 for a hypothetical reaction,which of the equations below could represent the reaction at 25°C?

If K_c equals 0.110 at 25°C for the reaction: N₂O₄(g) ⇌ 2 NO₂(g) ,what is K_c for the reaction: 6NO₂(g) ⇌ 3 N₂O₄(g) ?

The decomposition of ammonia is: 2 NH₃(g) = N₂(g) + 3 H₂(g) .If K_p is 1.5 × 10³ at 400°C,what is the partial pressure of ammonia at equilibrium when N₂ is 0.40 atm and H₂ is 0.15 atm?

Quiz 14: Chemical Equilibrium

Picture (1) represents an equilibrium mixture of solid CaCO3,solid CaO,and gaseous CO2,obtained as a result of the endothermic decomposition of CaCO3. -Which picture (2) -(4) represents the equilibrium mixture when more solid CaO is added?

Nitric oxide reacts with oxygen to form nitrogen dioxide: 2 NO(g) + O2(g) ⇌ 2 NO2(g) What is Kc for the forward reaction if the equilibrium concentration of NO is 0.200 M,O2 is 0.100 M,and NO2 is 0.200 M at 25°C?

Picture (1) represents an equilibrium mixture of solid CaCO3,solid CaO,and gaseous CO2,obtained as a result of the endothermic decomposition of CaCO3. -Which picture (2) -(4) represents the equilibrium mixture when more solid CaCO3 is added?

The equilibrium constant,Kp,equals 3.40 at 25°C for the isomerization reaction: cis-2-butene ⇌ trans-2-butene. If a flask initially contains 3.00 atm of each gas,in what direction will the system shift to reach equilibrium?

The decomposition of ammonia is: 2 NH3(g) ⇌ N2(g) + 3 H2(g) .If the partial pressure of ammonia is 1.60 × 10-3 atm and the partial pressures of N2 and H2 are each 0.250 atm at equilibrium,what is the value for Kc at 400°C for the forward reaction?

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO2(g) + O2(g) ⇌ 2 SO3(g) . If initial concentrations are [SO2] = 3.60 M,[O2] = 0.45 M,and [SO3] = 5.40 M,the system is

At some temperature,a 4.0 L flask is found to contain 10.0 mol of CO2,8.0 mol of C,and 10.0 mol of CO,at equilibrium.What is the value of the equilibrium constant,Kc,for this reaction?

For which one of the following reactions will Kc = Kp?

Picture (1) represents an equilibrium mixture of solid CaCO3,solid CaO,and gaseous CO2,obtained as a result of the endothermic decomposition of CaCO3. -Which picture (2) -(4) represents the equilibrium mixture when a catalyst is added?

Write the equilibrium equation for the reverse reaction: 4 CH4 (g) + 6 O2 (g) ⇌ 4 CO (g) + 8 H2O (g)

Which equilibrium below is homogeneous?

Picture (1) represents an equilibrium mixture of solid CaCO3,solid CaO,and gaseous CO2,obtained as a result of the endothermic decomposition of CaCO3. -Which picture (2) -(4) represents the equilibrium mixture at a higher temperature?

Write the equilibrium equation for the forward reaction: 4 CH4 (g) + 6 O2 (g) ⇌ 4 CO (g) + 8 H2O (g)

Picture (1) represents an equilibrium mixture of solid CaCO3,solid CaO,and gaseous CO2,obtained as a result of the endothermic decomposition of CaCO3. -Which picture (2) -(4) represents the equilibrium mixture after addition of four more CO2 molecules?

Kc is 1.67 × 1020 at 25°C for the formation of iron(III) oxalate complex ion: Fe3+(aq) + 3 C2O42-(aq) ⇌ [Fe(C2O4) 3]3-(aq) . If 0.0400 M Fe3+ is initially mixed with 1.00 M oxalate ion,what is the concentration of Fe3+ ion at equilibrium?

If Kc = 0.600,and Kp = 359 for a hypothetical reaction,which of the equations below could represent the reaction at 25°C?

If Kc equals 0.110 at 25°C for the reaction: N2O4(g) ⇌ 2 NO2(g) ,what is Kc for the reaction: 6NO2(g) ⇌ 3 N2O4(g) ?

The decomposition of ammonia is: 2 NH3(g) = N2(g) + 3 H2(g) .If Kp is 1.5 × 103 at 400°C,what is the partial pressure of ammonia at equilibrium when N2 is 0.40 atm and H2 is 0.15 atm?

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture when more solid CaO is added?

Nitric oxide reacts with oxygen to form nitrogen dioxide: 2 NO(g) + O₂(g) ⇌ 2 NO₂(g) What is K_c for the forward reaction if the equilibrium concentration of NO is 0.200 M,O₂ is 0.100 M,and NO₂ is 0.200 M at 25°C?

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture when more solid CaCO₃ is added?

The equilibrium constant,K_p,equals 3.40 at 25°C for the isomerization reaction: cis-2-butene ⇌ trans-2-butene. If a flask initially contains 3.00 atm of each gas,in what direction will the system shift to reach equilibrium?

The decomposition of ammonia is: 2 NH₃(g) ⇌ N₂(g) + 3 H₂(g) .If the partial pressure of ammonia is 1.60 × 10^-3 atm and the partial pressures of N₂ and H₂ are each 0.250 atm at equilibrium,what is the value for K_c at 400°C for the forward reaction?

The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) . If initial concentrations are [SO₂] = 3.60 M,[O₂] = 0.45 M,and [SO₃] = 5.40 M,the system is

At some temperature,a 4.0 L flask is found to contain 10.0 mol of CO₂,8.0 mol of C,and 10.0 mol of CO,at equilibrium.What is the value of the equilibrium constant,K_c,for this reaction?

For which one of the following reactions will K_c = K_p?

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture when a catalyst is added?

Write the equilibrium equation for the reverse reaction: 4 CH₄ (g) + 6 O₂ (g) ⇌ 4 CO (g) + 8 H₂O (g)

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture at a higher temperature?

Write the equilibrium equation for the forward reaction: 4 CH₄ (g) + 6 O₂ (g) ⇌ 4 CO (g) + 8 H₂O (g)

Picture (1) represents an equilibrium mixture of solid CaCO₃,solid CaO,and gaseous CO₂,obtained as a result of the endothermic decomposition of CaCO₃. -Which picture (2) -(4) represents the equilibrium mixture after addition of four more CO₂ molecules?

K_c is 1.67 × 10²⁰ at 25°C for the formation of iron(III) oxalate complex ion: Fe³⁺(aq) + 3 C₂O₄^2-(aq) ⇌ [Fe(C₂O₄) ₃]^3-(aq) . If 0.0400 M Fe³⁺ is initially mixed with 1.00 M oxalate ion,what is the concentration of Fe³⁺ ion at equilibrium?

If K_c = 0.600,and K_p = 359 for a hypothetical reaction,which of the equations below could represent the reaction at 25°C?

If K_c equals 0.110 at 25°C for the reaction: N₂O₄(g) ⇌ 2 NO₂(g) ,what is K_c for the reaction: 6NO₂(g) ⇌ 3 N₂O₄(g) ?

The decomposition of ammonia is: 2 NH₃(g) = N₂(g) + 3 H₂(g) .If K_p is 1.5 × 10³ at 400°C,what is the partial pressure of ammonia at equilibrium when N₂ is 0.40 atm and H₂ is 0.15 atm?