Consider the following reaction: CH3OH(g) ----> CO(g) + 2H2 (g) (delta H =+90.7k

Question

Consider the following reaction:

CH3OH(g) ----> CO(g) + 2H2 (g)    (delta H =+90.7k)
A) is heat absorbed or released in the course of this reaction?
b) calculate the amount of heat transferred when 45.0g of CH3OH(g)is decomposed by this reaction at constant pressure.
c) for a given sample of CH3OH, the enthalpy change on reaction is25.8kj. how many grams of hydrogen gas are produced? what is thevalue of delta H for the reverse of the previous reaction?
d) how many kilojoules of heat are released when 50.9 g of CO(g)reacts completely with H2O(g) to form CH3OH(g) at constantpressure?

Explanation / Answer

a) During this reaction, heat is absorbed, because the change inenthalpy is positive. b) 45.0 grams (1 mole/31.0 g)(90.7 kJ/1 mole) = 131.2 kJ heatabsorbed c) 25.8 kJ (2 moles H2/90.7 kJ) (2.00 grams/1 mole H) = .569 gramsH2 gas produced Delta H for the reverse reaction would be -25.8 kJ

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