Calculate the amount of heat transferred when 24.0g of ch3oh(g) is decomposed by this reaction at constant pressure. for a given sample of ch3oh , the enthalpy change during the reaction is 82.6kj . what mass of methane gas is produced? how many kilojoules of heat are released when 38.7g of ch4(g) reacts completely with o2(g) to form ch3oh(g) at constant pressure?

94,4 kJ of heat transferred.

10,5 g of CH₄ gas are produced.

304 kJ are released.

Explanation:

The reaction is:

2 CH₃OH(g) → 2 CH₄(g) + O₂(g) ΔH = +252 kJ

24,0 g of CH₃OH(g) are:

24,0g CH₃OH× = 0,749 moles of CH₃OH(g)

As two moles of CH₃OH(g) transferred +252 kJ, 0,749 moles of CH₃OH(g) transferred:

0,749 molesCH₃OH× = 94,4 kJ

When 2 moles of CH₄ are produced, the enthalpy change is +252 kJ. 82,6 kJ are:

82,6kJ×= 0,656 moles of CH₄

0,656 moles of CH₄ are:

0,656 moles of CH₄× = 10,5 g of CH₄

38,7 g of CH₄(g) are:

38,7g CH× = 2,41 moles of CH₄(g)

As two moles of CH₄ released 252 kJ, 2,41 moles of CH₄(g) released:

2,41 moles CH₄× = 304 kJ

I hope it helps!

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