Using Hess's law, calculate ?H for the reaction below, given thermochemical equations (1) - (3). H2(SO4)(l) ? SO3(g) + H2O(g) ?H = __________ (1) H2S(g) + 2O2(g) ? H2(SO4)(l) ?H = - 235.5 kJ (2) H2S(g) + 2O2(g) ? SO3(g) + H2O(l) ?H = - 207 kJ (3) H2O(l) ? H2O(g) ?H = 44 kJ
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First, we need to write the balanced equation for the reaction we want to calculate AH for: Hz(SO_X) + AaStg) + H,Ctw + 6H,Ole) -> SOslg + 2H_Ste) + 4H (1) Show more…
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Using Hess’s Law determine the heat of reaction for the following: C2H4(g) + 6F2(g) → 2CF4(g) + 4HF(g) 1. H2(g) + F2(g) → 2HF(g) ∆Hᵒ = -546.6 kJ 2. C(s) + 2F2(g) → CF4(g) ∆Hᵒ = -680.0 kJ 3. 2C(s) + 2H2(g) → C2H4(g) ∆Hᵒ = +52.4 kJ A. +2505.6 kJ B. -2505.6 kJ C. -1174.2 kJ D. +1174.2 kJ E. +277.4 kJ
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Use the information in thermochemical equations (1) through ( 3 ) to calculate the value of $\Delta H_{\mathrm{rxn}}^{\circ}$ for the reaction in equation (4). (1) $\mathrm{Pb}(s)+\frac{1}{2} \mathrm{O}_{2}(g) \rightarrow \mathrm{PbO}(s) \quad \quad \Delta H_{\mathrm{rxn}}^{\circ}=-219 \mathrm{kJ}$ (2) $\mathrm{C}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g) \Delta H_{\text {rxn }}^{\circ}=-394 \mathrm{kJ}$ (3) $\mathrm{PbCO}_{3}(s) \rightarrow \mathrm{PbO}(s)+\mathrm{CO}_{2}(g) \quad \Delta H_{\text {rxn }}^{\circ}=86 \mathrm{kJ}$ (4) $2 \mathrm{Pb}(s)+2 \mathrm{C}(s)+3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{PbCO}_{3}(s) \quad \Delta H_{\mathrm{rxn}}^{\circ}=?$
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