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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.

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)
###### 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

What scientific concept do you need to know in order to solve this problem?

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.

How long does this problem take to solve?

Our expert Chemistry tutor, Rae-Anne took 2 minutes and 43 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

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