Calculate the amount of energy in the form of heat that is produced when a volume of 3.56 L of SO2(g) is converted to 3.56 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.
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To calculate the amount of energy in the form of heat produced during the given process, we need to use the concept of the heat of reaction, also known as the enthalpy change (∆H).
Here's the step-by-step breakdown to solve this problem:
Step 1: Write the balanced equation
Start by writing the balanced chemical equation for the reaction. Based on the given information, the equation is:
SO2(g) + 1/2 O2(g) -> SO3(g)
Step 2: Determine the standard heat of reaction (∆H°)
Look up the standard heat of reaction, ∆H°, for the given reaction. For this problem, the value is provided as -198.2 kJ/mol.
Step 3: Convert volume to moles
The given volume of gas (3.56 L) needs to be converted to moles. To do this, we can use the ideal gas law:
PV = nRT
Given:
P = 1.00 bar (convert to atm by dividing by 1.01325 bar/atm)
V = 3.56 L
T = 25.0 °C (convert to Kelvin by adding 273.15)
R = 0.0821 L.atm/(mol.K) (gas constant)
Let's perform the conversion:
P = 1.00 bar / 1.01325 bar/atm = 0.987 atm
T = 25.0 °C + 273.15 = 298.15 K
Using the ideal gas law, we rearrange it to solve for the number of moles (n):
n = PV / RT
n = (0.987 atm) * (3.56 L) / (0.0821 L.atm/(mol.K) * 298.15 K)
Calculate the number of moles for SO2.
Step 4: Calculate the heat produced
Finally, to calculate the amount of energy in the form of heat produced during the reaction, we use the equation:
q = ∆H° * (moles of SO2)
Plug in the values:
q = -198.2 kJ/mol * (moles of SO2)
Multiply the number of moles by -198.2 kJ/mol to get the value of heat produced in kilojoules.
And there you have it! Follow these steps to calculate the amount of energy in the form of heat produced during the conversion process from SO2(g) to SO3(g).