Question

How many grams of hydrogen are necessary to react with 2.85 mol CO

Answer 1

To react with 2.85 moles of CO, 11.4912 grams of hydrogen gas (H₂) are necessary based on the balanced equation 2 H₂ + CO → CH₃OH.

Step-by-step explanation:

To determine how many grams of hydrogen are necessary to react with 2.85 mol of CO, we need to refer to the balanced chemical reaction equation that hydrogen and CO might participate in. One such reaction is the synthesis of methanol:

2 H₂ + CO → CH₃OH

According to this equation, 2 moles of hydrogen gas (H₂) react with 1 mole of carbon monoxide (CO) to produce methanol (CH₃OH). Therefore, to react with 2.85 moles of CO, we would need 5.70 moles of hydrogen gas (2 x 2.85 moles of CO). To convert moles of hydrogen to grams, we multiply by the molar mass of hydrogen (approximately 2.016 g/mol for H₂).

5.70 moles H₂ x 2.016 g/mol = 11.4912 g of H₂

Thus, 11.4912 grams of hydrogen are necessary to react with 2.85 moles of CO.

Answer 2

CO+2 H2=CH3OH

2.85 mol Co x (2mol H2/1 mol Co)=5.70 mol just concert to grams

5.70 mol H2 x (2 g H2/1 mol H2) =11.40 grams of H2