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

water and alcohols have similar properties because water molecules contain hydroxyl groups that can form hydrogen bonds with other water molecules and with alcohol molecules, and likewise alcohol molecules can form hydrogen bonds with other alcohol molecules as well as with water.