How much heat is released when 28.00 g of methane is combusted using the reaction below? CH4 + 2O2 → CO2 + 2H2O ΔHrxn = -990 kJ
Added by Janet S.
Step 1
First, we need to determine the moles of methane (CH4) in 28.00 g. To do this, we can use the molar mass of methane: Molar mass of CH4 = 12.01 g/mol (C) + 4(1.01 g/mol) (H) = 16.05 g/mol Moles of CH4 = mass/molar mass = 28.00 g/16.05 g/mol = 1.744 mol Show more…
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Methane burns with oxygen to produce carbon dioxide and water as a gas. The balanced thermochemical equation is $$ \mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g) \atop \Delta H^{\circ}=-802 \mathrm{~kJ} $$ How much methane, in grams, must be burned to release $432 \mathrm{~kJ}$ of heat?
How much heat would be released if 36 g of methane (molar mass: 16.05 g/mol) burned according to this thermochemical equation? CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O (l) ∆Hrxn = -891 kJ
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