If $\Delta Q$ and $\Delta W$ represent the heat supplied to the system and the work done on the system respectively,then the first law of thermodynamics can be written as

If heat is added at constant volume,$6300 \ J$ of heat are required to raise the temperature of an ideal gas by $150 \ K$. If instead,heat is added at constant pressure,$8800 \ J$ are required for the same temperature change. When the temperature of the gas changes by $300 \ K$,the internal energy of the gas changes by ..... $J$.

$Assertion:$ The heat supplied to a system is always equal to the increase in its internal energy.
$Reason:$ When a system changes from one thermal equilibrium to another,some heat is absorbed by it.

If $150 \ J$ of heat is added to a system and the work done by the system is $110 \ J$,then the change in internal energy will be .......... $J$.

The first law of thermodynamics states that:

When $150 \ J$ of heat is supplied to a system,the work done by the system is $110 \ J$. The change in the internal energy of the system is ....... $J$.