Question

Combustion of amyl alcohol (C5H11OH) occurs according to the following
reaction :
2C5H11OH(l)+15O2(g)®10CO2(g)+12H2O(l)
(a) How many water molecules are produced from each mole of amyl alcohol
burnt?
(b) How much volume (in litre) of CO2 at STP (0 ºC, 1 bar pressure) is
produced from each gram of amyl alcohol burnt?

Answer 1

Answer:

hey brainist here ur answer is

1)balance the reaction

2C5H11OH+15O2--->10CO2+12H20

2) number of moles of pentyl alcohol (C5H11OH) = 530 grams / 88.15 g/mole = 6.012 moles;

From the reaction’s coefficients, number of moles of oxygen =

= (15 x 6.012) / 2 = 45.1 moles;

Number of oxygen molecules = moles x Na = 45.1 mole x 6.02x1023 molecules/mole= 2.7 x 1025 molecules

3) Number of moles of carbon dioxide CO2 = 1.505 x 1021 / 6.02x1023 = 0.0025 moles;

From the reaction’s coefficients, number of moles of water =

= (12 x 0.0025) / 10 =0.003 moles;

Therefore, mass of water formed during this reaction = 0.003 mole x 18 g/mole = 0.054 g.

Explanation:

THANKS