Answer:
68.1% is percent yield of the reaction
Explanation:
The reaction of methane with oxygen is:
CH₄ + 2O₂ → CO₂ + 2H₂O
<em>Where 2 moles of oxygen react per mole of CH₄</em>
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Percent yield is:
Actual yield (28.2g CO₂) / Theoretical yield * 100
To solve this question we need to find theoretical yield finding limiting reactant :
<em>Moles CH₄:</em>
15.1g CH₄ * (1mol / 16.04g) = 0.9414 moles
<em>Moles O₂:</em>
81.2g * (1mol / 32g) = 2.54 moles
For a complete reaction of 0.9414 moles of CH₄ are needed:
0.9414 moles CH₄ * (2 mol O₂ / 1mol CH₄) = 1.88 moles of O₂. As there are 2.54 moles, O₂ is in excess and <em>CH₄ is limiting reactant</em>
In theoretical yield, the moles of methane added = Moles of CO₂ produced. That is 0.9414 moles CO₂. In grams = Theoretical yield:
0.9414 moles CO₂ * (44.01g / mol) = 41.43g CO₂
Percent yield: 28.2g CO₂ / 41.43g CO₂ * 100=
<h3>68.1% is percent yield of the reaction</h3>
John Dalton created the very first atomic theory. Dalton viewed atoms as tiny, solid balls. Dalton was an English school teacher who performed many experiments on atoms. 1.
Answer:
c. the same as
Explanation:
for a closed system:
⇒ ΔS > 0.....irreversible process
⇒ ΔSrev = ∫ dQ/T
for an irreversible process, ΔS is not the same as in a reversible process, since more than one reversible process is needed for the two ΔS to be equal.
⇒ ΔSirrev = ΔSrev1 + ΔSrev2 + ....
but if the initial and final states are the same, ΔS for an irreversible process can be calculated as if it were a reversible process.
⇒ ΔSirrev = ΔSrev
I believe the answer is yes