Answer : The volume of gas needed are, 90 L
Explanation : Given,
Volume of = 60 L
Now we have to determine the volume of needed.
As we know that at STP, 1 mole of gas contains 22.4 L volume of gas.
The given balanced chemical reaction is:
By the stoichiometry we can say that, 2 moles of react with 3 moles of oxygen gas to give 2 moles of gas and 2 moles of water vapor.
From the balanced reaction we conclude that,
As, volume of react with volume of gas
So, volume of react with volume of gas
Thus, the volume of gas needed are, 90 L
The percent yield of indigo : 79.6%
<h3>Further explanation</h3>
Percent yield is the comparison of the amount of product obtained from a reaction with the amount you calculated
General formula:
Percent yield = (Actual yield / theoretical yield )x 100%
An actual yield is the amount of product actually produced by the reaction. A theoretical yield is the amount of product that you calculate from the reaction equation according to the product and reactant coefficients
Reaction
2C₁₀H₁₁NO₄ + 2H₂O → C₁₆H₁₀N₂O₂ + 2C₂H₄O₂ + 4H₂O
Actual yield = 1.87 g
Theoretical yield = 2.35 g
The percent yield of indigo :
Explanation:
As it is given that water level is same as outside which means that theoretically, P = 756.0 torr.
So, using ideal gas equation we will calculate the number of moles as follows.
PV = nRT
or, n =
=
= 0.0052 mol
Also, No. of moles =
0.0052 mol =
mass = 0.0104 g
As some of the water over which the hydrogen gas has been collected is present in the form of water vapor. Therefore, at
= 24 mm Hg
= atm
= 0.03158 atm
Now, P =
= 0.963 atm
Hence, n =
= 0.0056 mol
So, mass of = 0.0056 mol × 2
= 0.01013 g (actual yield)
Therefore, calculate the percentage yield as follows.
Percent yield =
=
= 97.49%
Thus, we can conclude that the percent yield of hydrogen for the given reaction is 97.49%.
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