Question

he combustion of propane (C3H8) is given by the balanced chemical equation C_3H_8+5O_2\longrightarrow3CO_2+4H_2O C 3 H 8 + 5 O 2 ⟶ 3 C O 2 + 4 H 2 O How many grams of carbon dioxide gas (CO2) are produced burning 97 g of propane? Round your answer to the nearest gram.

Answer 1

290 grams

Step-by-step explanation:

Let's begin by writing the balanced chemical equations:

`C_(3)H_(8) +5O_(2) --->3CO_(2) +4H_(2)O`

Then we calculate the number of moles in 97g of propane.

n(propane)=
`(mass)/(molarmass) =(97g)/(44.1g/mol)=2.1995mol`

According to the balanced chemical equation, one mole of propane produces 3 moles of carbon dioxide. So the available number of moles of propane must be multiplied by three to work out the number of carbon dioxide produced.

n(carbon dioxide)= 2.1995mol*3 = 6.5985mol

mass(carbon dioxide) = moles * molar mass

= 6.5985 mol * 44.01 g/mol

= 290 grams