The amount of heat (in KJ) released when 3.5 moles of CH₄ react is 3115 KJ
<h3>Balanced equation</h3>
CH₄ + 2O₂ -> CO₂ + 2H₂O ΔH = 890 KJ
From the balanced equation above,
1 mole of CH₄ reacted to release 890 KJ of heat energy.
<h3>How to determine the heat energy released by 3.5 moles of CH₄</h3>
From the balanced equation above,
1 mole of CH₄ reacted to release 890 KJ of heat energy
Therefore,
3.5 moles of CH₄ will react ro release = 3.5 × 890 = 3115 KJ of heat energy
Thus, 3115 KJ of heat energy were released from the reaction
Learn more about enthalpy change:
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Answer:
x = 5.5
Step-by-step explanation:
Based on the Mid-segment theorem of a triangle, we would have the following:
EF = 2(AB)
AB = 7
EF = 2x + 3
Plug in the values
2x + 3 = 2(7)
Solve for x
2x + 3 = 14
Subtract 3 from each side
2x + 3 - 3 = 14 - 3
2x = 11
2x/2 = 11/2
x = 5.5
The answer to your question is 343.6g
Answer: Parallel
I believe that if you set up these equations into y = mx + b form, you're able to notice that the slope is the same for each equation. That causes the answer to be parallel
