Question

Consider the following reaction:
C(s) + H2O(g) ⇌ CO(g) + H2 (g)

If H = 131.4 kJ/mol, predict the direction of shift in equilibrium and the yield
of H2 using Le Chatelier’s Principle if:
(i) Pressures of gases are increased
(ii) Temperature is decreased
(iii) Concentration of C (s) is increased
(iv) Volume of reaction vessel is doubled.
(v) Determine the expression of Kc for this reaction.

Answer 1

Answer on Question #57955 - Chemistry - Inorganic Chemistry

Consider the following reaction:

\mathbf {C} _ {(s)} + \mathbf {H} _ {2} \mathbf {O} _ {(g)} \rightleftharpoons \mathbf {C O} _ {(g)} + \mathbf {H} _ {2} _ {(g)}

If $\Delta \mathbf{H} = 131.4\ \mathrm{kJ/mol}$, predict the direction of shift in equilibrium and the yield of $\mathbf{H}_2$ using Le Chatelier’s Principle if:

(I) Pressures of gases are increased

(II) Temperature is decreased

(III) Concentration of C (s) is increased

(IV) Volume of reaction vessel is doubled.

(V) Determine the expression of Kc for this reaction.

(I) Pressures of gases are increased

when the pressure increases, the equilibrium shifts toward smaller volume $1\ \mathrm{V} \rightarrow 2\ \mathrm{V}$

the equilibrium shifts to the left $(\leftarrow)$

the yield of $\mathrm{H}_{2}$ are decreased

(II) Temperature is decreased

\mathbf {C} _ {(s)} + \mathbf {H} _ {2} \mathbf {O} _ {(g)} \rightleftharpoons \mathbf {C O} _ {(g)} + \mathbf {H} _ {2} _ {(g)}

endothermic reaction, $\Delta \mathrm{H} > 0$

With decreasing temperature, the equilibrium shifts to the side of the exothermic reaction

the equilibrium shifts to the left $(\leftarrow)$

the yield of $\mathrm{H}_{2}$ are decreased

(III) Concentration of C (s) is increased

It does not affect the equilibrium displacement

(IV) Volume of reaction vessel is doubled.

by increasing the volume concentration decreases

the equilibrium shifts to the left $(\leftarrow)$

the yield of $\mathrm{H}_{2}$ are decreased

(V) Determine the expression of Kc for this reaction.

$$\mathbf {K c} = \frac {\left[ \mathbf {H} _ {2 (\mathbf {g})} \right] \cdot \left[ \mathbf {C O} _ {(\mathbf {g})} \right]}{\left[ \mathbf {H} _ {2} \mathbf {O} _ {(\mathbf {g})} \right]}$$

http://www.AssignmentExpert.com/