At $27 \, ^oC$,one mole of an ideal gas is compressed isothermally and reversibly from a pressure of $2 \ atm$ to $10 \ atm$. The values of $\Delta E$ and $q$ are $(R = 2 \ cal \ K^{-1} \ mol^{-1})$:

Consider the reaction at $300 \ K$: $H_{2(g)} + Cl_{2(g)} \to 2HCl_{(g)}$; $\Delta H^o = -185 \ kJ$. If $2 \ mole$ of $H_2$ completely react with $2 \ mole$ of $Cl_2$ to form $HCl$,what is $\Delta U^o$ for this reaction in $kJ$?

$18 \ g$ glucose is completely combusted in a bomb calorimeter of heat capacity $1400 \ kJ/K$. The temperature changes from $27 \ ^\circ C$ to $27.2 \ ^\circ C$. Calculate the magnitude of the standard enthalpy of combustion of glucose in $kJ/mol$. $[R = 8.314 \ J/mol-K]$

An ideal gas undergoes a cyclic process as shown in the figure.
$\Delta U_{BC} = -5 \ kJ \ mol^{-1}$,$q_{AB} = 2 \ kJ \ mol^{-1}$
$\Delta W_{AB} = -5 \ kJ \ mol^{-1}$,$W_{CA} = 3 \ kJ \ mol^{-1}$
Heat absorbed by the system during process $CA$ is......$kJ \ mol^{-1}$

The oxidising power of chlorine in an aqueous solution can be determined by the parameters indicated below:
$\frac{1}{2} Cl_{2(g)} \xrightarrow{\frac{1}{2} \Delta_{diss} H^{\Theta}} Cl_{(g)} \xrightarrow{\Delta_{eg} H^{\Theta}} Cl^{-}_{(g)} \xrightarrow{\Delta_{Hyd} H^{\Theta}} Cl^{-}_{(aq)}$
(Using the data: $\Delta_{diss} H_{Cl_2}^{\Theta} = 240 \ kJ \ mol^{-1}$, $\Delta_{eg} H_{Cl}^{\Theta} = -349 \ kJ \ mol^{-1}$, $\Delta_{Hyd} H_{Cl}^{\Theta} = -381 \ kJ \ mol^{-1}$), the total enthalpy change $\Delta H$ will be ............. $kJ \ mol^{-1}$.

The heat evolved in the combustion of methane is given by the following equation: $CH_{4(g)} + 2O_{2(g)} \to CO_{2(g)} + 2H_2O_{(l)}$; $\Delta H = -890.3 \ kJ$. How many grams of methane would be required to produce $445.15 \ kJ$ of heat of combustion?