Chemistry High School

Which is not relevant to systems containing a single reaction?
Group of answer choices
Fractional Conversion
Fractional Excess
Selectivity
Extent of Reaction
All of the above
None of the above

Answers

Answer 1

The group of answer choices that is not relevant to systems containing a single reaction is "Extent of Reaction."

The other options - Fractional Conversion, Fractional Excess, and Selectivity - are all relevant parameters when considering systems containing a single reaction.

- Fractional Conversion refers to the fraction or percentage of reactants that have undergone the desired reaction and been converted to products.

- Fractional Excess is the excess of one or more reactants over the stoichiometrically required amount in a reaction.

- Selectivity is a measure of how much of the desired product is formed compared to other possible products.

"Extent of Reaction" is typically used in the context of systems with multiple reactions, where it quantifies the progress or extent of each individual reaction in the system. In a system containing a single reaction, the extent of reaction is always complete (100%), so it is not a relevant parameter.

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Related Questions

Devise electrochemical cells in which the following overall reactions can occur: a) Zn(s)+Cu²+ (aq) → Cu(s)+Zn²+ (aq) b) Ce+ (aq) +Fe²+ (aq) → Ce³+ (aq) +Fe³+ (aq) c) Ag+(aq)+Cl¯(aq) → AgCl(s) d) Zn(s) +2Cl₂(g) → ZnCl₂ (aq) 2. What is the mole fraction of NaCl in a solu- tion containing 1.00 mole of solute in 1.00 kg of H₂O? 3. What is the molarity of a solution in which 1.00 × 10² g of NaOH is dissolved in 0.250 kg of H₂O? 4. What is the voltage (Ecell) of a cell com- prising a zinc half cell (zinc in ZnSO4) and a copper half cell (Cu in CuSO4)? The metal concentrations of ZnSO4 and CuSO4 are 1 and 0.01, respectively. The activ- ity coefficient for CuSO4 is 0.047 and for ZnSO4 is 0.70. 5. Calculate E for the half cell in which the reaction Cu++ (0.1 m) + 2e¯¯ = Cu(s) takes place at 25°C.

Answers

1. A galvanic cell is constructed to facilitate the reaction between zinc and copper ions by using zinc and copper electrodes immersed in their respective ion solutions.

2. The mole fraction of NaCl in a solution is determined by dividing the moles of NaCl by the total moles of solute and solvent.

Moles of NaCl = 1.00 mole

Moles of H₂O = mass of H₂O / molar mass of H₂O

Molar mass of H₂O = 18.015 g/mol

Mass of H₂O = 1.00 kg = 1000 g

Moles of H₂O = 1000 g / 18.015 g/mol

Mole fraction of NaCl = Moles of NaCl / (Moles of NaCl + Moles of H₂O)

By plugging in the values, the mole fraction of NaCl can be calculated.

3. The molarity (M) of a solution is calculated by dividing the moles of solute by the volume of the solution in liters. In this case, if 1.00 × 10² g of NaOH is dissolved in 0.250 kg of H₂O, the molarity of the solution can be calculated as follows:

Moles of NaOH = mass of NaOH / molar mass of NaOH

Molar mass of NaOH = 22.99 g/mol + 16.00 g/mol + 1.01 g/mol = 39.00 g/mol

Moles of NaOH = 1.00 × 10² g / 39.00 g/mol

Volume of the solution = mass of H₂O / density of H₂O

Density of H₂O = 1.00 g/mL = 1000 g/L

Volume of the solution = 0.250 kg / 1000 g/L

Molarity of the solution = Moles of NaOH / Volume of the solution

By plugging in the values, the molarity of the NaOH solution can be calculated.

4. To calculate the voltage (Ecell) of the given cell, the Nernst equation can be used, which is 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 balanced cell reaction, F is Faraday's constant, and Q is the reaction quotient.

In this case, the concentrations of ZnSO4 and CuSO4 are given as 1 and 0.01, respectively, and the activity coefficients for CuSO4 and ZnSO4 are given as 0.047 and 0.70, respectively.

By using the Nernst equation and

plugging in the given values, the voltage (Ecell) of the cell can be calculated.

5. The standard reduction potential (E°) of the half cell reaction Cu²+ (0.1 M) + 2e¯ = Cu(s) at 25°C can be obtained from standard reduction potential tables. By using the Nernst equation, E = E° - (RT / nF) * ln(Q), where E° is the standard reduction potential, R is the gas constant, T is the temperature in Kelvin, n is the number of electrons transferred in the balanced half cell reaction, F is Faraday's constant, and Q is the reaction quotient.

In this case, the concentration of Cu²+ is given as 0.1 M, and the temperature is 25°C.

By using the Nernst equation and plugging in the given values, the standard reduction potential (E°) for the half cell reaction can be calculated.

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