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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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FREE Expert Solution

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


87% (83 ratings)
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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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Our tutors have indicated that to solve this problem you will need to apply the Thermochemical Equations concept. You can view video lessons to learn Thermochemical Equations. Or if you need more Thermochemical Equations practice, you can also practice Thermochemical Equations practice problems.

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Based on our data, we think this problem is relevant for Professor Gillespie's class at FIU.