A system absorbs `10 kJ` of heat at constant volume and its temperature rises from `27^(@)C` to `37^(@)C`. The `DeltaE` of reaction is

One mole of a gas absorbs 500J of heat at constant volume. If its temperature is raised from 25^(@)C to 35^(@)C , the q,W and Delta E are

A system absorbs 100J of heat at constant volume and its temperature raises from 300K to 320K. Calculate the change in internal energy.

The rate constant is doubled when temperature increases from 27^(@)C to 37^(@)C . Activation energy in kJ is

One mole of a gas absorbs 200 J of heat at constant volume. Its temperature rises from 298 K to 308 K. The change in internal energy is :-

140 grams of nitrogen absorbs 60 calories of heat without change in volume. If the temperature increases from 27^(@)C to 30^(@)C while doing so then what is the value of molar heat capacity ?

A system absorbs 300cal of heat , its volume doubles and temperature rises from 273 to 298 k , the work done on the surrounding is 200 cal . Delta E for the above reaction is :

When 0.1 mol of a gas absorbs 41.75 J of heat at constant volume, the rise in temperature occurs equal to 20^(@)C . The gas must be

A substance of mass 1cdot5 kg absorbs 45 kcal of heat energy. If its temperature rises from 28^(@)C" to "38^(@)C , find its specific heat capacity.