a) Write an expression for the equilibrium constant for this reaction. 2Al(s) + 3MnSO4(39) Al2(SO4)3(g) + 3Mn(s) b) At e

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A Write An Expression For The Equilibrium Constant For This Reaction 2al S 3mnso4 39 Al2 So4 3 G 3mn S B At E 1 (94 KiB) Viewed 39 times

a) Write an expression for the equilibrium constant for this reaction. 2Al(s) + 3MnSO4(39) Al2(SO4)3(g) + 3Mn(s) b) At equilibrium, the concentration of the reactants and products for the reaction in (a) above are determined as follows: [MnSO4] = 0.35 M and [Al2(SO4)3] = 0.040 M. What is the value of the equilibrium constant (Kc)? Predict whether the products or reactants will be favoured at equilibrium. c) Given that the concentrations of the reactants and products for the reaction in (a) above at a particular time are [MnSO4] = 0.111 M and [Al2(SO4)3] = 0.119 M, determine the reaction quotient (Qc). Compare the Kc and Qc values and predict the favoured direction of the reaction. d) In ultraviolet light, methane reacts with bromine to produce an organic product (bromomethane) and hydrobromic acid, as shown by reaction below. CH4 (9) + Br₂(g) = CH₂Br (g) + HBr(g) AH = + 75 kJ/mol Explain the effects on the equilibrium of the above reaction with: i) Increasing temperature ii) Increasing pressure iii) iv) Decreasing the concentration of hydrobromic acid (HBr) Increasing the concentration of methane (CH4) Adding a catalyst V)