Chemistry Test 98

The rate of reaction increases to 2.3 times when the temperature is raised from 300 K to 310 K. If Q is the rate constant at 300 K then the rate constant at 310 K will be equal to –

The value of ΔH for the reaction R→ P by the following graph :

A reaction rate constant is given by :
k = 1.2 × 10¹⁴  sec^–1. It means :-

For the reaction A → B, E_a = 10 kJ/mol and ΔH = 5kJ/mol. The correct potential energy diagram for the reaction can be :-

An endothermic reaction A → B have an activation energy 15 kcal/mol and the heat of the reaction is 5 kcal/mol. The activation energy of the reaction B → A is –

A + B  C + D, K_c = 5 If at some time the concentration of A, B, C and D are 1, 2, 3, 4M, then find out the direction of reaction at this time.

20% of PCl₅ is not dissociated at 300°C. The reaction is carried out in a flask of 1 litre capacity. The value of K_c would be :

For reaction 

H_2(g) + Cl_2(g) ⇌ 2HCl_(g) at 200 K if K_c is 4.0 × 10³¹ then we conclude that :-

One mole of pure ethyl alcohol was treated with one mole of pure acetic acid at 25ºC. One third of the acid changes into ester at equilibrium. The equilibrium constant for the reaction will be :

If CuSO₄.5H₂O_(s)  CuSO₄.3H₂O_(s) + 2H₂O_(g) ; K_p = 1.086 × 10^–4 atm² at 25°C. The efflorescent nature of CuSO₄.5H₂O can be noticed when vapour pressure of H₂O is :-