The heats of combustion of $C_{(s)}$,$H_{2(g)}$,and $C_{2}H_{6(g)}$ are $-x_{1}$,$-x_{2}$,and $-x_{3}$ respectively. The heat of formation of $C_{2}H_{6(g)}$ is:

Calculate the work done in $J$ when $63.50 \ g$ of $Zn$ is dissolved in an open beaker with hydrochloric acid at $300 \ K$. (Atomic mass of $Zn = 63.5 \ amu$)

For the reaction $2 Cl ( g ) \rightarrow Cl _{2}( g )$,the correct option is

The heat of combustion of sucrose $(C_{12}H_{22}O_{11})$ is $1350 \ kcal \ mol^{-1}$. How much heat (in $kcal$) will be released by the combustion of $17.1 \ g$ of sucrose (in $.5$)?

From the following data,the enthalpy of dilution of $KCl$ will be ............ $kJ$.
$KCl_{(s)} + 20H_2O \to KCl(20H_2O); \Delta H = + 15.90 \ kJ$
$KCl_{(s)} + 200H_2O \to KCl(200H_2O); \Delta H = + 18.58 \ kJ$

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 ............. $kJ \ mol^{-1}$.