Chemical EquilibriumHard

Question

For the reaction NH2COONH4(s) $\rightleftharpoons$2NH3(g) + CO2(g), KP = 3.2 × 10−5 atm3. The total pressure of the gaseous products when sufficient amount of reactant is allowed to achieve equilibrium is

Options

A.0.02 atm
B.0.04 atm
C.0.06 atm
D.0.095 atm

Solution

$K_{p} = (2p)^{2}.p \Rightarrow P = \left( \frac{3.2 \times 10^{- 5}}{4} \right)^{1/4} = 0.02$

∴ Total pressure = 2P + P = 0.06 atm

Create a free account to view solution

View Solution Free
Topic: Chemical Equilibrium·Practice all Chemical Equilibrium questions

More Chemical Equilibrium Questions

Phosphorus pentachloride dissociates as follows, in a closed reaction vessel, PCl5(g) ⇋ PCl3(g) + Cl2(g) If total ...The position of equilibrium will shift in the given direction by the addition of inert gas at constant pressure in which...A gaseous mixture contains 0.30 moles of CO, 0.10 moles of H2, and 0.03 moles of H2O vapour and an unknown amount of CH4...In an evacuated rigid vessel of volume V litre, one mole of solid ammonium carbonate (NH2CONH4) is taken and the vessel ...For the reaction, A + 2B ⇋ 2C, the rate constants for the forward and the backward reactions are 1 × 10-4 and...