Question

1) If an ideal gas has a pressure of 6.83 atm, a temperature of 475 K, and a volume of 60.47 L, how many moles of gas are in the sample?

2) Solid ammonium chloride, NH4Cl, is formed by the reaction of gaseous ammonia, NH3, and hydrogen chloride, HCl.
NH3(g)+HCl(g)⟶NH4Cl(s)
A 6.00 g sample of NH3 gas and a 6.00 g sample of HCl gas are mixed in a 2.00 L flask at 25 ∘C.
How many grams of NH4Cl will be formed by this reaction?

Answer 1

1. To find the number of moles of gas in a sample, you can use the Ideal Gas Law: PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature in kelvin.
Rearranging the equation to solve for n, we get:

n = PV / RT

Plugging in the given values, we get:

n = (6.83 atm * 60.47 L) / (0.0821 Latm/molK * 475 K)
n = 0.759 mol

So, there are 0.759 moles of gas in the sample.

2. To find the amount of solid ammonium chloride formed in the reaction, we can use the balanced chemical equation:
NH3(g) + HCl(g) → NH4Cl(s)

1 mole of NH3 reacts with 1 mole of HCl to form 1 mole of NH4Cl.

First, find the number of moles of NH3 and HCl in the reaction:

NH3: 6.00 g / 17.03 g/mol = 0.3501 mol
HCl: 6.00 g / 36.46 g/mol = 0.1645 mol

Since the reaction requires an equal amount of NH3 and HCl, we can use the smaller value for the number of moles, which is 0.1645 mol.

The amount of solid ammonium chloride formed can be found by multiplying the number of moles by the molar mass of NH4Cl:

NH4Cl: 0.1645 mol * 53.49 g/mol = 8.808 g

So, 8.808 g of NH4Cl will be formed by the reaction