In: Chemistry
HCN dissociates into CN- and protons.
A) What is the equilibrium constant at T=298.15 K?
B) At what pH will the reaction move to the left if the solution contains 0.1 M HCN?
A) Since we know an equillibrium constant is related to the standard Gibbs free energy change for the reaction.
G = -RTlnK
finding G for HCN is equal to +124.7 KJ/mol
lnK = 124.7 / - 8.314 x 298.15
lnK = 124.7 / - 2478.8191
lnk = - 0.05030
K = e(-0.05030)
= 0.951
B) HCN H+ + CN-
At 0.1M HCN pH = 1 from pH table we get know that if H+ ions concentration increases then pH decreases here in this concerned can say reaction will get in forward direction. and if pH will be greater than 1 then reaction will move left in direction.