Given: 8CO + 17H2 → C8H18 + 8H2O In this chemical reaction, how many grams of H2 will react completely with 6.50 moles of CO? grams of H2 will react completely

27.63 g of H2.

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.

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