Problem: Elemental S reacts with O2 to form SO3 according to the reaction2 S + 3 O2 → 2 SO3A) How many O2 molecules are needed to react with 4.13 g of S? Express your answer numerically in units of molecules.B) What is the theoretical yield of SO3 produced by the quantities described in Part A? Express your answer numerically in grams.C) Next, consider a situation in which all of the S is consumed before all of the O2 reacts, or one in which you have excess S because all of the O2 has been used up. For each of the given situations, indicate whether S or O2 is the limiting reactant.• 3.00 mol Sulfur, 3.00 mol Oxygen• 3.00 mol Sulfur, 4.00 mol Oxygen• 3.00 mol Sulfur, 5.00 mol Oxygen

FREE Expert Solution

We’re given the following balanced reaction:

2 S + 3 O2 → 2 SO3

Part A: We’re being asked to calculate the O2 molecules needed to react with 4.13 g of S.

We need to perform a mole-to-mole comparison between O2 and S.

molar mass of S = 32.066 g/mol

1 mole = 6.022x1023 molecules

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Problem Details

Elemental S reacts with O2 to form SO3 according to the reaction

2 S + 3 O2 → 2 SO3

A) How many O2 molecules are needed to react with 4.13 g of S? Express your answer numerically in units of molecules.

B) What is the theoretical yield of SO3 produced by the quantities described in Part A? Express your answer numerically in grams.

C) Next, consider a situation in which all of the S is consumed before all of the O2 reacts, or one in which you have excess S because all of the O2 has been used up. For each of the given situations, indicate whether S or O2 is the limiting reactant.

• 3.00 mol Sulfur, 3.00 mol Oxygen

• 3.00 mol Sulfur, 4.00 mol Oxygen

• 3.00 mol Sulfur, 5.00 mol Oxygen