The heat $Q$ for a reaction at constant volume is equal to

An ideal gas expands in volume from $1 \times 10^{-3} \ m^3$ to $1 \times 10^{-2} \ m^3$ at $300 \ K$ against a constant pressure of $1 \times 10^5 \ N \ m^{-2}$. The work done is

Identify the state functions and path functions out of the following: enthalpy,entropy,heat,temperature,work,free energy.

On what factors does the enthalpy of dilution of a solution depend?

An ideal gas expands by $1.5 \ L$ against a constant external pressure of $2 \ atm$ at $298 \ K$. Calculate the work done (in $J$)?

If $5 \ mol$ of an ideal gas expands from $10 \ L$ to a volume of $100 \ L$ at $300 \ K$ under isothermal and reversible conditions,then the work done,$w$,is $-x \ J$. The value of $x$ is $ . . . . . . $. (Given $R = 8.314 \ J \ K^{-1} \ mol^{-1}$)