Question

7.0 G of a gas at 300k and 1 ATM pressure occupies a volume of 4.1 litres what is the molecular mass of the gas​

Answer 1

✔✔Here is your answer ✔✔

PV= m/M RT. or. M=m×RT/PV

=7.0×0.082×300/1×4.1

=42

❌Mahir❌

Answer 2

Answer: 42g

Step-by-step explanation:

• Given:- m=7g, R=0.082, T=300K, P=1 atm and V=4.1 litres.
• We know the standard gas equation is

           PV=nRT and n=$\frac{given\ mass}{molecular\ mass}$

        ⇒PV=$\frac{m}{M}RT$

        ⇒ M=$\frac{mRT}{PV}$

        ⇒ M=$\frac{7*0.082*300}{1*4.1}$

        ∴ M= 42g

• Hence, the required molecular mass is 42 g.

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