Calculate the heat produced in kJ when 280 g | vedclass

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(B) The chemical reaction is: $CaO_{(s)} + CO_{2(g)} \rightarrow CaCO_{3(s)}$First,calculate the standard enthalpy of reaction $(\Delta H^o_r)$:$\Delt

Vedclass · Accepted Answer

$877.55$

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(B) The chemical reaction is: $CaO_{(s)} + CO_{2(g)} ightarrow CaCO_{3(s)}$First,calculate the standard enthalpy of reaction $(\Delta H^o_r)$:$\Delta H^o_r = \Delta H^o_f(CaCO_3) - [\Delta H^o_f(CaO) + \Delta H^o_f(CO_2)]$$\Delta H^o_r = -1207 - [-635 + (-394)] = -1207 + 1029 = -178 \ kJ/mol$Next,calculate the change in internal energy $(\Delta E)$ for the reaction:$\Delta H = \Delta E + \Delta n_g RT$$\Delta E = \Delta H - \Delta n_g RT$Here,$\Delta n_g = 0 - 1 = -1$$T = 27 + 273 = 300 \ K$$R = 8.314 	imes 10^{-3} \ kJ \cdot K^{-1} \cdot mol^{-1}$For $280 \ g$ of $CaO$ (molar mass = $56 \ g/mol$):Moles of $CaO = \frac{280}{56} = 5 \ mol$Total $\Delta E = 5 	imes [\Delta H^o_r - (\Delta n_g RT)]$$\Delta E = 5 	imes [-178 - ((-1) 	imes 8.314 	imes 10^{-3} 	imes 300)]$$\Delta E = 5 	imes [-178 + 2.4942] = 5 	imes (-175.5058) = -877.529 \ kJ$The heat produced at constant volume $(q_v)$ is equal to $\Delta E$. Thus,the magnitude is $877.53 \ kJ$ (approximately $877.55 \ kJ$).

$(a)$ Entropy of vaporization	$(1)$ Decreases
$(b)$ $K$ for spontaneous process	$(2)$ Always has a $(+)$ value
$(c)$ Crystalline solid state	$(3)$ Has minimum entropy
$(d)$ $\Delta U$ for adiabatic expansion of an ideal gas	$(4)$ $\frac{\Delta H_{vap}}{T_b}$

Similar Questions

Match the following:

$(a)$ Entropy of vaporization $(1)$ Decreases

$(b)$ $K$ for spontaneous process $(2)$ Always has a $(+)$ value

$(c)$ Crystalline solid state $(3)$ Has minimum entropy

$(d)$ $\Delta U$ for adiabatic expansion of an ideal gas $(4)$ $\frac{\Delta H_{vap}}{T_b}$

Which graph represents an exothermic reaction?

$3 A_{(g)} \rightarrow 2 B_{(g)} + 2 D_{(g)} + E_{(g)}$
For the above reaction,$\Delta U = 5.1 \ kcal / mol$ and $\Delta S = 25 \ cal / mol \cdot K$. Which of the following is the correct statement at $300 \ K$?

Arrange the following isothermal processes in order of the magnitude of the work $(w)$ involved between states $1$ and $2$.
$A$. Expansion in single stage $(w_A)$
$B$. Expansion in multi stages $(w_B)$
$C$. Compression in single stage $(w_C)$
$D$. Compression in multi stages $(w_D)$

At $25^{\circ} \text{C}$,$1 \text{ mole}$ of butane is combusted to form $CO_2$ and liquid $H_2O$. The work done is $...... \text{ L atm}$.

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