Question 18 (10 points) Which statements are true in the following choice? Selec
ID: 877806 • Letter: Q
Question
Question 18 (10 points)
Which statements are true in the following choice? Select all that apply.
Question 18 options:
Consider the following reaction.
2SO2(g) + O2(g) -> 2SO3(g),
The expression of its Kc, the equilibrium constant using concentrations in function of its Kp, the equilibrium constant using pressures is Kc = Kp x (RT)^ 1.
Consider the following reaction.
2SO2(g) + O2(g) -> 2SO3(g),
The expression of its Kc, the equilibrium constant using concentrations in function of its Kp, the equilibrium constant using pressures is Kc = Kp / (RT)^-1.
Consider the following reaction:
Na2CO3(s) + 2HNO3(aq) <-> 2NaNO3(aq) + H2O(l) + CO2(g)
The expression of the equilibrium constant for the reaction is K = [NaNO3] ^2 x [CO2] / [HNO3]^2.
Because the reaction is a heterogeneous equilibrium, pure liquids and solids are not included in the expression of the equilibrium constant.
Consider the following reaction:
Na2CO3(s) + 2HNO3(aq) <-> 2NaNO3(aq) + H2O(l) + CO2(g)
The expression of the equilibrium constant for the reaction is K = [Na2CO3] x [HNO3]^2 / [NaNO3] ^2 x [CO2].
Because the reaction is a heterogeneous equilibrium, pure liquids and solids are included in the expression of the equilibrium constant.
Note: whenever appropriate, use the sign x for multiplication operations.
A chemical reaction can be considered as a combination of several reactions. Its equilibrium constant can be expressed as a combination of the equilibrium constants of the component reactions. For example the reaction :
Equation 1: H2(g) + CO2(g) <=> CO(g) + H2O(g) with K1 for equilibrium constant
K1 = [CO]x[H2O]) / [H2]x[CO2], can be viewed as a combination of the following reactions:
Equation 2: Co(s) + H2O(g) <=> CoO(s) + H2(g) with K2 for equilibrium constant
K2 = [H2]/[H2O] and
Equation 3: CoO(s) + CO(g) <=> Co(s) + CO2(g) with K3 for equilibrium constant
K3 = [CO2]/[CO].
Close examination of the right side of the expression of K1 shows it is made of a combination of K2 and K3. The expression of K1 in terms of K2 and K3 becomes:
K1 = (1/K2) x (1/K3)
Note: whenever appropriate, use the sign x for multiplication operations.
A chemical reaction can be considered as a combination of several reactions. Its equilibrium constant can be expressed as a combination of the equilibrium constants of the component reactions. For example the reaction :
Equation 1: H2(g) + CO2(g) <=> CO(g) + H2O(g) with K1 for equilibrium constant
K1 = [H2]x[CO2] / [CO]x[H2O]), can be viewed as a combination of the following reactions:
Equation 2: Co(s) + H2O(g) <=> CoO(s) + H2(g) with K2 for equilibrium constant
K2 = [H2]/[H2O] and
Equation 3: CoO(s) + CO(g) <=> Co(s) + CO2(g) with K3 for equilibrium constant
K3 = [CO2]/[CO].
Close examination of the right side of the expression of K1 shows it is made of a combination of K2 and K3. The expression of K1 in terms of K2 and K3 becomes:
K1 = K2 / K3
Consider the following reaction.
2SO2(g) + O2(g) -> 2SO3(g),
The expression of its Kc, the equilibrium constant using concentrations in function of its Kp, the equilibrium constant using pressures is Kc = Kp x (RT)^ 1.
Consider the following reaction.
2SO2(g) + O2(g) -> 2SO3(g),
The expression of its Kc, the equilibrium constant using concentrations in function of its Kp, the equilibrium constant using pressures is Kc = Kp / (RT)^-1.
Consider the following reaction:
Na2CO3(s) + 2HNO3(aq) <-> 2NaNO3(aq) + H2O(l) + CO2(g)
The expression of the equilibrium constant for the reaction is K = [NaNO3] ^2 x [CO2] / [HNO3]^2.
Because the reaction is a heterogeneous equilibrium, pure liquids and solids are not included in the expression of the equilibrium constant.
Consider the following reaction:
Na2CO3(s) + 2HNO3(aq) <-> 2NaNO3(aq) + H2O(l) + CO2(g)
The expression of the equilibrium constant for the reaction is K = [Na2CO3] x [HNO3]^2 / [NaNO3] ^2 x [CO2].
Because the reaction is a heterogeneous equilibrium, pure liquids and solids are included in the expression of the equilibrium constant.
Note: whenever appropriate, use the sign x for multiplication operations.
A chemical reaction can be considered as a combination of several reactions. Its equilibrium constant can be expressed as a combination of the equilibrium constants of the component reactions. For example the reaction :
Equation 1: H2(g) + CO2(g) <=> CO(g) + H2O(g) with K1 for equilibrium constant
K1 = [CO]x[H2O]) / [H2]x[CO2], can be viewed as a combination of the following reactions:
Equation 2: Co(s) + H2O(g) <=> CoO(s) + H2(g) with K2 for equilibrium constant
K2 = [H2]/[H2O] and
Equation 3: CoO(s) + CO(g) <=> Co(s) + CO2(g) with K3 for equilibrium constant
K3 = [CO2]/[CO].
Close examination of the right side of the expression of K1 shows it is made of a combination of K2 and K3. The expression of K1 in terms of K2 and K3 becomes:
K1 = (1/K2) x (1/K3)
Note: whenever appropriate, use the sign x for multiplication operations.
A chemical reaction can be considered as a combination of several reactions. Its equilibrium constant can be expressed as a combination of the equilibrium constants of the component reactions. For example the reaction :
Equation 1: H2(g) + CO2(g) <=> CO(g) + H2O(g) with K1 for equilibrium constant
K1 = [H2]x[CO2] / [CO]x[H2O]), can be viewed as a combination of the following reactions:
Equation 2: Co(s) + H2O(g) <=> CoO(s) + H2(g) with K2 for equilibrium constant
K2 = [H2]/[H2O] and
Equation 3: CoO(s) + CO(g) <=> Co(s) + CO2(g) with K3 for equilibrium constant
K3 = [CO2]/[CO].
Close examination of the right side of the expression of K1 shows it is made of a combination of K2 and K3. The expression of K1 in terms of K2 and K3 becomes:
K1 = K2 / K3
Explanation / Answer
1) True
2SO2(g) + O2(g) -> 2SO3(g),
The expression of its Kc, the equilibrium constant using concentrations in function of its Kp, the equilibrium constant using pressures is Kc = Kp x (RT)^ 1.
2) True
2SO2(g) + O2(g) -> 2SO3(g),
The expression of its Kc, the equilibrium constant using concentrations in function of its Kp, the equilibrium constant using pressures is Kc = Kp / (RT)^- 1.
3) True
Na2CO3(s) + 2HNO3(aq) <-> 2NaNO3(aq) + H2O(l) + CO2(g)
The expression of the equilibrium constant for the reaction is K = [NaNO3] ^2 x [CO2] / [HNO3]^2.
4) all are True
H2(g) + CO2(g) <=> CO(g) + H2O(g) with K1 for equilibrium constant
K1 = [CO]x[H2O]) / [H2]x[CO2], can be viewed as a combination of the following reactions:
Equation 2: Co(s) + H2O(g) <=> CoO(s) + H2(g) with K2 for equilibrium constant
K2 = [H2]/[H2O] and
Equation 3: CoO(s) + CO(g) <=> Co(s) + CO2(g) with K3 for equilibrium constant
K3 = [CO2]/[CO].
Close examination of the right side of the expression of K1 shows it is made of a combination of K2 and K3. The expression of K1 in terms of K2 and K3 becomes:
K1 = (1/K2) x (1/K3)
5) K1 is wrong. and K2 right , K3 ritgh. K1 = K2 / K3 is wrong
correct expression for K1 = [H2O]x[CO] / [CO2]x[H2])
Equation 1: H2(g) + CO2(g) <=> CO(g) + H2O(g) with K1 for equilibrium constant
K1 = [H2]x[CO2] / [CO]x[H2O]), can be viewed as a combination of the following reactions:
Equation 2: Co(s) + H2O(g) <=> CoO(s) + H2(g) with K2 for equilibrium constant
K2 = [H2]/[H2O] and
Equation 3: CoO(s) + CO(g) <=> Co(s) + CO2(g) with K3 for equilibrium constant
K3 = [CO2]/[CO].
Close examination of the right side of the expression of K1 shows it is made of a combination of K2 and K3. The expression of K1 in terms of K2 and K3 becomes:
K1 = K2 / K3
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