Question

What volume will 2.0 mol H2(g) occupy at 40.0 C 0.50=atm pressure?

plza nswer asap in English not in Hindi plz

Answer 1

Explanation:

n= 2 mol

T= 273+40= 313k

P = 0.50atm

using PV= nRT

(0.50atm)×V = (2mol)× (8.314J/Kmol) ×(313k)

V = 10.409L

Answer 2

Pressure (P) = 0.5 atm

Number of moles (n) = 2

Temperature (∅) = 40°C = 313 K

Volume (V) = unknown

Assuming that the given Hydrogen gas is an ideal gas, we can say that :

VP = nR∅

V = nR∅/P

V = (2×8.31×313)/0.5

V = 5202.06/0.5

V = 10404.12 m^3

V = 10.4 L

Hence, the volume of the gas is 10.4L