Question
Asked Oct 13, 2019

Calculate the number of moles of methane needed to complete the heating process.

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
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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

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check_circleExpert Solution
Step 1

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

Step 2

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.

Step 3

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
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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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