In an experiment starting with 1 mole `C_2H_5OH` 1 mole `CH_3COOH` and 1 mole of water, the equilibrium mixture on analysis shows that `54.3%` of the acid is esterified. Calculate `K_c`.

When 1 mole of ethanol Is mixed with 1 mole of acetic acid, 0.67 mole of ethyl acetate is produced at equilibrium. Calculate K_c for the reaction.

Ethyl acetate is formed by the reaction between ethanol and acetic acid and the equilibrium is represented as: CH_(3)COOH(l)+C_(2)H_(5)OH(l)hArr CH_(3)COOC_(2)H_(5)(l)+H_(2)O(l) (1) Write the concentration ration (reaction, quotient), Q_(c) , for this reaction (note: Water is not in excess and is not a solvent in this reaction). (2) At 293K, if one starts with 1.00 mol of acetic acid and 0.18 mol of ethanol, there is 0.171 mol of ethyl acetate in the final equilibrium mixture. calculate the equilibrium constant. (3) Starting with 0.5 mol of ethanol and 1.0 mol of acetic acid and maintaining it at 293K, 0.214 mol of ethyl acetate is found after sometime. has equilibrium been reached?

One mole of H_2 , 2 moles of I_2 and 3 moles of HI are injected in a one litre of flask. What will be the concentration of H_2, I_2 and HI at equilibrium when K_c is 45.9 ?

2 moles of PCl_5 were heated at 327^@C in a 2 litre flask. It was found that 40% of PCl_5 dissociates to give PCl_3 and Cl_2 at equilibrium. Calculate the equilibrium constant for the dissociation of PCl_5 at equilibrium.

Two moles of H_(2) and three moles of I_(2) are taken in 2 dm^(3) vessel and heated. If the equilibrium mixture contains 0.8 moles of HI, calculate K_(p) and K_(c) for the reaction H_(2(g))+I_(2(g))hArr 2HI_((g))

At 700 K, CO_2 and H_2 react to form CO and H_2O . For this process K is 0.11. [fa mixture of 0.45 mole of CO_2 and 0.45 mole of H_2 is heated to 700 K, then After equilibrium is reached another 0.34 mole of CO_2 and 0.34 mole of H_2 are added to the reaction mixture. Find the composition of the mixture at the new equilibrium state. (Assume volume to be 1 dm^3 )

In a chemical reaction A + 2B overset(rightarrow)(leftarrow)2C. 2.0 moles of ‘A’. 3 moles of B and 2.0 moles of C are placed in a 2.0 L flask and the equilibrium concentration of C is 0.5 mol//L . Calculate the equilibrium constant (k) for the reaction.