Question

A mixture containing 2.65 g each of CH4(g), C2H4(g) and C4H10(g) is contained in a 1.50...

A mixture containing 2.65 g each of CH4(g), C2H4(g) and C4H10(g) is contained in a 1.50 L flask at a temperature of 25°C. (a) Calculate the partial pressure of each of the gases in the mixture. PCH4 = atm PC2H4 = atm PC4H10 = atm (b) Calculate the total pressure of the mixture.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

mass of each gas = 2.65g

moles of Ch4 = 2.65g/molar mass

= 2.65/16

= 0.1656

moles of C2H4 = 2.65/28

=0.09464

moles of C4H10 = 2.65/58

= 0.04568

Partial pressure of methane = nRT/V

= 0.1656mol x 0.0821 L.atm/mol.K x 298K/ 1.50L

= 2.701 atm

Partial pressure of C2H4 = nRT/V

= 0.09464mol x 0.0821 L.atm/mol.K x 298K/ 1.50L

= 1.543atm

Partial pressure of C4H10 = nRT/V

= 0.04568mol x 0.0821 L.atm/mol.K x 298K/ 1.50L

= 0.7450atm

Total pressure = 0.7450 + 1.543 +2.701

= 4.989 atm

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A mixture containing 0.768 mol He(g), 0.286 mol Ne(g), and 0.116 mol Ar(g) is confined in...
A mixture containing 0.768 mol He(g), 0.286 mol Ne(g), and 0.116 mol Ar(g) is confined in a 10.00-L vessel at 25 ∘C. Calculate the partial pressure of He in the mixture. P= atm Calculate the partial pressure of Ne in the mixture. P= atm Calculate the partial pressure of Ar in the mixture. P= atm Calculate the total pressure of the mixture. P= atm
2a) A mixture of hydrogen and krypton gases, in a 5.66 L flask at 11 °C,...
2a) A mixture of hydrogen and krypton gases, in a 5.66 L flask at 11 °C, contains 0.623 grams of hydrogen and 8.50 grams of krypton. The partial pressure of krypton in the flask is atm and the total pressure in the flask is atm b) A mixture of argon and neon gases is maintained in a 6.51 L flask at a pressure of 1.94 atm and a temperature of 74 °C. If the gas mixture contains 6.64 grams of...
A gas mixture of 16.0 g of CH4 and 30.0 g of C2H6 are at standard...
A gas mixture of 16.0 g of CH4 and 30.0 g of C2H6 are at standard temperature and pressure. What is the partial pressure of CH4 in the mixture? a) 0.125 atm b) 0.250 atm c) 0.500 atm d) 0.750 atm e) 1.00 atm
1. A 48500 mL cylinder containing C4H8 at a pressure of 1.50 atm is connected by...
1. A 48500 mL cylinder containing C4H8 at a pressure of 1.50 atm is connected by a valve to 62800 mL cylinder containing O2 at 6.00 atm pressure. Calculate the partial pressure (atm) of C4H8 when the valve is opened. 2. A 91.0 L cylinder containing C4H10 at a pressure of 266.0 torr is connected by a valve to 8.00 L cylinder containing C3H6 at 0.400 atm pressure. Calculate the partial pressure (torr) of C4H10 when the valve is opened....
The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) CH4(g) +...
The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) CH4(g) + CCl4(g) Calculate the equilibrium partial pressures of all species when CH2Cl2(g) is introduced into an evacuated flask at a pressure of 0.856 atm at 350 K. PCH2Cl2 = ________ atm PCH4 = _________ atm PCCl4 = _______ atm
Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown amount...
Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown amount of propane, C3H8) were added to the same 10.0-L container. At 23.0 ∘C, the total pressure in the container is 4.40 atm . Calculate the partial pressure of each gas in the container. Express the pressure values numerically in atmospheres, separated by commas. Enter the partial pressure of methane first, then ethane, then propane. A gaseous mixture of O2 and N2 contains 37.8 %...
A mixture containing 0.770 mol He(g), 0.244 mol Ne(g), and 0.119 mol Ar(g) is confined in...
A mixture containing 0.770 mol He(g), 0.244 mol Ne(g), and 0.119 mol Ar(g) is confined in a 10.00-L vessel at 25 ∘C Part A Calculate the partial pressure of He in the mixture. Part B Calculate the partial pressure of Ne in the mixture Part C Calculate the partial pressure of Ar in the mixture. Part D Calculate the total pressure of the mixture
part a.) A mixture of neon and xenon gases is maintained in a 9.44 L flask...
part a.) A mixture of neon and xenon gases is maintained in a 9.44 L flask at a pressure of 3.71 atm and a temperature of 39 °C. If the gas mixture contains 10.5 grams of neon, the number of grams of xenon in the mixture is_____ g. part b.) The stopcock connecting a 3.94 L bulb containing hydrogen gas at a pressure of 8.05 atm, and a 4.18 L bulb containing neon gas at a pressure of 1.61 atm,...
1/ 0.987 mol sample of xenon gas at a temperature of 19.0 °C is found to...
1/ 0.987 mol sample of xenon gas at a temperature of 19.0 °C is found to occupy a volume of 28.2 liters. The pressure of this gas sample is .... mm Hg. 2/ A sample of nitrogen gas collected at a pressure of 477 mm Hg and a temperature of 278 K has a mass of 20.0 grams. The volume of the sample is ...... L. 3/ A 4.97 gram sample of carbon dioxide gas has a volume of 856...
Determine the number of moles of each gas present in a mixture of CH4 and C2H6...
Determine the number of moles of each gas present in a mixture of CH4 and C2H6 in a 2.00-L vessel at 25°C and 1.72 atm, given that the partial pressure of CH4 is 0.45 atm. What is the number of moles of CH4? mol What is the number of moles of C2H6? mol
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT