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olga_2 [115]
3 years ago
11

Based on the following reaction, determine how much heat is released if 500. grams of methane is combusted in excess oxygen: CH4

+ 2 O2  CO2 + 2 H2O H= – 890 kJ
Chemistry
1 answer:
EastWind [94]3 years ago
3 0

Answer:

- 13,150.6kJ

Explanation:

CH4 + 2 O2 ------> CO2 + 2 H2O ΔH= – 890 kJ

The ΔH is enthalpy change of combustion , which is the heat is either absorbed or released by the combustion of one mole of a substance.

ΔH=−890 kJ/mol (released in the combustion of one mole of methane)

using the molar mass  (in grams )of methane to get moles of sample

(237g × 1 mole of CH4)/16.04g=14.776 moles  of CH4

Since 1 mole produces 890 kJ of heat upon combustion, then 14.776 moles will produce

ΔH = 14.776moles of CH4 × 890kJ/1mole of CH4

=13,150.6kJ

Therefore ΔH = - 13,150.6kJ

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Reaction

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2. Find the mole ratio of  CaCO₃ : CO₂(from equation = 1 : 1)

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3. Find the mass of CO₂ from the molar mass of CO₂

\tt mass_{CO_2}=n_{CO_2}\times MW_{CO_2}

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