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Which has the smallest entropy?
C (diamond)
Which statement is correct?
when Q = K then triangleG = 0
The most probable state is the one with the ________.
largest number of possible arrangements
Which substances are included in the equilibrium constant expression, Kc?
only gases and dissolved substances
Which, if any, of the following processes is spontaneous under the specified conditions?
CO2(s) → CO2(g) at 0*C, 1 atm pressure
HI decomposes into its elements according to second-order kinetics. How long will it take for the concentration to decrease to 1.25 M from an initial concentration of 2.25 M? The rate constant, k, equals 1.6 × 10−3 M−1hr−1.
2 HI(g) → H2(g) + I2(g)
2.2 × 10² hours
A substance, A, decomposes according to zero-order kinetics from an initial concentration of 1.90 M to 0.420 M in 85.2 seconds. What is the value of the rate constant, k?
1.74 × 10−2 M∙s−1
HI decomposes into its elements according to second-order kinetics. What concentration of HI remains from an initial concentration of 2.30 M after 4.5 hours? The rate constant, k, equals 1.6 × 10−3 M−1s−1.
2 HI(g) → H2(g) + I2(g)
2.26 M
Which expression best defines the rate of the reaction with respect to CO2, given the following reaction?
C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)
What is the rate of change of H2O if the rate of change of CO2 is 0.600 M/s?
C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g)
0.800 M/s
What are the units for the rate constant, k, for a first-order reaction?
s−1
Radioactive decay follows first-order kinetics. If sodium-24 has a half-life of 14.96 hours, what is its rate constant, k?
4.63 × 10−2 hr−1
Which equation shows the integrated rate law for a substance that reacts according to second-order kinetics?
The reaction of NO and O3 reacts with second-order kinetics. If it takes 94 seconds for the concentration of NO to go from 3.00 M to 1.25 M, what is the rate constant, k?
NO(g) + O3(g) → NO2(g) + O2(g)
4.96 × 10-3 M−1∙s−1
A substance, Z, with an initial concentration of 1.75 M follows second-order kinetics and decays with a half-life of 6.8 minutes. What is the value of the rate constant, k?
8.4 × 10−2 M−1∙min−1
The rate law expresses the relationship between the concentrations of reactants and the rate of reaction.
Given the rate law, rate = k[A]2[B]2, the rate will increase by a factor of ____ when the concentration of A and B are both doubled.
Given the rate law, rate = k[A]2[B]2, the rate will increase by a factor of ____ when the concentration of A and B are both doubled.
16
A reaction has the general rate law: rate = k[A]2[B]2. What is the order with respect to A and what is the overall order of the reaction?
Second order with respect to A; fourth order overall
At equilibrium, both the forward reaction and the reverse reaction occur simultaneously and at the same rate. Since the rates are the same, the concentrations of the reactants and products do not change.
An equilibrium constant expression can be developed, which is a mathematical expression indicating the relationship between the reactants and the products.
The equilibrium concentrations can be substituted into the equilibrium expression to determine the equilibrium constant, K. The equilibrium constant can also be denoted as “K,” “Kc,” or “Keq.”
What is the equilibrium constant, K, for the following reaction if the concentration of CO was measured to be 3.1 × 10-2 M, the concentration of O2 was measured to be 1.7 × 10-2 M, and CO2 was measured to be 1.452 × 10-1 M?
2 CO(g) + O2(g) ⇌ 2 CO2(g)
K = 1.3 × 103
At equilibrium, both the forward reaction and the reverse reaction occur simultaneously and at the same rate. Since the rates are the same, the concentrations of the reactants and products do not change.
An equilibrium constant expression can be developed, which is a mathematical expression indicating the relationship between the reactants and the products.
The equilibrium concentrations can be substituted into the equilibrium expression to determine the equilibrium constant, K. The equilibrium constant can also be denoted as “K,” “Kc,” or “Keq.”
What is the concentration of CO if the concentration of Cl2 was measured to be 0.75 M, COCl2 was measured to be 2.21 M, and the equilibrium constant, K, is 5.3?
CO(g) + Cl2(g) ⇌ COCl2(g)
[CO] = 0.56 M
