The enthalpies of the elements in their standard states are assumed to be

What happens when methane undergoes combustion in systems $A$ and $B$ respectively?

System $A$	System $B$
Temperature rise	Temperature remains same

For an exothermic reaction,

$1 \ mol$ of an ideal gas is allowed to expand isothermally and reversibly from $1 \ L$ to $5 \ L$ at $300 \ K$. The change in enthalpy (in $kJ$) is $(R = 8.3 \ J \ K^{-1} \ mol^{-1})$.

Extensive properties depend on the quantity of matter,while intensive properties do not. Classify the following properties as extensive or intensive:
Mass,internal energy,pressure,heat capacity,molar heat capacity,density,mole fraction,specific heat,temperature,and molarity.

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 $(R = 8.3 \ J \ K^{-1} \ mol^{-1})$