Given the equation 2SO2(g) +O2(g) -> 2SO3(g), H = -197.8 kJ per Mole, find the quantity of heat transferred when 8.54 grams of sulfur dioxide react completely.
I'm stuck. Please help >-<
molmass SO2=64g (check that)
8.54/(64)=Heat/(-197.8kJ)
The equation tells you that 2 mols SO2 will generate 197.8 kJ. How much is 2 mols SO2? That's 2*64 = 128 g SO2 will generate 197.8 kJ. So what will 8.54 g do? Set up a ratio/proportion or use reason to do it. Here is ratio/proportion:
(128 g/197.8 kJ) = 8.54 g/x kJ). Solve for x.
Reason:
197.8 kJ x (8.54/128) = ?
Sorry I posted too. I was almost through answering when the phone rang and when the conversation was over I didn't check if the question had been answered.
To find the quantity of heat transferred when 8.54 grams of sulfur dioxide (SO2) reacts completely, we can follow these steps:
1. Convert the mass of sulfur dioxide (SO2) to moles:
molar mass of SO2 = 32.07 g/mol + 2(16.00 g/mol) = 64.07 g/mol
moles of SO2 = mass of SO2 / molar mass of SO2
moles of SO2 = 8.54 g / 64.07 g/mol
2. Calculate the quantity of heat transferred per mole of SO2:
H = -197.8 kJ/mol
3. Calculate the quantity of heat transferred when 8.54 grams of SO2 reacts completely:
quantity of heat transferred = (moles of SO2) * (H)
quantity of heat transferred = (moles of SO2) * (-197.8 kJ/mol)
Now let's calculate the values:
1. moles of SO2 = 8.54 g / 64.07 g/mol
moles of SO2 ≈ 0.1333 mol
2. quantity of heat transferred = (0.1333 mol) * (-197.8 kJ/mol)
quantity of heat transferred ≈ -26.36 kJ
Therefore, the quantity of heat transferred when 8.54 grams of sulfur dioxide react completely is approximately -26.36 kJ. Note that the negative sign indicates an exothermic reaction, meaning heat is released.