1. (4 points) The value of K for the gaseous reaction CO + H2O CO2 + H2 is 0.1.

Question

1. (4 points)
The value of K for the gaseous reaction CO + H2O CO2 + H2 is 0.1. Which one of the following statements concerning the relative concentrations of substances must always be true at equilibrium?
a) [CO2] = [H2O]
b) [CO2] = [H2]
c) [CO][H2O] x 10 = [CO2][H2]
d) [CO2][H2] is greater than [CO][H2O]
e) [CO2][H2] is less than [CO][H2O]

If the equilibrium constant for a reaction A + B C + D is K, which of the following expressions is true of the equilibrium constant K* for the reaction C + D A + B under the same conditions?
a) K* = K
b) K* = (1/K)
c) K* = 1 - K
d) K* = 1 - (1/K)
e) K* = 1 + K

In the reaction: CO32-(aq) + H2O(l) ---> HCO3-(aq) + OH-(aq) the carbonate ion is the
a) Arrhenius Base
b) Arrhenius Acid
c) Bronsted Lowry Acid
d) Bronsted Lowry Base
e) two of the above

Explanation / Answer

1) the given reaction is

C0 + H20 ---> C02 + H2

the equilibrium constant is

K = [C02][H2] / [C0] [H20]

0.1 = [C02] [H2] / [C0] [H20]

[C0] [H20] = 10 [C02] [H2]

we can see that

[C0] H20] >> [C02] [H2]

that is

[C02] [H2] << [C0] [H20]

so

the answer is e) [C02] [H2] is less than [CO] [H20]

2)

A + B ---> C + D

now

K = [C] [D} / [A] [B]

consider the second reaction

C + D --> A + B

the equilirbium constant is given as

K` = [A ] [B] / [C] [D]

we can see that

K` = 1/ K

so

the answer is b) K` = 1 / K

3) given reaction is

C032- + H20 ---> HC03- + OH-

from the equation

we can see that

C032- accepts a Proton (H+ ) to form HC03-

So

C032- is bronsted lowry base

also

C032- dissolved in water produced OH- ions

so

C032- is also arrhenius base

So

the answer is e) two of the above

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