Chemistry Question Bank

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

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

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

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…

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

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

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.

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

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

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

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…

The vapour density of completely dissociated NH4Cl would be

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

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…

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

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

For the homogeneous reaction 4 NH3 + 5 O2 4 NO + 6 H2O the equilibrium constant Kc has the units of

In the gas phase reaction C2H4 + H2 C2H6, the equilibrium constant can be expressed in units of :

In an exothermic reaction, a 10oC rise in temperature will

For the system A (g) + 2 B (g) C (g) the equilibrium concentrations are A = 0.06 mol L–1 B = 0.12 mol L–1 C = 0.216 mol L–1. The Keq for the reaction is

The decomposition of N2O4 to NO2 is carried out at 280º C in chloroform. When equilibrium is reached 0.2 mol of N2O4 and 2 × 10–3mol of NO2 are present in 2 litre solution. The equilibrium constant for the reaction N2…

Two moles of HI were heated in a sealed tube at 440ºC till the equilibrium was reached. HI was found to be 22% decomposed. The equilibrium constant for dissociation is

56 g of N2 and 6g H2 were kept at 400ºC in l litre vessel. The equilibrium mixture contained 27.54g of NH3. The approximate value of Kc for the above reaction in mol-2 lit2 is

One mole of SO3 was placed in a vessel of 1 litre capacity at a certain temperature when the following equilibrium was established 2 SO3 2 SO2 + O2 At equilibrium, 0.6 moles of SO2 were formed. The equilibrium consta…

4 moles of A are mixed with 4 moles of B when 2 moles of C are formed at equilibrium according to the reaction A + B C + D The value of the equilibrium constant is