Question 1

Based on the balanced chemical equation shown below,determine the mass percent of Fe³⁺ in a sample of iron ore,if 22.40 mL of a 0.1000 M stannous chloride,SnCl₂(aq),solution is required to completely react with theFe³⁺ present in the ore sample.The chemical equation for the reaction is: 2 Fe³⁺(aq)+ Sn²⁺(aq)→ 2 Fe²⁺(aq)+ Sn⁴⁺(aq).

Accepted Answer

The answer of Based on the balanced chemical equation shown...

Question 2

According to the balanced equation shown below,3.00 mole of oxalic acid,H₂C₂O₄,reacts with ________ moles of permanganate,MnO₄^-. 5 H₂C₂O₄(aq)+ 2 MnO₄^-(aq)+ 6 H⁺(aq)→ 10 CO₂(g)+ Mn²⁺(aq)+ 8 H₂O(l)

Accepted Answer

According to the balanced chemical equation, 5 moles of oxalic acid react with 2 moles of permanganate. Therefore, 3.00 moles of oxalic acid would react with (3.00/5)*2 = 1.20 moles of permanganate.

Question 3

The initial concentrations of Ag⁺(aq)and Cu²⁺(aq)are both 1.0 M.What will happen to the cell voltage if 5.0 M AgNO₃ is added to the compartment containing the 1.0 M Ag⁺(aq)? The cell voltage will

Accepted Answer

The addition of 5.0 M AgNO3 to the compartment containing the 1.0 M Ag⁺(aq) will increase the concentration of Ag+ ions, which will shift the equilibrium of the half-reaction: Ag+ + e- ⇌ Ag to the left, decreasing the concentration of Ag+ ions in solution. This shift will drive the overall cell reaction to proceed in the direction favored by the reduction potential of the Cu2+/Cu half-reaction, resulting in an increase in cell voltage. Therefore, the cell voltage will increase.

Question 4

Consider the following galvanic cell. 
-What is the quantitative change in the cell voltage on increasing the ion concentration in the cathode compartment by a factor of 10?

Accepted Answer

The answer of Consider the following galvanic cell. 
-What is...

Question 5

Shown below is an electrochemical cell with anode a and cathode c.Both the anode and the cathode are inert electrodes.The liquid shown in compartment b of the cell is molten potassium chloride,KCl(l). 
-Determine whether this is a galvanic or an electrolytic cell and give the reaction occurring at the anode and the reaction occurring at the cathode.

Accepted Answer

In an electrolytic cell, an external voltage is applied to drive a non-spontaneous reaction. The anode is the site of oxidation, and the cathode is the site of reduction. In choice B, the anode reaction involves the oxidation of chloride ions (Cl-) to chlorine gas (Cl2), and the cathode reaction involves the reduction of potassium ions (K+) to potassium metal (K), which is consistent with the operations of an electrolytic cell.

Question 6

Based on the balanced chemical equation shown below,determine the molarity of a solution containing Fe²⁺(aq),if 40.00 mL of the Fe²⁺(aq)solution is required to completely react with 30.00 mL of a 0.500 M potassium bromate,KBrO₃(aq),solution.The chemical equation for the reaction is: 6 Fe²⁺(aq)+ BrO₃^-(aq)+ 6 H⁺(aq)→ 6 Fe³⁺(aq)+ Br^-(aq)+ 3 H₂O(l).

Accepted Answer

First, we need to use stoichiometry to determine the moles of KBrO3 that reacted with the Fe²⁺(aq) solution: 30.00 mL of 0.500 M KBrO3 = 0.0150 moles KBrO3 Using the balanced chemical equation, we can see that 6 moles of Fe²⁺(aq) react with 1 mole of KBrO3, so: 0.0150 moles KBrO3 * (6 moles Fe²⁺(aq) / 1 mole KBrO3) = 0.0900 moles Fe²⁺(aq) Now we can use the volume and moles of the Fe²⁺(aq) solution to determine its molarity: Molarity = moles of solute / volume of solution in liters Molarity = 0.0900 moles / 0.04000 L = 2.25 M Therefore, the correct answer is choice C, 2.25 M.

Question 7

What are the coefficients in front of NO₃^-(aq)and Mg(s)when the following redox equation is balanced in an acidic solution? ________ NO₃^-(aq)+ ________ Mg(s)→ ________ NO(g)+ ________ Mg²⁺(aq)

Accepted Answer

The answer of What are the coefficients in front of...

Question 8

-Is the cell shown above a galvanic or an electrolytic cell? What is the direction of ion flow?

Accepted Answer

The answer of 
-Is the cell shown above a galvanic...

Question 9

Consider the galvanic cell shown below. 
-What is the quantitative change in the cell voltage on increasing the ion concentration in the cathode compartment by a factor of 10?

Accepted Answer

The Nernst equation describes the effect of ion concentration on cell voltage. Increasing the ion concentration at the cathode by a factor of 10 results in an increase in cell voltage, calculated using the Nernst equation. The change in voltage can be approximated as $0.0592/n$ log(10), where $n$ is the number of electrons transferred. For a monovalent ion ($n=1$), this results in a change of approximately +0.0592 V, which is closest to +0.03 V, indicating an increase in cell voltage.

Question 10

Shown below is an electrochemical cell with anode a and cathode c.Both the anode and the cathode are inert electrodes.The liquid shown in compartment b of the cell is molten potassium chloride,KCl(l). 
-Determine the direction of electron flow and the direction of ion flow.

Accepted Answer

In a molten salt electrolyte like KCl(l), the positively charged potassium ions (K+) are attracted to the negatively charged cathode and are reduced (gain electrons) to form potassium metal. The negatively charged chloride ions (Cl-) are attracted to the positively charged anode and are oxidized (lose electrons) to form chlorine gas. Therefore, electrons flow from the anode (a) to the cathode (c) and chloride ions move towards the anode (a) while potassium ions move towards the cathode (c). Hence, option B is the correct choice.

Question 11

What are the coefficients in front of NO₃^-(aq)and Zn(s)when the following equation is balanced in a basic solution? ________ NO₃^-(aq)+ ________ Ni(s)→ ________ Ni²⁺(aq)+ ________ NO(g)

Accepted Answer

The balanced equation in a basic solution is $2 \, \text{NO}_3^- (aq) + 3 \, \text{Zn} (s) \rightarrow 2 \, \text{NO} (g) + 3 \, \text{Zn}^{2+} (aq)$. This shows that the coefficients in front of $\text{NO}_3^-$ and $\text{Zn}$ are 2 and 3, respectively.

Question 12

-Is the cell shown above a galvanic or an electrolytic cell? Which is the anode and which is the cathode?

Accepted Answer

The answer of 
-Is the cell shown above a galvanic...

Question 13

In the unbalanced equation shown below how many moles of electrons are transferred per mole of reducing agent? C₂O₄2- (aq)+ MnO₄^-(aq)→ CO₂(aq)+ Mn²⁺(aq)

Accepted Answer

In the balanced equation, we see that 2 moles of electrons are transferred per mole of reducing agent (C₂O₄2-). This is because the coefficient of the reducing agent in the balanced equation is 2. Choice B is the only option that matches this value.

Question 14

What are the coefficients in front of IO₃^-(aq)and I^-(aq)when the following equation is balanced in an acidic solution? ________ IO₃^-(aq)+ ________ I^-(aq)→ ________ I₂(aq)

Accepted Answer

In an acidic solution, the balanced equation is IO₃⁻ + 5I⁻ + 6H⁺ → 3I₂ + 3H₂O. The coefficients for IO₃⁻ and I⁻ are 1 and 5, respectively.

Question 15

Consider the galvanic cell shown below. 
-What is the quantitative change in the cell voltage on increasing the ion concentration in the anode compartment by a factor of 10?

Accepted Answer

According to the Nernst equation, an increase in ion concentration in the anode compartment would lead to a decrease in cell voltage. The change in voltage is given by ΔE = -0.0592/n log ([ion] new/[ion] old), where n is the number of electrons involved in the cell reaction. Since the ion concentration is increased by a factor of 10, we have [ion] new = 10[ion] old. Substituting this into the Nernst equation gives ΔE = -0.0592/n log(10) = -0.0592/n * 1.0 = -0.0592/n V. Since we do not know the value of n, we cannot determine the exact voltage change, but we can conclude that it will be negative. The closest answer choice is C, which corresponds to a decrease of 0.02 V.

Question 16

What are the coefficients in front of Ni(s)and O₃(g)when the following equation is balanced in a basic solution? ________ Ni(s)+ ________ O₃(g)→ ________ Ni₂O₃(s)+ ________ O₂(g)

Accepted Answer

In order to balance the equation in basic solution, we need to add OH- ions to both sides of the equation. The balanced equation is: 2Ni(s) + 3O₃(g) + 12OH-(aq) → 2Ni₂O₃(s) + 3O₂(g) + 6H2O(l) So, the coefficients in front of Ni(s) and O₃(g) are 2 and 3, respectively. Therefore, the correct answer is B.

Question 17

Based on the balanced chemical equation shown below,what volume of 0.250 M K₂S₂O₃(aq),is needed to completely react with 12.44 mL of 0.125 M KI₃(aq)? 2 S₂O₃^2-(aq)+ I₃^-(aq)→ S₄O₆^2-(aq)+ 3 I^-(aq)

Accepted Answer

The answer of Based on the balanced chemical equation shown...

Question 18

What is the molarity of a potassium triiodide solution,KI₃(aq),if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.500 M thiosulfate solution,K₂S₂O₃(aq)? The chemical equation for the reaction is: 2 S₂O₃^2-(aq)+ I₃^-(aq)→ S₄O₆^2-(aq)+ 3 I^-(aq).

Accepted Answer

The balanced equation shows that 2 moles of thiosulfate react with 1 mole of triiodide. Using the volume and molarity of thiosulfate, calculate moles of thiosulfate: 0.025 L * 0.500 M = 0.0125 moles. Thus, moles of I3- = 0.0125 / 2 = 0.00625 moles. Molarity of KI3 = 0.00625 moles / 0.030 L = 0.208 M.

Question 19

Consider the following galvanic cell. 
-What is the quantitative change in the cell voltage on increasing the ion concentration in the anode compartment by a factor of 10?

Accepted Answer

According to the Nernst equation, the cell potential is given by:
Ecell = E°cell - (RT/nF) ln(Q)
where E°cell is the standard cell potential, R is the gas constant, T is the temperature in Kelvin, n is the number of electrons transferred in the cell reaction, F is the Faraday constant, and Q is the reaction quotient.
On increasing the ion concentration in the anode compartment by a factor of 10, the reaction quotient Q would increase by a factor of 10 as well. This would result in a negative logarithmic term, which would decrease the cell potential. Since the anode compartment is where oxidation occurs and the anode is the negative electrode in this cell, the cell potential would decrease. Therefore, the correct answer is C, -0.03 V.

Question 20

The initial concentrations of Ag⁺(aq)and Cu²⁺(aq)are both 1.0 M.What will happen to the cell voltage if Cu(NO₃)₂ is added to the compartment containing the 1.0 M Cu²⁺(aq)? The cell voltage will

Accepted Answer

The answer of The initial concentrations of Ag⁺(aq)and Cu²⁺(aq)are both...

Quiz 18: Electrochemistry

According to the balanced equation shown below,3.00 mole of oxalic acid,H₂C₂O₄,reacts with ________ moles of permanganate,MnO₄^-. 5 H₂C₂O₄(aq) + 2 MnO₄^-(aq) + 6 H⁺(aq) → 10 CO₂(g) + Mn²⁺(aq) + 8 H₂O(l)

The initial concentrations of Ag⁺(aq) and Cu²⁺(aq) are both 1.0 M.What will happen to the cell voltage if 5.0 M AgNO₃ is added to the compartment containing the 1.0 M Ag⁺(aq) ? The cell voltage will

Consider the following galvanic cell. -What is the quantitative change in the cell voltage on increasing the ion concentration in the cathode compartment by a factor of 10?

What are the coefficients in front of NO₃^-(aq) and Mg(s) when the following redox equation is balanced in an acidic solution? NO₃^-(aq) + Mg(s) → NO(g) + Mg²⁺(aq)

-Is the cell shown above a galvanic or an electrolytic cell? What is the direction of ion flow?

Consider the galvanic cell shown below. -What is the quantitative change in the cell voltage on increasing the ion concentration in the cathode compartment by a factor of 10?

Shown below is an electrochemical cell with anode a and cathode c.Both the anode and the cathode are inert electrodes.The liquid shown in compartment b of the cell is molten potassium chloride,KCl(l) . -Determine the direction of electron flow and the direction of ion flow.

What are the coefficients in front of NO₃^-(aq) and Zn(s) when the following equation is balanced in a basic solution? NO₃^-(aq) + Ni(s) → Ni²⁺(aq) + NO(g)

-Is the cell shown above a galvanic or an electrolytic cell? Which is the anode and which is the cathode?

In the unbalanced equation shown below how many moles of electrons are transferred per mole of reducing agent? C₂O₄2- (aq) + MnO₄^-(aq) → CO₂(aq) + Mn²⁺(aq)

What are the coefficients in front of IO₃^-(aq) and I^-(aq) when the following equation is balanced in an acidic solution? IO₃^-(aq) + I^-(aq) → I₂(aq)

Consider the galvanic cell shown below. -What is the quantitative change in the cell voltage on increasing the ion concentration in the anode compartment by a factor of 10?

What are the coefficients in front of Ni(s) and O₃(g) when the following equation is balanced in a basic solution? Ni(s) + O₃(g) → Ni₂O₃(s) + O₂(g)

Based on the balanced chemical equation shown below,what volume of 0.250 M K₂S₂O₃(aq) ,is needed to completely react with 12.44 mL of 0.125 M KI₃(aq) ? 2 S₂O₃^2-(aq) + I₃^-(aq) → S₄O₆^2-(aq) + 3 I^-(aq)

What is the molarity of a potassium triiodide solution,KI₃(aq) ,if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.500 M thiosulfate solution,K₂S₂O₃(aq) ? The chemical equation for the reaction is: 2 S₂O₃^2-(aq) + I₃^-(aq) → S₄O₆^2-(aq) + 3 I^-(aq) .

Consider the following galvanic cell. -What is the quantitative change in the cell voltage on increasing the ion concentration in the anode compartment by a factor of 10?

The initial concentrations of Ag⁺(aq) and Cu²⁺(aq) are both 1.0 M.What will happen to the cell voltage if Cu(NO₃) ₂ is added to the compartment containing the 1.0 M Cu²⁺(aq) ? The cell voltage will

Quiz 18: Electrochemistry

According to the balanced equation shown below,3.00 mole of oxalic acid,H2C2O4,reacts with ________ moles of permanganate,MnO4-. 5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+(aq) → 10 CO2(g) + Mn2+(aq) + 8 H2O(l)

The initial concentrations of Ag+(aq) and Cu2+(aq) are both 1.0 M.What will happen to the cell voltage if 5.0 M AgNO3 is added to the compartment containing the 1.0 M Ag+(aq) ? The cell voltage will

Consider the following galvanic cell. -What is the quantitative change in the cell voltage on increasing the ion concentration in the cathode compartment by a factor of 10?

What are the coefficients in front of NO3-(aq) and Mg(s) when the following redox equation is balanced in an acidic solution? ________ NO3-(aq) + ________ Mg(s) → ________ NO(g) + ________ Mg2+(aq)

-Is the cell shown above a galvanic or an electrolytic cell? What is the direction of ion flow?

Consider the galvanic cell shown below. -What is the quantitative change in the cell voltage on increasing the ion concentration in the cathode compartment by a factor of 10?

Shown below is an electrochemical cell with anode a and cathode c.Both the anode and the cathode are inert electrodes.The liquid shown in compartment b of the cell is molten potassium chloride,KCl(l) . -Determine the direction of electron flow and the direction of ion flow.

What are the coefficients in front of NO3-(aq) and Zn(s) when the following equation is balanced in a basic solution? ________ NO3-(aq) + ________ Ni(s) → ________ Ni2+(aq) + ________ NO(g)

-Is the cell shown above a galvanic or an electrolytic cell? Which is the anode and which is the cathode?

In the unbalanced equation shown below how many moles of electrons are transferred per mole of reducing agent? C2O42- (aq) + MnO4-(aq) → CO2(aq) + Mn2+(aq)

What are the coefficients in front of IO3-(aq) and I-(aq) when the following equation is balanced in an acidic solution? ________ IO3-(aq) + ________ I-(aq) → ________ I2(aq)

Consider the galvanic cell shown below. -What is the quantitative change in the cell voltage on increasing the ion concentration in the anode compartment by a factor of 10?

What are the coefficients in front of Ni(s) and O3(g) when the following equation is balanced in a basic solution? ________ Ni(s) + ________ O3(g) → ________ Ni2O3(s) + ________ O2(g)

Based on the balanced chemical equation shown below,what volume of 0.250 M K2S2O3(aq) ,is needed to completely react with 12.44 mL of 0.125 M KI3(aq) ? 2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq)

What is the molarity of a potassium triiodide solution,KI3(aq) ,if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.500 M thiosulfate solution,K2S2O3(aq) ? The chemical equation for the reaction is: 2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq) .

Consider the following galvanic cell. -What is the quantitative change in the cell voltage on increasing the ion concentration in the anode compartment by a factor of 10?

The initial concentrations of Ag+(aq) and Cu2+(aq) are both 1.0 M.What will happen to the cell voltage if Cu(NO3) 2 is added to the compartment containing the 1.0 M Cu2+(aq) ? The cell voltage will

According to the balanced equation shown below,3.00 mole of oxalic acid,H₂C₂O₄,reacts with ________ moles of permanganate,MnO₄^-. 5 H₂C₂O₄(aq) + 2 MnO₄^-(aq) + 6 H⁺(aq) → 10 CO₂(g) + Mn²⁺(aq) + 8 H₂O(l)

The initial concentrations of Ag⁺(aq) and Cu²⁺(aq) are both 1.0 M.What will happen to the cell voltage if 5.0 M AgNO₃ is added to the compartment containing the 1.0 M Ag⁺(aq) ? The cell voltage will

What are the coefficients in front of NO₃^-(aq) and Mg(s) when the following redox equation is balanced in an acidic solution? NO₃^-(aq) + Mg(s) → NO(g) + Mg²⁺(aq)

What are the coefficients in front of NO₃^-(aq) and Zn(s) when the following equation is balanced in a basic solution? NO₃^-(aq) + Ni(s) → Ni²⁺(aq) + NO(g)

In the unbalanced equation shown below how many moles of electrons are transferred per mole of reducing agent? C₂O₄2- (aq) + MnO₄^-(aq) → CO₂(aq) + Mn²⁺(aq)

What are the coefficients in front of IO₃^-(aq) and I^-(aq) when the following equation is balanced in an acidic solution? IO₃^-(aq) + I^-(aq) → I₂(aq)

What are the coefficients in front of Ni(s) and O₃(g) when the following equation is balanced in a basic solution? Ni(s) + O₃(g) → Ni₂O₃(s) + O₂(g)

Based on the balanced chemical equation shown below,what volume of 0.250 M K₂S₂O₃(aq) ,is needed to completely react with 12.44 mL of 0.125 M KI₃(aq) ? 2 S₂O₃^2-(aq) + I₃^-(aq) → S₄O₆^2-(aq) + 3 I^-(aq)

The initial concentrations of Ag⁺(aq) and Cu²⁺(aq) are both 1.0 M.What will happen to the cell voltage if Cu(NO₃) ₂ is added to the compartment containing the 1.0 M Cu²⁺(aq) ? The cell voltage will