The variation of equilibrium constant with temperature is given below:
Temperature: T₁=25°C, T₂=100°C
Equilibrium Constant: K₁=10, K₂=100
The value of ∆H°, ∆G° at T₁ and ∆G° at T₂ (in kJmol⁻¹) respectively, are close to
[Use R=8.314JK⁻¹mol⁻¹]

The standard enthalpy of combustion at 25°C of hydrogen, cyclohexene (C₆H₁₀) and cyclohexane (C₆H₁₂) are –241, –3800 and –3920 kJ mol–1 respectively. Calculate the standard enthalpy of hydrogenation of cyclohexene.

HCP crystal is made of A ions and B ions are arranged in 2/3rd of octahedral voids. The simplest formula of compound is :-

Enthalpy of neutralisation of CH₃COOH by NaOH is – 50.6 kJ/mol and the heat of neutralisation of a strong acid with NaOH is – 55.9 kJ/mol. The value of ΔH for the ionisation of CH₃COOH is :

Kindly Consider following table–

<!-- [if !supportLists]-->(i)    <!--[endif]-->The correct match is–

 

 

  

Which of the following is a carbonate ore ?