Question

Compute the heat of reaction at 1000 °C = 1273 K for $\frac{1}{2}$H$_2$(g) + $\frac{1}{2}$Cl$_2$(g) $\longrightarrow$ HCl(g) Given $\Delta H^{\circ}_{298}$ = -92.312 kJ/mol and the data for $C_p$ from Table 7.1: $C_p^{\circ}$(H$_2$)/R = 3.4958 - 0.1006(10$^{-3}$)T + 2.419(10$^{-7}$)T$^2$ $C_p^{\circ}$(Cl$_2$)/R = 3.8122 + 1.2200(10$^{-3}$)T - 4.856(10$^{-7}$)T$^2$ $C_p^{\circ}$(HCl)/R = 3.3876 + 0.2176(10$^{-3}$)T + 1.860(10$^{-7}$)T$^2$

          Compute the heat of reaction at 1000 °C = 1273 K for
$\frac{1}{2}$H$_2$(g) + $\frac{1}{2}$Cl$_2$(g) $\longrightarrow$ HCl(g)

Given $\Delta H^{\circ}_{298}$ = -92.312 kJ/mol and the data for $C_p$ from Table 7.1:

$C_p^{\circ}$(H$_2$)/R = 3.4958 - 0.1006(10$^{-3}$)T + 2.419(10$^{-7}$)T$^2$
$C_p^{\circ}$(Cl$_2$)/R = 3.8122 + 1.2200(10$^{-3}$)T - 4.856(10$^{-7}$)T$^2$
$C_p^{\circ}$(HCl)/R = 3.3876 + 0.2176(10$^{-3}$)T + 1.860(10$^{-7}$)T$^2$

Compute the heat of reaction at 1000 °C = 1273 K for
(1)/(2)H2(g) + (1)/(2)Cl2(g) ⟶ HCl(g)

Given Δ H^∘298 = -92.312 kJ/mol and the data for Cp from Table 7.1:

Cp^∘(H2)/R = 3.4958 - 0.1006(10^-3)T + 2.419(10^-7)T^2
Cp^∘(Cl2)/R = 3.8122 + 1.2200(10^-3)T - 4.856(10^-7)T^2
Cp^∘(HCl)/R = 3.3876 + 0.2176(10^-3)T + 1.860(10^-7)T^2

Added by Gregorio G.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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Solved by Expert Snehal J

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Compute the heat of reaction at 1000Â°C = 1273 K for Hg + Cl2(g) â†’ HCl(g) Given Î”HÂ°298 = -92.312 kJ/mol and the data for C, from Table 7.1: C(H)/R = 3.4958 - 0.1006(10^-3T) + 2.419(10^-7T^2) C(Cl)/R = 3.8122 + 1.2200(10^3T) + 4.856(10^7T^2) C(HCl)/R = 3.3876 + 0.2176(10^-3T) + 1.860(10^-7T^2)