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. _______ grams of H2 will react completely.

Answer 1

Answer:- 27.6 grams of hydrogen are required.

Solution:- The given balanced equation is:

$8CO+17H_2\rightarrow C_8H_1_8+8H_2O$

From balanced equation, there is 8:17 mol ratio between CO and $H_2$ means 17 moles of hydrogen are required to react completely with 8 moles of CO.

Let's calculate the number of moles of hydrogen required to react completely with 6.50 moles of CO and convert to grams on multiplying by molar mass of hydrogen as:

$6.50 moles CO(\frac{17 mol H_2}{8 mol CO})(\frac{2g H_2}{1mol H_2})$

= $27.6 g H_2$

So, 27.6 grams of hydrogen are required to react completely with 6.50 moles of CO.

Answer 2

Answer:

not correct^

Explanation: