You will need to use the ideal gas constant: R = 0.083145 L·bar/(mol·K) Sulfur d

Question

You will need to use the ideal gas constant: R = 0.083145 L·bar/(mol·K)

Sulfur dioxide, SO_2(g), can react with oxygen to produce sulfur trioxide, SO_3(g), by the following reaction The standard enthalpies of formation for SO_2(g) and SO_3(g) are Calculate the amount of energy in the form of heat that is produced when a volume of 4.69 L of SO_2(g) is converted to 4.69 L of SO_3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 degree C. Assume ideal gas behavior.

Explanation / Answer

V = 4.69 L of SO2

V2 = 4.69 L of SO3

P = 1 bar

T = 25°C

R = 0.083145 Lbar/molK

find heat

2SO2 + O2 --> 2SO3

Find the heat of reaction

Hrxn = Hproducts - Hreactants = 2*-395.7 kJ/mol - 2*-296.8 kJ/mol = -197.8 kJ

Hrxn = -197.8 kJ

Find initial moles of SO2

PV = nRT

n = PV/RT)

n = 1bar * 4.69L / (0.083145*298K ) = 0.18928 mol of SO2

find moles of SO3

PV =nRT

n = PV/(RT) = (1bar*4.69L)/(0.08314 * 298) = 0.18928 mol of SO3

Therefore

if 2 mol of SO3 produced will libreate H =  -197.8 kJ

Therefore

0.18928 mol of SO3 will give = 0.18928/2 * -197.8 = -18.72 kJ

E = -18.72 kJ

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