Factors Affecting Rate Constant

In a reaction, 2A → Products, the concentration of A decreases from 0.5 mol L⁻¹ to 0.4 mol L⁻¹ in 10 minutes. Calculate the rate during this interval?

A first order reaction has a rate constant 1.15 10⁻³ s⁻¹. How long will 5 g of this reactant take to reduce to 3 g?

A sample of pure PCl₅ was introduced into an evacuated vessel at 473 K. After equilibrium was attained, concentration of PCl₅ was found to be 0.5 × 10^–1 mol L^–1. If value of K_c is 8.3 × 10^–3, what are the concentrations of PCl₃ and Cl₂ at equilibrium?

Predict which of the following reaction will have appreciable concentration of reactants and products:

a)

b)

c)

What is K_c for the following equilibrium when the equilibrium concentration of each substance is: [SO₂]= 0.60 M, [O₂] = 0.82 M and [SO₃] = 1.90 M ?

2SO₂ (g) + O₂ (g) ⇌ 2SO₃ (g)

Consider a certain reaction A → Products with k = 2.0 × 10⁻² s⁻¹. Calculate the concentration of A remaining after 100 s if the initial concentration of A is 1.0 mol L⁻¹.

A sample of pure PCl₅ was introduced into an evacuated vessel at 473 K. After equilibrium was attained, concentration of PCl₅ was found to be

0.5 × 10^–1 mol L^–1. If value of K_c is 8.3 × 10^–3, what are the concentrations of PCl₃ and Cl₂ at equilibrium?

For the reaction:

2A + B → A₂B

the rate = k[A][B]² with k = 2.0 × 10⁻⁶ mol⁻² L² s⁻¹. Calculate the initial rate of the reaction when [A] = 0.1 mol L⁻¹, [B] = 0.2 mol L⁻¹. Calculate the rate of reaction after [A] is reduced to 0.06 mol L⁻¹.

What is the equilibrium concentration of each of the substances in the equilibrium when the initial concentration of ICl was 0.78 M?

Predict which of the following reaction will have appreciable concentration of reactants and products:

a)

b)

c)

Define Order and Molecularity?

The rate constant for a reaction depends upon each of the following, EXCEPT:

1. temperature

2. solvent for solutions

3. concentration of reactants

4. nature of reactants

The value of K_cfor the reaction

3 O₂ (g) 2 O₃ (g)

is 2.0 ×10^–50 at 25°C. If the equilibrium concentration of O₂ in air at 25°C is 1.6 ×10^–2, what is the concentration of O₃?

What is the equilibrium concentration of each of the substances in the equilibrium when the initial concentration of ICl was 0.78 M?

The value of K_c for the reaction

3O₂ (g) 2O₃ (g)

is 2.0 ×10^–50 at 25°C. If the equilibrium concentration of O₂ in air at 25°C is 1.6 ×10^–2, what is the concentration of O₃?

1. extent of the reaction
2. temperature of the reaction
3. initial concentration of the reactants
4. the time of completion of reaction

1. i, ii, iii
2. ii, iii, iv
3. i, ii
4. iii, iv

What is K_c for the following equilibrium when the equilibrium concentration of each substance is: [SO₂]= 0.60 M, [O₂] = 0.82 M and [SO₃] = 1.90 M ?

1. Products
2. Concentration
3. Initial amounts
4. Change in amounts
5. Reactants

What is the maximum concentration of equimolar solutions of ferrous sulphate and sodium sulphide so that when mixed in equal volumes, there is no precipitation of iron sulphide? (For iron sulphide, K_sp = 6.3 × 10^–18).

1. $e^{k/m}$
2. $k$
3. $k/m$
4. $mk$

The rate constant for a reaction depends upon each of the following, EXCEPT:

1. solvent for solutions

2. temperature

3. concentration of reactants

4. nature of reactants

Consider a certain reaction A → Products with k = 2.0 × 10⁻² s⁻¹. Calculate the concentration of A remaining after 100 s if the initial concentration of A is 1.0 mol L⁻¹.

1. $e^{k/m}$
2. $k$
3. $k/m$
4. $mk$

1. $–6\left(2.303\right)RT$
2. $+6RT$
3. $-6RT$
4. $+6\left(2.303\right)RT$

A first order reaction has a rate constant 1.15 10⁻³ s⁻¹. How long will 5 g of this reactant take to reduce to 3 g?

1. True
2. False

1. He changed the temperature of the reaction
2. He changed the concentrations of the reactants
3. He replaced $O_{2}with{F}_2$
4. He used a catalyst in the reaction

1. He replaced $O_{2}with{F}_2$
2. He used a catalyst in the reaction
3. He changed the temperature of the reaction
4. He changed the concentrations of the reactants