How much heat is evolved when 320 g of SO2 is burned according to the chemical equation shown below? 2 SO2(g) + O2(g) ----> 2 SO3(g) ΔHorxn = -198 kJ
So 2*64 g SO2 or 128 grams (two moles SO2) evolve 198 kJ, how much heat do we get from 320 g SO2.
That's dH = 198 kJ x (320/128) = ? kJ
Well, there's nothing quite like a burning question! So, let's calculate the heat evolved, shall we?
According to the balanced equation, 2 moles of SO2 are required to produce 2 moles of SO3. So, let's convert the given mass of SO2 (320 g) into moles. The molar mass of SO2 is approximately 64 g/mol.
So, moles of SO2 = (320 g) / (64 g/mol) = 5 moles
Since the equation states that ΔHorxn (the heat of reaction) is -198 kJ, we now know that 2 moles of SO2 produce -198 kJ. Therefore, 5 moles of SO2 will produce (5/2) * (-198 kJ) = -495 kJ.
So, to answer your question, approximately -495 kJ of heat is evolved when 320 g of SO2 is burned. But don't worry, this is just a chemical reaction, not a hot temper!
To find the amount of heat evolved when 320 g of SO2 is burned, we need to use the stoichiometry of the reaction and the given enthalpy change.
Step 1: Calculate the molar mass of SO2.
Sulfur (S) has an atomic mass of 32.07 g/mol, and Oxygen (O) has an atomic mass of 16.00 g/mol. Since SO2 has one sulfur and two oxygen atoms, the molar mass of SO2 is:
Molar mass of SO2 = (1 × atomic mass of S) + (2 × atomic mass of O)
= (1 × 32.07 g/mol) + (2 × 16.00 g/mol)
= 64.07 g/mol.
Step 2: Calculate the number of moles of SO2.
Number of moles = Mass / Molar mass
= 320 g / 64.07 g/mol
≈ 4.998 mol (approximately 5 mol).
Step 3: Use the balanced equation to determine the amount of heat evolved per mole of SO2.
According to the balanced equation, for every 2 moles of SO2 burned, 198 kJ of heat is evolved. Therefore, for 1 mole of SO2 burned, the amount of heat evolved is:
Heat evolved per mole of SO2 = (-198 kJ) ÷ 2
= -99 kJ.
Step 4: Calculate the heat evolved for 5 moles of SO2.
Heat evolved = Heat evolved per mole of SO2 × Number of moles
= (-99 kJ/mol) × 5 mol
= -495 kJ.
Therefore, when 320 g of SO2 is burned, approximately 495 kJ of heat is evolved.
To calculate the heat evolved during the combustion of SO2, you need to use stoichiometry and the given enthalpy change of the reaction (ΔHorxn).
Step 1: Determine the moles of SO2
To find the moles of SO2, divide the given mass (320 g) by the molar mass of SO2, which is 64.07 g/mol:
moles of SO2 = mass of SO2 / molar mass of SO2
moles of SO2 = 320 g / 64.07 g/mol ≈ 5.00 mol
Step 2: Use the stoichiometry of the reaction
From the balanced equation, you can see that 2 moles of SO2 reacts to form 2 moles of SO3. Therefore, the moles of SO3 formed will also be 5.00 mol.
Step 3: Calculate the heat evolved
The heat evolved can be calculated using the equation:
heat evolved = moles of SO3 × ΔHorxn
heat evolved = 5.00 mol × (-198 kJ/mol)
heat evolved = -990 kJ
Therefore, when 320 g of SO2 is burned according to the given reaction, approximately 990 kJ of heat is evolved.