Question

Pure hydrogen sulphide is stored in a tank of 100 litre capacity
at 20° C and 2 atm pressure. The mass of the gas will be
(a) 34 g (b) 340 g (c) 282.68 g (d) 28.24 g

Answer 1

Answer:

0.2825 kg

Explanation:

The given data :

Volume ( V ) = 100 liter = 0.001 * 100 m³  = 0.1 m³

Temperature ( T) =  20° C = 273 + 20 = 293 K

Pressure ( P ) = 2 atm = 2 * 1.01 * 10⁵ pa   = 202000 Pa

We know the ideal gas equation.

PV = mRT

m = mass of the gas

R = gas constant of H₂S = 243.96 J/KgK

Substituting the values in equation,

202000 * 0.1 = m * 243.96 * 293

m = $\frac{202000 * 0.1}{243.96*293}$    = 0.2825 kg

Answer 2

The mass of the gas will be 282.68 g.

Step by step explanation:

From the given,

Pressure of gas = 2 atm

Number of moles of hydrogen sulfide = 34

Mass of gas can be calculated by the following formula.

                      $\bold{\frac{PV}{RT}=\frac{m}{M}}$.......................(1)

P = Pressure of the gas = 2 atm

V = Volume of the gas = 100 L

R = Gas constant = 0.082 atm.L/mol.K

T = Temperature = 20 + 273 = 293K

M = Moles of gas = 34

Rearrange the equation (1) is as follows.

                     $\bold{m=\frac{mPV}{RT}}$.........................(2)

Substitute the all given values in equation (1)

                        $\Rightarrow =\frac{34\times 2\times 100}{0.0821\times 293}=282.68g$

Therefore, the mass of the gas will be 282.68 g.

Hence, "c" is the correct option.

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