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).

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

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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 = mCTQ = (65.0 g)(4.18 J/ g˚C)(26˚C)

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


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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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What scientific concept do you need to know in order to solve this problem?

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

What professor is this problem relevant for?

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