For the decomposition of ammonium carbamate, NH4(NH2CO2)(s) arrow 2NH3(g) + CO2(g), Kp = 0.0596...
Question:
For the decomposition of ammonium carbamate, {eq}NH_4(NH_2CO_2)(s) \leftrightharpoons 2NH_3(g) + CO_2(g) {/eq}, {eq}K_p {/eq} = 0.0596 at a certain temperature. A solid sample of ammonium carbamate is introduced into an evacuated container, and some solid remains in the container at equilibrium. What is the total pressure in the container?
A. 0.738 atm
B. 1.17 atm
C. 0.930 atm
D. 0.391 atm
E. 0.246 atm
Gas-Phase Chemical Equilibrium:
Reversible reaction systems with gaseous species are relatively common. Each gaseous species present inside the reaction container has a certain partial pressure value, in addition to its molar concentration. This allows the reaction progress to be monitored two different ways. Specifically, the partial pressures change over time and become constant at equilibrium, just like the concentrations. Therefore an alternate equilibrium constant {eq}K_p {/eq} and its expression, is used to relate these constant pressure values.
Answer and Explanation: 1
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Answer: A
The balanced reaction equation is:
{eq}NH_4(NH_2CO_2)(s) \leftrightharpoons 2NH_3(g) + CO_2(g) {/eq}
The equilibrium constant...
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