Calculate the $PV$ type of work for the following reaction at $1 \ bar$ pressure. $C_3H_{6(g)} (150 \ mL) + HCl_{(g)} (150 \ mL) \longrightarrow C_3H_7Cl_{(g)} (150 \ mL)$ (in $J$)

When an ideal gas expands isothermally from $5 \ m^3$ to $10 \ m^3$ at $25 \ ^{\circ}C$ against a constant pressure of $10^7 \ N \cdot m^{-2}$,then the work done on the gas is (in $MJ$)

During an isothermal expansion of an ideal gas,its:

One mole of an ideal gas at $300 \ K$ and $20 \ atm$ expands to $2 \ atm$ under isothermal and reversible conditions. The work done by the gas is $-x \ kJ \ mol^{-1}$. The value of $x$ is $(R = 8.3 \ J \ K^{-1} \ mol^{-1})$

What will be the work done on an ideal gas enclosed in a cylinder,when it is compressed by a constant external pressure,$p_{ext}$ in a single step as shown in the figure? Explain graphically.

Prove that the change in enthalpy of a system in which a chemical reaction occurs is equal to the heat gained by the system at constant pressure.