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

We are asked to calculate the minimum mass of CH_{4} is required to heat 65.0 g of water by 26.0˚C? (Assume 100% heating efficiency.) (For water, C_{s}= 4.18 J/g•˚C).

Calculate Q :

$\overline{){\mathbf{Q}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{mC}}{\mathbf{\u2206}}{\mathbf{T}}}\phantom{\rule{0ex}{0ex}}\mathbf{Q}\mathbf{}\mathbf{=}\mathbf{}(65.0\overline{)g})(4.18J/\overline{)\mathrm{g}}\u2022\overline{)\u02daC})\left(26\overline{)\u02daC}\right)$

**Q = 7064.2 J **

We'll use the thermochemical equation to calculate the mass of CH_{4}.

Molar mass CH_{4} = 16.05 g/mol

CH_{4}(g) + O_{2}(g) → CO_{2}(g) + H_{2}O(g); ΔH_{rxn}˚ = –802.3 kJ/mol

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

CH_{4}(g) + O_{2}(g) → CO_{2}(g) + H_{2}O(g); ΔH_{rxn}˚ = –802.3 kJ/mol

What minimum mass of CH_{4} is required to heat 65.0 g of water by 26.0˚C? (Assume 100% heating efficiency.) (For water, C_{s}= 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 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.

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