These are two questions and two answers.
Answers:
Explanation:
<u>1) Balanced chemical equation (given):</u>
- CO₂(g) + 4H₂(g) → CH₄(g) + 2H₂O(g)
<u>2) Part A: How many moles of methane are produced when 59.6 moles of carbon dioxide gas react with excess hydrogen gas? </u>
a)<u> Mole ratios:</u>
- 1 moles CO₂(g) : 1 mole CH₄(g)
b) <u>Proportion:</u>
- 1 moles CO₂ / 1 mol CH₄ = 59.6 moles CO₂ / x
⇒ x = 59.6 mol CH₄ ← answer
<u>3) Part B How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 42.1 moles of water vapor? </u>
a) <u>Mole ratios:</u>
- 4 mol H₂(g) : 2 mol H₂O(g)
b) <u>Proportion:</u>
- 4 mol H₂ / 2 mol H₂O = x / 42.1 mol H₂O
⇒ x = 42.1 × 4 / 2 moles CH₄ = 84.2 mol H₂ (g) ← answer
Density (p) = Mass / volume
P=295/15.625
=18.88
therefore p=18.88
They'd observe any new substances or new color, and temp. that is irreversible.
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Answer:
The concentration of CH₃OH in equilibrium is [CH₃OH] = <em>2,8x10⁻¹ M</em>
Explanation:
For the equilibrium:
CO (g) + 2H₂(g) ⇄ CH₃OH(g) keq= 14,5
Thus:
14,5 =
In equilibrium, as [CO] is 0,15M and [H₂] is 0,36M:
14,5 =
Solving, the concentration of CH₃OH in equilibrium is:
<em>[CH₃OH] = 0,28M ≡ 2,8x10⁻¹ M</em>
I hope it helps!
Is there multiple choice?