Question 1

Calculate G^ for reaction, CH _ 4(g) + H _ 2(g) C _2 H _ 6(g) (K_p = 2 10^ 17 , R = 8.314\ JK ^ -1 mol ^ -1 )

Accepted Answer

The standard Gibbs free energy change is related to the equilibrium constant by the equation: G^ = -RT K_p = -2.303 RT K_p Assuming standard temperature T = 298 K and substituting the given values: G^ = -2.303 8.314 298 (2 10^ 17 ) G^ = -5705.84 ( 2 + 17 10) G^ = -5705.84 (0.3010 + 17) G^ = -5705.84 17.3010 G^ = -98716 J mol ^ -1 G^ = -98.716 kJ mol ^ -1 Answer: -98.716 kJ mol^ -1

Question 2

Find n when 1 mol of each NH _ 3(g) and HCl _ (g) , reacts to form solid NH _4 Cl .

Accepted Answer

The balanced chemical equation for the reaction is: NH _ 3(g) + HCl _ (g) NH _4 Cl _ (s) The change in the number of moles of gaseous species, n, is given by the difference between the number of moles of gaseous products and gaseous reactants. Number of moles of gaseous products, n_P = 0 Number of moles of gaseous reactants, n_R = 1 + 1 = 2 n = n_P - n_R = 0 - 2 = -2 Answer: -2

Chemical Equilibrium — Previous Year Questions & Solutions