Chemistry Question Bank

Calculate c K for the reversible process given below if p K 167 and T = 800ºC CaCO (s) CaO(s) CO (g)

For which one of the following reactions p c K K ? (a) PCl PCl Cl (b) N O 2NO (c) N 3H 2NH (d) 2SO 2SO O

Kc for the reaction N2 (g) + O2 (g) 2 NO (g) at 300 K is 4.0 × 10–6. Kp for the above reaction will be (R = 2 cal mol–1 K–1)

For reaction PCl3 (g) + Cl2 (g) PCl5 (g), the value of Kc at 250ºC is 26. The value of Kp at this temperature will be :

If Kp for a reaction A (g) + 2 B (g) 3 C (g) + D (g) is 0.05 atm at 1000 K. Its Kc in terms of R will be

In the above reaction one mole each of the acetic acid and alcohol are heated in the presence of little conc. H2SO4. On equilibrium being attained

When 3 moles of ethyl alcohol are mixed with 3 moles of acetic acid, 2 moles of ester are formed at equilibrium according to the equation CH3COOH + C2H5OH CH3COOC2H5 + H2O The value of the equilibrium constant for the…

1.1 mole of A is mixed with 2.2 mole of B and the mixture is kept in a one-litre flask till the equilibrium, A + 2B 2C + D is reached. At equilibrium 0.2 mol of C is formed. The equilibrium constant of the above react…

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

3.2 moles of hydrogen iodide were heated in a sealed bulb at 444°C till the equilibrium state was reached. Its degree of dissociation at this temperature was found to be 22%. The number of moles of hydrogen iodide pre…

Pure ammonia is placed in a vessel at temperature where its dissociation (α) is appreciable. At equilibrium

At a certain temp. 2HI H2 + I2 Only 50% HI is dissociated at equilibrium. The equilibrium constant is

One mole of N2O4(g) at 100 K is kept in a closed container at 1.0 atm pressure. It is heated to 400 K, where 30% by mass of N2O4(g) decomposes of NO2(g). The resultant pressure will be

15 moles of H2 and 5.2 moles of I2 are mixed and allowed to attain equilibrium at 500ºC. At equilibrium, the HI is found to be 10 moles. The equilibrium constant for the formation of HI is.

XY2 dissociates as : XY (g) XY(g) Y(g) Initial pressure of XY2 is 600 mm Hg. The total pressure at equilibrium is 800 mm Hg. Assuming volume of system to remain constant, the value of Kp is

5 moles of SO2 and 5 moles of O2 are allowed to react to form SO3 in a closed vessel. At the equilibrium stage 60% of SO2 is used up. The total number of moles of SO2, O2 and SO3 in the vessel now is

0.6 mole of NH3 in a reaction vessel of 2dm3 capacity was brought to equilibrium. The vessel was then found to contain 0.15 mole of H2 formed by the reaction 2NH3(g) N2(g) + 3H2(g) Which of the following statements i…

A mixture of 0.3 mole of H2 and 0.3 mole of I2 is allowed to react in a 10 litre evacuated flask at 500ºC. The reaction is H I 2HI , the K is found to be 64. The amount of unreacted 2I at equilibrium is

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