Pls solve the no 2 no sum with steps.

$$\begin{gathered} 2. The enthalpy change for a reaction \\ C{H}_4\left(g\right)+C{l}_2\left(g\right)\to C{H}_{3}Cl\left(g\right)+HCl\left(g\right) \\ is -115kJ mo{l}^{-1} \end{gathered}$$
How much heat is evolved/absorbed during the formation of 2.525 kg of ${\mathrm{CH}}_3\mathrm{Cl}$ by this reaction?How many moles of  Cl₂ is consumed?

Dear Student,

From the given data, we can see that 115 kJ  of heat is produced when 1 mol of CH₃Cl is formed, since the enthalpy change is negative.

Now, the number of moles of CH₃Cl that are present in 2.525 kg are:
$$\begin{gathered} Molar mass of C{H}_{3}Cl = 12 + 3x1 + 35.5=50.5 g mo{l}^{-1} \\ Given mass = 2.525 kg = 2525 g \\ Number of moles = \frac{Given mass}{Molar mass}=\frac{2525}{50.5}=50 mol \\ Now, 1 mol produces 115 kJ energy \\ so, 50 mol produces 50 x 115 = 5750 kJ \end{gathered}$$


From the reaction, we can see that 1 mol of Cl₂ is required to produce 1 mol of CH₃Cl
So, 50 mol of Cl₂ is consumed to produce 50 mol of CH₃Cl.


Hope it helps.

Regards