Answer:
27.63 g of H2.
Step-by-step explanation:
We'll begin by writing the balanced equation for the reaction. This is illustrated below:
8CO + 17H2 → C8H18 + 8H2O
Thus, we can say that:
From the balanced equation above,
8 moles of CO reacted with 17 moles of H2.
Next, we shall determine the number of mole H2 that will react completely with 6.50 moles of CO.
This can be obtained as illustrated below:
From the balanced equation above,
8 moles of CO reacted with 17 moles of H2.
Therefore, 6.5 moles of CO will react with = (6.5 x 17)/8 = 13.813 moles of H2.
Therefore, 13.813 moles of H2 is needed to react completely with 6.50 moles of CO.
Finally, we shall convert 13.813 moles of H2 to grams. This can be achieved by doing the following:
Molar mass of H2 = 2x1 = 2 g/mol
Mole of H2 = 13.813 moles
Mass of H2 =.?
Mole = mass /molar mass
13.813 = mass of H2 /2
Cross multiply
Mass of H2 = 13.813 x 2
Mass of H2 = 27.63 g
Therefore, 27.63 g of H2 is needed for the reaction.