Thermodynamics - 1 - JEE MCQ

1 mole of a diatomic gas is contained in a piston. It gains 50.0 J of heat and work is done on the surrounding by the system is -100 J. Thus,

A sample containing 1.0 mole of an ideal gas is expanded isothermally and reversibly to ten time of its original volume, in two separate experiments. The expansion is carried out 300 K and at 600 K, respectively. Choose the correct option.

Change in enthalpy for reaction,
2H₂O_2(l) → 2H₂O_(l) + O_2(g)
if heat of formation of H₂O_2(l) and H₂O_(l) are −188 and −286 kJ/mol respectively, is

If ΔH is the change in enthalpy and ΔE, the change in internal energy accompanying a gaseous reaction, then

During compression of a spring the work done is 10 kJ and 2 kJ escaped to the surroundings as heat. The change in internal energy, ΔU (in kJ) is :
 

Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The enthalpy change (in kJ) for the process is

When 5 litres of a gas mixture of methane and propane is perfectly combusted at 0°C and 1 atmosphere, 16 litres of oxygen at the same temperature and pressure is consumed. The amount of heat released from this combustion in kJ (ΔH_comb. (CH₄) = 890 kJ mol⁻¹, ΔH_comb. (C₃H₈) = 2220 kJ mol⁻¹) is

Consider the following reactions:

Enthalpy of formaton of H₂O(l) 

The correct relationship between free energy change in a reaction and the corresponding equilibrium constant 
K_c  is

For silver, C_p(JK^–1 mol^–1) = 23 + 0.01 T. If the temperature (T) of 3 moles of silver is raised from 300 K to 1000 K at 1 atm pressure, the value of ΔH will be close to -