can some one please help me please

Chemistry
Tutor: None Selected Time limit: 1 Day

What is the mass of a 8156.2 mL sample of hydrogen gas at 99.7oC and 69.49 kPa

What is the mass of 2.04 L of ammonia gas at STP?

What is the molar volume for a gas at -118.2oC and 2168.28 mmHg? 

What is the density of sulfur dioxide gas at STP?

Feb 7th, 2015

Please note that, I apply the equation of gases, as below:

P*V=n*R*T, where n is the number of mol of the gas, V is the volume occupied by the gas, P is the pressure exerted by the gas, R is the constant of the gases, namely R = 0.08206 liter*atm/ °K. So we have:

Question 1)

n = (P*V)/(R*T) = (0.68 * 8.1562) /( 0.08206*372.85) = 0.18 mol of H2 gas

then the mass of H2 is 0.18* 2 = 0.36 grams

Please note thatthe pressure is 69490/101325 = 0.68 atm

and the temperature is:

273.15+99.7= 372.85 °K


Question 2)

here we have molecular mass of ammonia (NH3) = 17,

so n= (P*V) / (R*T)= (1*2.04)/(0.08206*273.15) = 0.091 mol of NH3,

so the mass of ammonia is 0.091 * 17 = 1.55 grams of NH3 gas.

Please note that the STP condition are T = 273.15 °K and P = 1 atm.


Question 3)

here we can write:

V/n = R*T/P = 0.08206*154.95 / 2.853 = 4.46 liter/mol,

since the temperature is T = 273.15-118.2= 154.95, and the pressure P is 2168.28/760 = 2.853 atm.


Question 4)

here we have molecular mass of SO2 = 64,

density = (P* molecular mass) / (R*T) = (1*64)/(0.08206*273.15) = 2.855 grams/liter

Feb 7th, 2015

Studypool's Notebank makes it easy to buy and sell old notes, study guides, reviews, etc.
Click to visit
The Notebank
...
Feb 7th, 2015
...
Feb 7th, 2015
Mar 1st, 2017
check_circle
Mark as Final Answer
check_circle
Unmark as Final Answer
check_circle
Final Answer

Secure Information

Content will be erased after question is completed.

check_circle
Final Answer