What is the mass of the solid NH4Cl formed when 75.5 g of NH3 is mixed with an equal mass of HCl? What is the volume of the gas remaining, measured at 14.0°C and 752 mmHg? What gas is it? NH3(g) + HCl(g) → NH4Cl(s) What is the mass of the NH4Cl produced?

Answer : The volume of the gas remaining is 56.5 liters.

The gas is hydrochloric acid and the formula of the gas is HCl.

The mass of produced is, 110.7 grams.

Explanation :

The balanced chemical reaction will be:

First we have to calculate the moles of and HCl

Molar mass of NH_3 = 17 g/mole

and,

Molar mass of HCl = 36.5 g/mole

Now we have to calculate the limiting and excess reagent.

From the balanced reaction we conclude that

As, 1 mole of HCl react with 1 mole of

So, 2.07 mole of HCl react with 2.07 mole of

From this we conclude that, is an excess reagent because the given moles are greater than the required moles and HCl is a limiting reagent and it limits the formation of product.

The remaining moles of HCl gas = 4.44 - 2.07 = 2.37 moles

Now we have to calculate the volume of the gas remaining.

Using ideal gas equation :

PV = nRT

where,

P = Pressure of gas = 752 mmHg = 0.989 atm     (1 atm = 760 mmHg)

V = Volume of gas = ?

n = number of moles of gas = 2.37 moles

R = Gas constant = 0.0821 L.atm/mol.K

T = Temperature of gas =

Putting values in above equation, we get:

V = 56.5 L

Now we have to calculate the moles of

As, 1 mole of HCl react with 1 mole of

So, 2.07 mole of HCl react with 2.07 mole of

Now we have to calculate the mass of

Molar mass of = 53.5 g/mole

Thus, the volume of the gas remaining is 56.5 liters.

The gas is hydrochloric acid and the formula of the gas is HCl.

The mass of produced is, 110.7 grams.

the ratio of the conjugate base to the acid required to attain the desired ph.