How many moles of gas must be forced into a 3.5 L ball to give it a gauge pressure of 8.8 psi at 22 ∘C? The gauge pressure is re
1 answer:
Answer : The number of moles of gas forced into a 3.5 L ball must be 2.28 moles.
Explanation :
Using ideal gas equation:
where,
P = pressure of gas = 23.3 psi = 1.58 atm
conversion used : (1 atm = 14.7 psi)
V = volume of gas = 3.5 L
T = temperature of gas =
n = number of moles of gas = ?
R = gas constant = 0.0821 L.atm/mole.K
Now put all the given values in the ideal gas equation, we get:
Therefore, the number of moles of gas forced into a 3.5 L ball must be 2.28 moles.
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Answer:
%age Yield = 85.36 %
Solution:
The Balance Chemical Reaction is as follow,
C₆H₁₂O + Acid Catalyst → C₆H₁₀ + Acid Catalyst + H₂O
According to Equation ,
100 g (1 mole) C₆H₁₂O produces = 82 g (1 moles) of C₆H₁₀
So,
4.0 g of C₆H₁₂O will produce = X g of C₆H₁₀
Solving for X,
X = (4.0 g × 82 g) ÷ 100 g
X = 3.28 g of C₆H₁₀ (Theoretical Yield)
As we know,
%age Yield = (Actual Yield ÷ Theoretical Yield) × 100
%age Yield = (2.8 g ÷ 3.28 g) × 100
%age Yield = 85.36 %
