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babunello [35]
3 years ago
7

Which of the following statements is always true? a. The rate law can be determined from the stoichiometric equation. b. The rat

e of a catalyzed reaction is independent of the concentration of the catalyst. c. The rate for a reaction depends on the concentrations of all the reactants. d. The rate constant is independent of the concentrations of the reacting species. e. Exothermic reactions have lower activation energies than endothermic reactions.
Chemistry
1 answer:
AysviL [449]3 years ago
7 0

Answer:

d. The rate constant is independent of the concentrations of the reacting species.

Explanation:

According top law of mass action,

The rate of a reaction is directly proportional to product of active concentration of the reactant each raised to the power of their orders (experimentally determined numbers).

R = k [A]^m[B]^n....

Where, k is rate constant

m and n are order

Hence, a is incorrect.

If order is equal to zero, it means that the rate does not depend on the concentration of that reactant which means that c is incorrect.

Rate constant in the expression of the rate law depends only on temperature and thus, d is correct.

Statement e is not always true.

Catalyst is the specie that alters the rate of a reaction which means that b is incorrect.

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3 years ago
Carbon tetrachloride can be produced by the following reaction: Suppose 1.20 mol of and 3.60 mol of were placed in a 1.00-L flas
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The given question is incomplete. The complete question is :

Carbon tetrachloride can be produced by the following reaction:

CS_2(g)+3Cl_2(g)\rightleftharpoons S_2Cl_2(g)+CCl_4(g)

Suppose 1.20 mol CS_2(g) of and 3.60 mol of Cl_2(g)  were placed in a 1.00-L flask at an unknown temperature. After equilibrium has been achieved, the mixture contains 0.72 mol  of CCl_4. Calculate equilibrium constant at the unknown temperature.

Answer: The equilibrium constant at unknown temperature is 0.36

Explanation:

Moles of  CS_2 = 1.20 mole

Moles of  Cl_2 = 3.60 mole

Volume of solution = 1.00  L

Initial concentration of CS_2 = \frac{moles}{volume}=\frac{1.20mol}{1L}=1.20M

Initial concentration of Cl_2 = \frac{moles}{volume}=\frac{3.60mol}{1L}=3.60M

The given balanced equilibrium reaction is,

                 CS_2(g)+3Cl_2(g)\rightleftharpoons S_2Cl_2(g)+CCl_4(g)

Initial conc.         1.20 M        3.60 M                  0                  0

At eqm. conc.     (1.20-x) M   (3.60-3x) M   (x) M        (x) M

The expression for equilibrium constant for this reaction will be,

K_c=\frac{[S_2Cl_2]\times [CCl_4]}{[Cl_2]^3[CS_2]}

Now put all the given values in this expression, we get :

K_c=\frac{(x)\times (x)}{(3.60-3x)^3\times (1.20-x)}

Given :Equilibrium concentration of CCl_4 , x = \frac{moles}{volume}=\frac{0.72mol}{1L}=0.72M

K_c=\frac{(0.72)\times (0.72)}{(3.60-3\times 0.72)^3\times (1.20-0.72)}

K_c=0.36

Thus equilibrium constant at unknown temperature is 0.36

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