3 seperate questions but i would highely appreciate some help on them and unders

Question

3 seperate questions but i would highely appreciate some help on them and understanding how to start/do them.

thank you

Phosgene (COCh) is colorless gas that smells like newly mown hay. It is a useful industrial chemical that was used as a chemical weapon in World War I. What is the density of phosgene at standard temperature and pressure (STP)? A sample of a gas occupies 455 mL at 55 °C and 735 Torr. What will be the temperature of the gas if it is transferred to a 1.25 L container at a pressure of 175 Torr? naly hre s n1B bulb, in which the gas pressure is 6.9 atmosheres anda smaller 9t bulib, n which the gas pressure is 6.02 atmospheres. The valve between the bulbs is then opened. What is the final pressure of the device if the temperature remains constant? 9L 6.02 atm 18L 6.93 atm

Explanation / Answer

1)

P = 1.0atm

T = 273 K

Molar mass of COCl2,

MM = 1*MM(C) + 1*MM(O) + 2*MM(Cl)

= 1*12.01 + 1*16.0 + 2*35.45

= 98.91 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:

1.0 atm *98.91 g/mol = density * 0.08206 atm.L/mol.K *273.0 K

density = 4.4152 g/L

Answer: 4.415 g/L

2)

Given:

Pi = 735 torr

Pf = 175 torr

Vi = 455.0 mL

= (455.0/1000) L

= 0.455 L

Vf = 1.25 L

Ti = 55.0 oC

= (55.0+273) K

= 328 K

use:

(Pi*Vi)/(Ti) = (Pf*Vf)/(Tf)

(735.0 torr*0.455 L)/(328.0 K) = (175.0 torr*1.25 L)/(Tf)

Tf = 214.5474 K

Answer: 214.5 K

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