Answer:
The answer to your question is 98.9 %
Explanation:
Data
moles of methane = CH₄ = 2.0
excess air
Percent yield = ?
mass of CO₂ = 87 g
- Balanced chemical reaction
CH₄ + 2O₂ ⇒ CO₂ + 2H₂O
Reactants Elements Products
1 C 1
4 H 2
4 O 2
- Calculate the molar mass of CH₄
CH₄ = 12 + 4 = 16 g
- Convert the moles to mass
16 g of CH₄ ----------------- 1 mol
x ----------------- 2 moles
x = (2 x 16) / 1
x = 32 g of CH₄
-Calculate the theoretical formation of CO₂
16 g of CH₄ ----------------- 44 g of CO₂
32 g of CH₄ ---------------- x
x = (32 x 44) / 16
x = 88 g of CO₂
-Calculate the Percent yield
Percent yield = Actual yield/Theoretical yield x 100
Percent yield = 87/88 x 100
Percent yield = 98.9 %
the equilibrium concentration of H₂(g) at 700°C = 0.00193 mol/L
0.00193 mol/L
Given that:
numbers of moles of H₂S = 0.59 moles
Volume = 3.0-L
Equilibrium constant = 9.30 × 10⁻⁸
The equation for the reaction is given as :
2H₂S ⇄ 2H₂(g) + S₂(g)
The initial concentration of H₂S =
The initial concentration of H₂S =
= 0.1966 mol/L
The ICE table is shown be as :
2H₂S ⇄ 2H₂(g) + S₂(g)
Initial 0.9166 0 0
Change -2 x +2 x + x
Equilibrium (0.9166 - 2x) 2x x
(since 2x < 0.1966 if solved through quadratic equation)
The equilibrium concentration for H₂(g) = 2x
∴
= 0.00193 mol/L
Thus, the equilibrium concentration of H₂(g) at 700°C = 0.00193 mol/L
To know more about equilibrium concentration
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Mixture: matter than is composed of two or more substances that can be separated by physical means (ex; let's say you have a jar of red and blue marbles. this is a mixture. You can separate the colors with your hands (physical means.))
Compound: a substance in which two or more atoms are chemically combined in a fixed proportion (ex: water is a compound that consists of the element hydrogen and the element oxygen).
The answer is <span>Fluorine my dude
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