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Asked Nov 16, 2019
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Calculate the amount of energy in the form of heat that is produced when a volume of 4.37 L of SO2(g) is converted to 4.37 L of SO3(g) according to this process at constant pressure and temperature of 1.00 bar and 25.0 ° C. Assume ideal gas behavior.

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Step 1

Given, 4.37L of SO2(g) converted to 4.37L of SO3(g).

Pressure = 1.00bar.

Temperature = 25.0 degree Celsius.

Step 2

The balanced reaction and the moles of SO2(g) and S...

2 SO,+o 2So
pressure 1bar=0.987 atm
Temperature 25+273 = 298 K
Moles of SO, orSO;
PV =nRT
PV
RT
0.987atmx4.37L
0.082Latm/molKx298K
-0.176mol SO2 or SO
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2 SO,+o 2So pressure 1bar=0.987 atm Temperature 25+273 = 298 K Moles of SO, orSO; PV =nRT PV RT 0.987atmx4.37L 0.082Latm/molKx298K -0.176mol SO2 or SO

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