The combustion of propane may be described by the chemical equation C 3 H 8 ( g ) + 5 O 2 ( g ) ⟶ 3 CO 2 ( g ) + 4 H 2 O ( g ) C3H8(g)+5O2(g)⟶3CO2(g)+4H2O(g) How many grams of O 2 ( g ) O2(g) are needed to completely burn 17.9 g C 3 H 8 ( g ) ?

65.1g of O2 will be needed

Explanation:

The equation for the reaction is given below:

C3H8 + 5O2 —>3CO2 + 4H2O

Molar Mass of C3H8 = (3x12) + (8x1) = 36 + 8 = 44g/mol

Molar Mass of O2 = (16x2) = 32g/mol

Mass conc. of O2 from the balanced equation = 5 x 32 = 160g

From the above calculations, we can easily find the mass of O2 needed to completely burn 17.9 g C3H8. This can be done by the following:

From the equation,

44g of C3H8 was completely burnt by 160g of O2.

Therefore,

17.9g of C3H8 will be burnt by Xg of O2. i.e

Xg of O2 = (17.9x160) / 44 = 65.1g

it would be d. henry moseley

hope this !

and sorry if i'm late. have a good rest of your day! : d

answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error