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Consider the following balanced chemical reaction: 2 H2(g) + CO (g) -> CH4O (1). If

6.12 g of H₂ reacts with excess CO, how many grams of CH4O can be produced?
Select one:
a. 16.5g
b. 27.29
c. 64.5g
d. 48.6 g
e. 75.8 g

User Lelon
by
7.7k points

1 Answer

9 votes

Answer:

d

Step-by-step explanation:

2H₂(g) +CO(g) → CH₄O (l)

Since H₂ was reacted with excess CO, H₂ is the limiting reagent. This means that the amount of product formed is dependent on the amount, i.e. the number of moles, of H₂.

The number of moles of H₂ can be calculated by taking the mass divided by its Mr (relative molecular mass).

Mr of H₂= 2(1)= 2

Moles of H₂ (g)

= 6.12 ÷2

= 3.06 mol

From the balanced equation, 2 moles of H₂(g) produces 1 mole of CH₄O(g).

Since we have 3.06 moles of H₂(g),

Moles of CH₄O (l) produced

= 3.06 ÷2

= 1.53 mol

Mr of CH₄O

= 12 +4 +16

= 32

Mass= mole ×Mr

Mass of CH₄O (l) produced

= 1.53(32)

= 48.96 g

Thus, d would be the best option.

User Abdoulsn
by
8.3k points