<u>Answer:</u> The mass of produced is 9910.5 g
<u>Explanation:</u>
- <u>For </u><u>:</u>
Molarity is calculated by using the equation:
......(1)
Molarity of = 3.0 M
Volume of solution = 25.0 L
Putting values in equation 1, we get:
- <u>For </u><u>:</u>
The ideal gas equation is given as:
.......(2)
where,
P = pressure of the gas = 0.68 atm
V = volume of gas =
n = number of moles of gas = ? moles
R = Gas constant = 0.0821 L.atm/mol.K
T = temperature of the gas = 298 K
Putting values in equation 2, we get:
For the given chemical equation:
By stoichiometry of the reaction:
If 1 mole of reacts with 1 mole of
So, 75 moles of will react with = of
As the given amount of is more than the required amount. Thus, it is present in excess and is considered as an excess reagent
Thus, is considered a limiting reagent because it limits the formation of the product.
By the stoichiometry of the reaction:
If 1 mole of produces 1 mole of
So, 75 moles of will produce = of
The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:
We know, molar mass of = 132.14 g/mol
Putting values in above equation, we get:
Hence, the mass of produced is 9910.5 g