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3 years ago

If you burn 150. g of C2H6O, how many grams of CO2 and H2O can be produced?

Business

1 answer:

VLD [36.1K]3 years ago

5 0

Answer:

We will produce 2.87 * 10³ grams CO2 and 1.76 *10³ grams H2O

Explanation:

Step 1: Data given

Mass of C2H6O = 150.0 grams

Molar mass of C2H6O = 46.07 g/mol

Step 2: The balanced equation

C2H6O + 3O2 → 2CO2 + 3H2O

Step 3: Calculate moles C2H6O

Moles C2H6O = mass C2H6O / molar mass C2H6O

Moles C2H6O = 150.0 grams / 46.07 g/mol

Moles C2H6O = 3.256 moles

Step 4: Calculate moles products

For 1 mol C2H6O we need 3 moles O2 to produce 2 moles CO2 and 3 moles H2O

For 3.256 moles C2H6O we'll have 2*3.256 = 6.512 moles CO2

For 3.256 moles C2H6O we'll have 3 * 3.256 = 9.768 moles H2O

Step 5: Calculate mass of products

Mass CO2 = 6.512 moles * 44.01 g/mol = 286.6 grams = 2.87 * 10³ grams

Mass H2O = 9.768 moles * 18.02 g/mol = 176.0 grams = 1.76 *10³ grams

We will produce 2.87 * 10³ grams CO2 and 1.76 *10³ grams H2O

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Total equivalent units 100,000 66,000 83,000

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