Problem: Consider the following reaction: CH3OH (g) → CO (g) + 2 H 2 (g)       ΔH = +90.7 kJ(d) How many kilojoules of heat are released when 50.9 g of CO(g) reacts completely with H 2 (g) to form CH3OH(g) at constant pressure?

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FREE Expert Solution

We’re being asked to determine the heat (q) absorbed by the reaction of 50.9 g CO

The given reaction is:

CH­3OH (g)  CO(g) + 2 H2(g); ΔH = +90.7 kJ


From the balanced equation, we can see that the given ΔH˚rxn (+90.7 kJ) corresponds to 1 mole of CO


Recall that at constant pressure, heat is equivalent to enthalpy.



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Problem Details

Consider the following reaction: 
CH3OH (g) → CO (g) + 2 H 2 (g)       ΔH = +90.7 kJ

(d) How many kilojoules of heat are released when 50.9 g of CO(g) reacts completely with H 2 (g) to form CH3OH(g) at constant pressure?

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