Chemical EquilibriumHard
Question
In a 5.76 L vessel, 0.5 moles of H2 gas and 0.5 moles of I2 vapours are allowed to react to form HI (g) at 447°C, then the total pressure of gases at equilibrium would be (R = 0.08 L-atm/K-mol)
Options
A.20 atm
B.10 atm
C.5 atm
D.1 atm
Solution
H2(g) + I2(g) $\rightleftharpoons$ 2HI(g)
As Δng = 0, moles of system is not changing.
$P = \frac{nRT}{V} = \frac{(0.5 + 0.5) \times 0.08 \times 720}{5.76} = 10\text{ atm}$
Create a free account to view solution
View Solution FreeMore Chemical Equilibrium Questions
In a closed container maintained at 1 atm pressure and 25o C, 2 moles of SO2(g) and 1 mole of O2(g) were allowed to reac...For the reaction: $$\text{PCl}_5(g) \rightleftharpoons \text{PCl}_3(g) + \text{Cl}_2(g)$$ which of the following conditi...Consider the following gaseous equilibrium in a closed container of volume "V" at T(K).$$P_{2}(\text{ }g) + Q_{2}(\text{...For the equilibrium SrCl2·6H2O(s) $\rightleftharpoons$SrCl2·2H2O(s) + 4H2O(g), KP = 8.1 × 10−7 atm4 at 27oC. If 1.642 L ...N2 and H2 are taken in 1 : 3 molar ratio in a closed vessel to attained the following equilibrium N2(g) + 3H2(g) ⇋...