Question

1. Assuming there is an excess of oxygen present, how much carbon dioxide (in kg) will be produced in the combustion of 4.000 L of gasoline (C8H18)? The density of gasoline is 0.79 g / mL. C - 12.00 g/mol H - 1.00 g/mol O - 16.00 g/mol. ______________

2. Which of the following molecules will NOT show a linear molecular geometry?

		BeCl2
		SO2
		CO2
		XeF2

Answer 1

1. The balanced equation for the combustion of gasoline (C₈H₁₈) can be written as follows.

2C₈H₁₈(g) + 25O₂(g) 16CO₂(g) + 18H₂O(g)

The mass of gasoline = 4000 mL * 0.79 g/mL = 3160 g

The no. of moles of gasoline = 3160 g/(114 g.mol^-1) = 27.7193 mol

From the balanced equation, the mole ratio of gasoline to CO₂ = 2:16 = 1:8

Therefore, the no. of moles of CO₂ produced = 8*27.7193 mol = 221.7544 mol

Hence, the mass of CO₂ produced = 221.7544 mol * 44 g/mol = 9.757 kg

2. The answer is SO₂, which shows bent geometry.