Methanol ch3oh which is used in racing cars and in fuel

Question

Methanol, CH₃OH, which is used in racing cars and in fuel cells, can be made by the reaction of carbon monoxide and hydrogen.

CO(g) + 2 H₂(g) → CH₃OH(l)

Suppose 373 g of CO and 67.0 g of H₂ are mixed and allowed to react. What mass of methanol can be produced? What mass of the excess reactant remains after the limiting reactant has been consumed?

_____________ g CH₃OH

____________ g excess reactant

2) For this reaction, 4.35 g hydrogen gas reacts with 40.2 g iodine.

hydrogen (g) + iodine (s)  hydrogen iodide (g)

What is the maximum mass of hydrogen iodide that can be formed? ____________ g

What is the FORMULA for the limiting reagent?

What mass of the excess reagent remains after the reaction is complete?___________ g

3)Consider this reaction, which occurs in the atmosphere and contributes to photochemical smog:

SO₂(g) + H₂O(l) →H₂SO₃(g)

If there is 14.24 g SO₂ and excess H₂O present, the reaction yields 14.4 g H₂SO₃. Calculate the percent yield for the reaction.

_______________________%

4)Glucose, C₆H₁₂O₆, reacts with oxygen to give CO₂ and H₂O. What mass of oxygen (in grams) is required for complete reaction of 40.0 g of glucose? What masses of carbon dioxide and water (in grams) are formed?

 _______g O₂

 _________g CO₂

_________ g H₂O