Question

Calculate the total pressure in a mixture of 8g of dioxygen

Answer 1

Answer:56.025 bar

Explanation:

wt. of O2 =8g

nO2 =8/32 =0.25

wt. of H2 =4g

nH2 = 4/2 = 2 moles

total no. of moles = 2+0.25

                            =2.25

v=1dm^3=1L

T= 27 degree =300K

PV=nRT

P * 1 = 2.25*0.083*300

P= 56.025 bars

Answer 2

HLO MATE HERE IS UR ANSWER.

GIVEN DATA :

Volume (v) = 1dm^3.

Temperature (T) = 27degreeC + 273= 300k

Gas constant(R) = 0.083 bar dm^3k^-1 mol^-1

No .of moles of O2, no2= 8/32=0.25.

No .of moles ofH2,nH2 =4/2 = 2.

Total no.of moles ,n = no2 +nH2=0.25 + 2 = 2.25

From ideal gas equation PV= nRT

===> p= nRT/v

====> 2.25× 0.083× 300/1

=====> 56. 025bar.