What mass of propane gas ($C_3H_8$) must burn in excess oxygen to produce 9.00 imes 10^3 kJ of heat, given the thermochemical equation: $C_3H_8 (g) + 5O_2 (g) o 3CO_2 (g) + 4H_2O (l)$ $Delta H = -2.22 imes 10^3 kJ$ a. 179 g b. 35.8 g c. 4.05 g d. 13.2 g e. heat is not produced by this reaction
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This means that if we burn more propane, we will produce more heat. The thermochemical equation tells us that burning one mole of propane produces -2.22 x 10^3 kJ of heat. The negative sign indicates that heat is released in the reaction. The molar mass of Show more…
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What mass of propane (C3H8) would be needed to produce this heat? a) C3H8 (g), for the combustion reaction ΔH = -2220 KJ/mol C3H8 (g) + 5 O2 (g) --> 3 CO2 (g) + 4 H2O (g); ΔH = -2220 KJ/mol
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Calculate the enthalpy change when $5.00 \mathrm{~g}$ of propane is burned with excess oxygen according to the reaction $$\mathrm{C}_{3} \mathrm{H}_{8}(g)+5 \mathrm{O}_{2}(g) \rightarrow 3 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2}\mathrm{O}(l) \quad \Delta H=-2221 \mathrm{~kJ} / \mathrm{mol}$$
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