How many grams of CO2 would be formed from 30 grams of C4H10 in the following (UNBALANCED) reaction? ?

Question

How many grams of CO2 would be formed from 30 grams of C4H10 in the following (UNBALANCED) reaction?

C4H10 + O2 → CO2 + H2O

I believe that the balanced equation is:

2C4H10 + 13 O2 → 8 CO2 + 10 H2O

But I am not sure where to go after that.....any help would be appreciated!!

Answer 1

Your balanced equation looks good to me also.

To work out the mass of CO2 formed you first need to work out the number of moles of C4H10 that you start with, you always compare compounds based on moles.

moles of C4H10 = mass / molecular weight

molecular weight C4H10 = (4 x 12.01) + (10 x 1.008) = 58.12 g/mol

So moles = 30 g / 58.12 g/mol

= 0.516 moles of C4H10

From your equation, you know that for every 2 moles of C4H10 you produce 8 moles of CO2, (1 mole gives you 4 moles)

Therefore number of moles of CO2 produced = 4 x moles of C4H10

= 4 x 0.516

= 2.064 moles of CO2 is produced from 30 g of C4H10

Again, moles = mass / molecular weight

So mass of CO2 = moles  x molecular weight

molecular weight CO2 = 12.01 + (16.00 x 2) = 44.01 g/mol

mass = 2.064 moles x 44.01 g/mol

= 90.84 g

= 91g (2 sig figs)

Answer 2

2 C4H10 + 13 O2 >> 8 CO2 + 10 H2O

moles C4H10 = 30 g / 58.124 g/mol = 0.516

Moles CO2 = 0.516 x 8 / 2 = 2.06

Mass CO2 = 44 g/mol x 2.06 mol = 90.8 g