I just really want to learn how to solve this kind of problem. I know it involve

Question

I just really want to learn how to solve this kind of problem. I know it involves finding heat and work but I'm having a hard time trying to figure that out.

The picture wont upload so:

Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g), by the following reaction

2SO2(g) + O2(g) --> 2SO3(g)

The standard enthalpies of formation for SO2(g) and SO3(g) are:

SO2(g) = -298.8 kj/mol

SO3(g) = -395.7 kj/mol

Calculate the amount of energy in the form of heat that is produced when a volume of 4.14 L of SO2(g) is converted to 4.14 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C. Assume ideal gas behavior.

Explanation / Answer

Pressrue, P = 1 bar

Temperature T = 25'C = 298 K

Volume V = 4.14 L

Gas constant, R = 8.314*10-2 L bar K-1 mol-1

Using ideal gas constant, PV = nRT

n = PV/RT

Putting values we get :

n = 0.167 moles

Given reaction :

2SO2 (g) + O2(g) ----> 2SO3(g)

According to this reaction, heat produced = 2dHf(SO3)*n + dHf(O2) - 2dHf(SO2)*n

Here, n = number of moles = 0.167

dHf(O2) = standard enthalpy of formation of O2 = 0

Putting values we get :

Heat produced = 2*(-395.7)*0.167 + 0 - 2*(-298.8)*0.167 = -32.36 kJ

Thus, 32.36 kJ heat is consumed because sig is negative.

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