Question

DO ALL PARTS OF THE QUESTION AND USE SIGNIFICANT FIGURES!!! IF YOU DO NOT DO THIS I WILL DOWNVOTE YOU!!!!

QUESTION 1 Save Answer Calculate the density of freon -12 (CF2Cl2) at 26.3 °C and 0.695 atm. density = _ g/L QUESTION 2 Save Answer What volume of O2 (at 0.916 atm and 20.3 °C) is produced by the decomposition of 4.52 kg of Hgo? 2 HgO(s) --> 2 Hg(1) + O2(g) V= __L

Answer 1

1)
P = 0.695atm
T= 26.3 oC
= (26.3+273) K
= 299.3 K

Molar mass of CF2Cl2,
MM = 1*MM(C) + 2*MM(F) + 2*MM(Cl)
= 1*12.01 + 2*19.0 + 2*35.45
= 120.91 g/mol

Lets derive the equation to be used
use:
p*V=n*R*T
p*V=(mass/molar mass)*R*T
p*molar mass=(mass/V)*R*T
p*molar mass=density*R*T

Put Values:
0.695 atm *120.91 g/mol = density * 0.08206 atm.L/mol.K *299.3 K
density = 3.4214 g/L
Answer: 3.42 g/L

2)

Molar mass of HgO,
MM = 1*MM(Hg) + 1*MM(O)
= 1*200.6 + 1*16.0
= 216.6 g/mol

mass of HgO = 4.52*10^3 g
mol of HgO = (mass)/(molar mass)
= 4.52*10^3/2.166*10^2
= 20.87 mol

According to balanced equation
mol of O2 formed = (1/2)* moles of HgO
= (1/2)*20.87
= 10.43 mol

Given:
P = 0.916 atm
n = 10.43 mol
T = 20.3 oC
= (20.3+273) K
= 293.3 K

use:
P * V = n*R*T
0.916 atm * V = 10.43 mol* 0.08206 atm.L/mol.K * 293.3 K
V = 274.0516 L
Answer: 274 L