Chemistry Question Bank

The equilibrium constant (Kp) for the reaction PCl5(g) PCl3(g) + Cl2(g) is 16. If the volume of the container is reduced to one half its original volume, the value of Kp for the reaction at the same temperature will be

Calculate the partial pressure of carbon monoxide from the following CaCO3 (s) CaO(s) + CO2; Kp = 8 × 10–2 CO2(g) + C (s) 2CO(g) ; Kp = 2

An amount of solid NH4HS is placed in a flask already containing ammonia gas at a certain temperature and 0.50 atm. pressure. Ammonium hydrogen sulphide decomposes to yield NH3 and H2S gases in the flask. When the dec…

At the equilibrium of the reaction, N2O4 (g) 2 NO2 (g), the observed molecular weight of N2O4 is 80 g mol –1 at 350 K. The percentage of dissociation of N2O4 (g) at 350 K is

The vapour density of completely dissociated NH4Cl would be

2 mol of N2 is mixed with 6 mol of H2 in a closed vessel of one litre capacity. If 50% of N2 is converted into NH3 at equilibrium, the value of Kc for the reaction N2(g) + 3H2(g) 2NH3(g) is

In the reaction, H2 + I2 2HI. In a 2 litre flask 0.4 moles of each H2 and I2 are taken. At equilibrium 0.5 moles of HI are formed. What will be the value of equilibrium constant, Kc

4.5 moles each of hydrogen and iodine heated in a sealed ten litre vessel. At equilibrium, 3 moles of HI were found. The equilibrium constant for H2(g) + I2(g) 2 HI(g) is

In a 500 ml capacity vessel CO and Cl2 are mixed to form COCl2. At equilibrium, it contains 0.2 moles of COCl2 and 0.1 mole of each of CO and Cl2. The equilibrium constant Kc for the reaction CO + Cl2 COCl2 is

The equilibrium concentration of X, Y and YX2 are 4, 2 and 2 moles respectively for the equilibrium 2X + Y YX2. The value of Kc is

For the reaction 2SO2 + O2 2SO3, the units of Kc are

A + B C + D. If finally the concentration of A and B are both equal but at equilibrium concentration of D will be twice of that of A then what will be the equilibrium constant of reaction.

In a reaction A + B C + D, the equilibrium concentrations of A, B, C and D (in moles/litre) are 0.5, 0.8, 0.4 and 1.0 respectively. The equilibrium constant is

For the system A(g) + 2B(g) C(g),the equilibrium

On a given condition, the equilibrium concentration of HI, H2 and I2 are 0.80, 0.10 and 0.10 mole/litre. The equilibrium constant for the reaction H2 + I2 2HI will be

4 moles of A are mixed with 4 moles of B. At equilibrium for the reaction A + B C + D, 2 moles of C and D are formed. The equilibrium constant for the reaction will be

The equilibrium constant for the reaction N2(g) + O2(g) 2NO(g) at temperature T is 4×10–4. The value of Kc for the reaction NO N (g) O (g) at the same temperature is

Which of the following reaction(s) is/are in homogeneous equilibria? (a) N g 3H g 2NH g (b) CH COOC H aq H O l CH COOH aq C H OH aq (c) Fe aq SCN aq Fe SCN aq

In a homogeneous system , all the reactants and products are in the

At equilibrium the concentrations of N 3.0 10 M x , O 4.2 10 M x and NO 2.8 10 M x in a sealed vessel at 800K. What will be Kc for the reaction, N g O g 2NO g ?

The following concentrations were obtained for the formation of NH3 from N2 and H2 at equilibrium at 500 K. N 1.5 10 M. x H 3.0 10 M x and NH 1.2 10 M. x Calculate the equilibrium constant. (a) 1.08 10 x (…

Molar concentration of different species is indicated by enclosing these in square bracket and it is implied that these are

At a given temperature, the product of …X… of the reaction products raised to the respective stoichiometric of coefficient in the balanced chemical equation …Y… by the product of concentrations of the reactants raised…

For a reaction, H g I g 2HI g c HI g K H g I g Point out the correct statement.

The equilibrium equation is also known as the …X… because in the early days of chemistry, concentration was called …Y… Here, (X) and (Y) refer to