Problem: The value of ΔH° for the reaction below is +128.1 kJ:CH3OH(l) → CO(g) + 2H2(g)How many kJ of heat are consumed when 5.10 g of CO(g) is formed as shown in the equation?A) 0.182B) 162C) 8.31D) 23.3E) 62.0

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We are asked to calculate the kJ of heat that are consumed when 5.10 g of CO(g) is formed.

The reaction is already balanced: 

CH3OH(l) → CO(g) + 2 H2(g)

  • CO(g) has a coefficient of only 1. 
  • This means that +128.1 kJ is consumed per 1 mole of CO.
  • We are given the mass so we still need to convert it to moles


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Problem Details

The value of ΔH° for the reaction below is +128.1 kJ:

CH3OH(l) → CO(g) + 2H2(g)

How many kJ of heat are consumed when 5.10 g of CO(g) is formed as shown in the 

equation?

A) 0.182

B) 162

C) 8.31

D) 23.3

E) 62.0

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