Question

Pure hydrogen sulphide is store in a tank of 100 litre capacity at 20°C and 2 atm pressure. The mass of the gas will be

Answer 1

Answer:

283.371 g

Explanation:

Given that:

Pressure = 2 atm

Temperature = 20°C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15  

So,  

T = (20 + 273.15) K = 293.15 K  

T = 293.15 K

Volume = 100 L

Using ideal gas equation as:

PV=nRT

where,  

P is the pressure

V is the volume

n is the number of moles

T is the temperature  

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

2 atm × 100 L = n × 0.0821 L.atm/K.mol × 293.15 K  

⇒n = 8.31 moles

Given that :

The gas is hydrogen sulfide.

Molar mass = 34.1 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$8.31= \frac{Mass\ taken}{34.1\ g/mol}$

$Mass= 283.371\ g$