# 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).

###### 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

97% (461 ratings) ###### 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).

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Our tutors have indicated that to solve this problem you will need to apply the Thermochemical Equations concept. You can view video lessons to learn Thermochemical Equations. Or if you need more Thermochemical Equations practice, you can also practice Thermochemical Equations practice problems.

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Based on our data, we think this problem is relevant for Professor Hempstead's class at York University.