Chemistry Question Bank

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

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

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

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

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

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.

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

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

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

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 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

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

For the reaction C(s) CO (g) 2CO(g) The partial pressure of CO and CO are 2.0 and 4.0 atm respectively then equilibrium p K for the reaction will be (BCECE 2008)

Equimolar concentrations of H and I are heated to equilibrium in a 2 L flask. At equilibrium, the forward and the backward rate constants are found to be equal. NH N NH What percentage of initial concentration of H …

In the equilibrium 2NH N 3H , 6 moles of is taken in 10 L flask. If concentration of at equilibrium is x, then concentration of at equilibrium is (DUMET 2008)

Now, the total pressure at equilibrium, p(1 α)+pα+0.5pα = P P p = ...(2) 1+0.5α From eq (1) and eq(2), p P P P K 0.5 1 + 0.5α K P 0.5 2K P x x