Ammonium sulfate (NH4)2SO4 is made by reacting 25.0 L of 3.0 mol/L H2SO4 with 3.1× 103 L of NH3 at a pressure of 0.68 atm and a temperature of 298 K according to the following reaction . NH3(g) + H2SO4(aq) → (NH4)2SO4 (aq)

How many grams of ammonium sulfate are produced?

The mass of produced is 9910.5 g

Explanation:

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:

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

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