# Problem: Natural gas burns in air to form carbon dioxide and water, releasing heat.CH4(g) + O2(g) → CO2(g) + H2O(g); ΔHrxn˚ = –802.3 kJ/molWhat minimum mass of CH4 is required to heat 65.0 g of water by 26.0˚C? (Assume 100% heating efficiency.) (For water, Cs= 4.18 J/g•˚C).

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###### FREE Expert Solution

We are asked to calculate the minimum mass of CH4 is required to heat 65.0 g of water by 26.0˚C? (Assume 100% heating efficiency.) (For water, Cs= 4.18 J/g•˚C).

Calculate Q :

Q = 7064.2 J

We'll use the thermochemical equation to calculate the mass of CH4.

Molar mass CH4 = 16.05 g/mol

CH4(g) + O2(g) → CO2(g) + H2O(g); ΔHrxn˚ = –802.3 kJ/mol ###### Problem Details

Natural gas burns in air to form carbon dioxide and water, releasing heat.

CH4(g) + O2(g) → CO2(g) + H2O(g); ΔHrxn˚ = –802.3 kJ/mol

What minimum mass of CH4 is required to heat 65.0 g of water by 26.0˚C? (Assume 100% heating efficiency.) (For water, Cs= 4.18 J/g•˚C).