The equilibrium constant K_c at 298 K for the reaction

A + B $\rightleftharpoons$ C + D

is 100. Starting with an equimolar solution with concentrations of A, B, C and D all equal to 1M, the equilibrium concentration of D is_________* 10^-2 M. (Nearest integer)

Value of K_p for the equilibrium reaction N₂O_4(g) $\stackrel{}{?}$ <!-- [if gte mso 9]><xml> </xml><![endif]--> 2NO_2(g) at 288 K is 47.9. The K_c for this reaction at same temperature is_________. (Nearest integer)

(R = 0.083 L bar K^-1 mol^-1)

If 80g of copper sulphate CuSO₄ $\cdot$ <!-- [if gte mso 9]><xml> </xml><![endif]-->5H₂O is dissolved in deionized water to make 5L of solution. The concentration of the copper sulphate solution is x × 10^-3 mol L^-1. The value of x is________.

[Atomic masses Cu : 63.54u, S : 32u, O : 16u, H : 1u]

When 5.1g of solid NH₄HS is introduced into a two litre evacuated flask at 27°C, 20% of the solid decomposes into gaseous ammonia and hydrogen sulphide. The K_p for the reaction at 27°C is x × 10^-2. The value of x is_______. (Integer answer)

[Given R = 0.082 L atm K^-1 mol^-1]