Answer:
4804.5 g of SO₂ are needed to the reaction
Explanation:
The reaction to produce sulfuric acid is:
2SO₂ + O₂ + 2H₂O → 2H₂SO₄
Ratio is 1:2. 1 mol of oxygen needs 2 moles of sulfur dioxide in order to react. We can propose this rule of three.
If 1 mol of O₂ react to 2 moles of SO₂
Then, 37.50 moles of O₂ will react with (37.5 . 2) /1 = 75 moles of SO₂
We convert the moles to mass, to know the answer:
75 mol . 64.06 g / 1 mol = 4804.5 g of SO₂
Answer:
952.2g SO3
Explanation:
Molar mass of C4H8S2 is 120.2363 g/mol
Mol in 750.0g = 750.0/120.2363 = 6.238 mol
1mol C4H8S2 produces 2 mol SO3
6.238 mol will produce 2×6.238 = 12.476 mol SO3
Molar mass SO3 = 32+3×16 = 80.0g/mol
Theoretical yield = 12.476×80.0 = 998.08g
The actual yield is 95.4%
Actual mass-produced = 95.4/100×998.08 = 952.2g SO3 produced
Hope it will help you.
<span>1 mol N2 = 2 mol NH3
325g / 16g/mol = 20.3 mol which ammonia only requires 10.15 mol N2 to produce
10.15 mol x 28.014g/mol
= 284 g
it makes sense that the mass required should be smaller than the mass of the larger product molecules</span>
Explain the question more please hggghhg
Elector would be that a laser converts electrical energy
