One mole of a diatomic gas is heated at constant pressure starting at $ 27^{\circ}C $. How much energy must be added to the gas as heat to double its volume?

In an isobaric process of an ideal gas,the ratio of work done by the system to the heat supplied $\left(\frac{W}{Q}\right)$ is

$A$ certain amount of heat energy is supplied to a monoatomic ideal gas which expands at constant pressure. What fraction of the heat energy is converted into work?

In a reversible isochoric change,

In an isobaric process,the work done by a diatomic gas is $10 \ J$. The heat given to the gas will be (in $J$):

When $1 \, mol$ of nitrogen gas is heated at constant pressure at room temperature,it is supplied with $1163.4 \, J$ of energy. The increase in temperature is ....... $K$ $(R = 8.31 \, J \, mol^{-1} \, K^{-1})$.