3CO2 + 4H2O How Many Grams Of CO2 Will Be Produced From 7.00 ...

Subject ZIP Search Search Find an Online Tutor Now Ask Ask a Question For Free Login Chemistry Stoichiometry In the following reaction (already balanced) C3H8 + 5O2 —> 3CO2 + 4H2O How many grams of CO2 will be produced from 7.00 g of C3H8 and 98.0 g of O2? (Rounded to three significant figures) Follow • 1 Add comment More Report

1 Expert Answer

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First, we need to convert grams of each reactant to moles.

When we convert grams to moles or moles to grams, we use molar mass.

The molar mass of O2 is 16.0g/mol, C3H8 is 44.1g/mol

-> O2 : 98.0g / (16.0 g/mol) = 6.13 mol

-> C3H8 : 7.00g / (44.1g/mol) = 0.159 mol

Now, we need to find which one is limiting reactant.

From balanced equation, we get 1:5 ratio between C3H8 : O2.

If we assume C3H8 is limiting reactant, we will consume 0.159 moles (all) and (0.159moles * 5 = 0.795)moles of O2. Since we have enough amount of O2 for this reaction, our assumption was correct.

Therefore, C3H8 is limiting reactant and O2 is excess reactant.

Then, we take ratio between C3H8 : CO2 to find the number of mole of CO2 produced.

They have 1:3 ratio, so we will get (0.159 * 3 = 0.477)moles of CO2.

For final answer, we need to convert moles to grams.

The molar mass of CO2 is 44.01g/mol.

-> 0.477mol * 44.01g/mol = 21.0 g

Answer : 21.0g of CO2

Hope this is helpful! :)

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