From the data in Table 2C.4 of the Resource section, calculate ?rH? and ?rU? at (i) 298 K, (ii) 478 K for the reaction C(graphite) + H2O(g) ? CO(g) + H2(g). Assume all heat capacities to be constant over the temperature range of interest.
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4. These values are typically given in kJ/mol for enthalpies and J/(mol·K) for entropies. For the reaction C(graphite) + H2O(l) → CO(g) + H2(g), the values are as follows: - ΔHf°[C(graphite)] = 0 kJ/mol (since it's a standard state) - ΔHf°[H2O(l)] = -285.83 Show more…
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For the reaction C(graphite) $+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons$ $\mathrm{CO}(g)+\mathrm{H}_{2}(g), \Delta H_{R}^{\circ}=131.28 \mathrm{kJ} \mathrm{mol}^{-1}$ at $298.15 \mathrm{K} .$ Use the values of $C_{P, m}^{\circ}$ at $298.15 \mathrm{K}$ in the data tables to calculate $\Delta H_{R}^{\circ}$ at $125.0^{\circ} \mathrm{C}$
At 298 K, ΔH°r = 131.28 kJ⋅mol−1 for the reaction C(graphite) + H2O(g) → CO(g) + H2(g) with CP,m = 8.53, 33.58, 29.12, and 28.82 J⋅K−1⋅mol−1 for graphite, H2O(g), CO(g), and H2(g), respectively. Calculate ΔH°r at 175 °C from this information. Assume that the heat capacities are independent of temperature. Express your answer to five significant figures and include the appropriate units.
Madhur L.
a) Consider the reaction: B2H6(g) + 3O2(g) → B2O3(s) + 3H2O(g) ∆H = -2035 kJ How much heat is released when a mixture of 9.85 g B2H6 and 7.72 g O2 is burned? b) The specific heat capacity of graphite is 0.71 J/°Cg. Calculate the energy required to raise the temperature of 3.2 mol of graphite by 25.0°C. c) The specific heat capacity of graphite is 0.71 J/°Cg. Calculate the energy required to raise the temperature of 30 kg graphite from 294 K to 348 K. d) The specific heat capacity of graphite is 0.71 J/°Cg. Calculate the molar heat capacity for graphite.
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