Answer:
The acetylene must be fill at 315 atm.
Explanation:
Given data:
Pressure of oxygen =P₁= 135 atm
Volume of oxygen = V₁=7.00 L
Volume of acetylene = V₂=3.00 L
Pressure of acetylene =P₂= ?
Solution:
According to Boyle's law
P₁V₁ = P₂V₂
P₂ = P₁V₁/V₂
P₂ = 135 atm × 7.0 L / 3.00 L
P₂ = 945 atm. L/ 3.00 L
P₂ = 315 atm
The acetylene must be fill at 315 atm.
Percentage yield = (actual yield / theoretical
yield) x 100%<span>
The balanced equation for the reaction is,
CH₄(g) + Cl₂<span>(g) </span>→ CH₃Cl(g)
+ HCl(g)</span><span>
Since there is excess of Cl₂ gas, we can assume that all of CH₄ gas are reacted.</span><span>
Moles of CH₄(g) = mass / molar mass</span><span>
= 25.0 g / 16 g/mol
= 1.5625 mol
The stoichiometric ratio between CH₄(g) and CH₃Cl(g)
is 1 : 1</span><span>
Hence moles of CH₃Cl(g) = 1.5625 mol</span><span>
Molar mass of CH₃Cl(g) = 50.5 g/mol</span><span>
Mass of CH₃Cl(g) = number of moles x molar mass</span><span>
= 1.5625 mol x 50.5 g/mol
<span>
= 78.9 g</span>
Hence theoretical yield = 78.9 g
Actual yield = 45.0 g
Hence,
<span> Percentage yield = (45.0 g / 78.9 g) x 100% </span>
<span>
= 57.03%</span></span>
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