Methane is combusted to heat 10 kg of ice from -20°C to 70°C. Use the following information to answer the followingquestion.CP,ice +37.1 J/mole-°CCp,water 75.3 J/mole-°CAHfus, water= +6.01 kJ/moleAHcombustion, methane802 kJ/mole
Calculate the number of moles of methane needed to complete the heating process.
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Methane is combusted to heat 10 kg of ice from -20°C to 70°C. Use the following information to answer the following question. CP,ice +37.1 J/mole-°C Cp,water 75.3 J/mole-°C AHfus, water = +6.01 kJ/mole AHcombustion, methane 802 kJ/mole
Given information:
Mass of ice = 10 kg
Initial temperature = -20 °C
Final temperature = 70 °C
Cp,ice = + 37.1 J/mole.°C
Cp,water = + 75.3 J/mole.°C
ΔHfus, water = + 6.01 kJ/mole
ΔHcombustion, methane = -802 kJ/mole
The amount of heat required to raise the temperature by 1°C is known as heat capacity. The heat capacity at constant pressure is represented by Cp.
The amount of heat released or absorbed can be expressed in terms of heat capacity and temperature chan...
![ice n.Cp.AT
10kg
18.01528g/mole
-x37.1 J/mole. Cx[70-(-20)] °C
10000g
x37.1 J/mole. C70-(-20)] °C
18.01528g/mole
= 1853426.6 J
= 1853.42 kJ](https://prod-qna-question-images.s3.amazonaws.com/qna-images/answer/0a7468cf-5dcd-4f1e-8912-bf38d1cd3387/48aa804d-13e8-46cf-b0b7-194cb8fc03cc/y1w7kpw.png)
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ice n.Cp.AT 10kg 18.01528g/mole -x37.1 J/mole. Cx[70-(-20)] °C 10000g x37.1 J/mole. C70-(-20)] °C 18.01528g/mole = 1853426.6 J = 1853.42 kJ
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