Chemical EquilibriumHard
Question
ΔfGo for the formation of HI(g) from its gaseous elements is – 2.303 kcal/mol at 500 K. When the partial pressure of HI is 10 atm and of I2(g) is 0.001 atm, then what must be the partial pressure of hydrogen be at this temperature to reduce the magnitude of ΔG for the reaction to zero?
Options
A.1000 atm
B.10000 atm
C.100 atm
D.31.63 atm
Solution
$\Delta G^{o} = - 2.303RT.\ln K_{eq}$
$\Rightarrow - 2.303 \times 10^{3} = - 2.303 \times 2 \times 500 \times \ln K_{eq} $$${\therefore K_{eq} = 10 }{\text{Now, }K_{eq} = \frac{P_{HI}}{P_{H_{2}}^{1/2} \times P_{I_{2}}^{1/2}} \Rightarrow \frac{10}{P_{H_{2}}^{1/2} \times (0.001)^{1/2}}}$$
$\therefore P_{H_{2}} = 1000\text{ atm}$
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