Question

Given:

8CO + 17H2 → C8H18 + 8H2O

In this chemical reaction, how many grams of H2 will react completely with 6.50 moles of CO? Express your answer to three significant figures.

Answer 1

27.6g to 3 sig fig. Moles ratio of CO: H2 is 8:17 so if there is 6.50 moles of CO reacting it is with (17/8 x 6.5) = 13.81 moles of H2. The Mr of H2 is 2x1 = 2. The mass of H2 = moles x Mr so 13.81 x 2 = 27.6

Answer 2

Mass of H2 = 27.6 g

Step-by-step explanation:

Given:

Moles of CO = 6.50

The balanced reaction is:

8CO + 17H2 → C8H18 + 8H2O

Based on the reaction stoichiometry:

8 moles of CO reacts with 17 moles of H2

Therefore, 6.50 moles of CO would react with:

=
`(6.50\ moles\ CO * 17\ moles\ H2)/(8\ moles\ CO) = 13.8 moles`

Molar mass of H2 = 2 g/mole

Mass of H2 reacted =
`Moles *molar mass = 13.8 moles * 2g/mol= 27.6 g`