# Problem: Assuming the heat released from the combustion of CH 4 can be used with 100% efficiency, how much CH4 (in g) is required to be combusted in the presence of excess oxygen to warm 1.75 kg of water (Cw= 4.184 J/gK) from 25.0 to 98.0 °C? The enthalpy of combustion of CH4 is -802.3 kJ/mol.A. 56.5 gB. 46.2 gC. 28.7 gD. 10.7 gE. 7.04 g

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###### Problem Details

Assuming the heat released from the combustion of CH 4 can be used with 100% efficiency, how much CH4 (in g) is required to be combusted in the presence of excess oxygen to warm 1.75 kg of water (Cw= 4.184 J/gK) from 25.0 to 98.0 °C? The enthalpy of combustion of CH4 is -802.3 kJ/mol.

A. 56.5 g

B. 46.2 g

C. 28.7 g

D. 10.7 g

E. 7.04 g

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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 Burk's class at MSSTATE.