Answer :
Answer:
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×[tex]\frac{1mol}{32,04186g}[/tex] = 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×[tex]\frac{+252 kJ}{2moles}[/tex] = 94,4 kJ
When 2 moles of CH₄ are produced, the enthalpy change is +252 kJ. 82,6 kJ are:
82,6kJ×[tex]\frac{2moles}{252 kJ}[/tex]= 0,656 moles of CH₄
0,656 moles of CH₄ are:
0,656 moles of CH₄×[tex]\frac{16,05 g}{1mol}[/tex] = 10,5 g of CH₄
38,7 g of CH₄(g) are:
38,7g CH×[tex]\frac{1mol}{16,05g}[/tex] = 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×[tex]\frac{+252kJ}{2moles}[/tex] = 304 kJ
I hope it helps!
We have that for the Question, it can be said that heat transferred and mass of methane gas is produced and kilojoules of heat are released is given as
- 0.75 moles heat change = 95 KJ
- CH4 in gm produced = 10.45 gm
- Heat= - 306 KJ
From the question we are told
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?
1)
Generally, the moles of methanol is
CH3OH moles =\frac{24}{ 32}
CH3OH moles= 0.75moles
Where
2 moles [tex]CH_3OH[/tex] heat change =252.8 KJ
Therefore
0.75 moles heat change = 252.8 x \frac{0.75}{2}
0.75 moles heat change = 95 KJ
2)
Gnerally Heat is 82.6 KJ
Therefore
CH3OH moles = CH4 moles produced
CH3OH moles= ( 82.6/252.8) x 2 = 0.654 moles
CH4 in gm produced = 0.654 x 16
CH4 in gm produced = 10.45 gm
3)
moles of CH4 = \frac{38.7}{16} = 2.42 moles
Therefore
heat = ( 252.8) x ( \frac{2.42}{2})
heat= - 306 KJ
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