100 mL of H_{2(g)} and 100 mL of Cl_{2(g)} | vedclass

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(A) The balanced chemical equation is: $H_{2(g)} + Cl_{2(g)} \longrightarrow 2 HCl_{(g)}$.According to Avogadro's Law,at constant temperature and pres

Vedclass · Accepted Answer

$0 \ J$

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(A) The balanced chemical equation is: $H_{2(g)} + Cl_{2(g)} \longrightarrow 2 HCl_{(g)}$.According to Avogadro's Law,at constant temperature and pressure,the volume of gases is proportional to the number of moles.Initial volume of reactants: $V_1 = 100 \ mL (H_2) + 100 \ mL (Cl_2) = 200 \ mL$.Final volume of products: $V_2 = 200 \ mL (HCl)$.Change in volume: $\Delta V = V_2 - V_1 = 200 \ mL - 200 \ mL = 0 \ mL = 0 \ dm^3$.Work done $(W)$ is given by: $W = -P_{ext} \Delta V$.Since $\Delta V = 0$,$W = -1 \ bar 	imes 0 \ dm^3 = 0 \ J$.

$100 \ mL$ of $H_{2(g)}$ and $100 \ mL$ of $Cl_{2(g)}$ were allowed to react at $1 \ bar$ pressure as: $H_{2(g)} + Cl_{2(g)} \longrightarrow 2 HCl_{(g)}$. What will be the $PV$ type of work done during the reaction?

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