Question

2.0 g of N2, H2 and 0.50 g of 9.0 g of O2 are placed in...

2.0 g of N2, H2 and 0.50 g of 9.0 g of O2 are placed in a container of 1.00 L to 27 degrees C, determine the total pressure in the container (presumed ideal gas PV = nRT). using the law of Dalton calculate the partial pressure of O2.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

given are the weights of nitrogen, hydrogen and oxygen gases.

we can calculate the number of moles of each gas as

number of moles = weight/molecular weight

number of moles of N2 (n1) = 2/28 = 0.0714 mol

number of moles of H2 (n2)= 0.5/2 = 0.25 mol

number of moles of O2 (n3)= 9/32 = 0.28125 mol

hence total number of moles(n) = 0.0714 + 0.25 + 0.28125 = 0.6 mol

now use ideal gas equation,

PV = nRT

P1 = 0.60.0821300 (temperature T = 27+273 = 300K)

P = 14.778 atm

now for partial pressure of O2

use dalton law,

Pi = yiP (here yi is mole fraction)

P3 = (0.28125/0.6)14.778

P3 = 6.9 atm

hence partial pressure of O2 is 6.9 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 of 2.00 g of H2 and 1.00 g of He is placed in a...
A mixture of 2.00 g of H2 and 1.00 g of He is placed in a 1.00 L container at 310 K. Calculate the partial pressure of each gas and the total pressure.
A gas mixture contains 0.70 mol of N2, 0.25 mol of H2, and 0.35 mol of...
A gas mixture contains 0.70 mol of N2, 0.25 mol of H2, and 0.35 mol of CH4. Calculate the pressure of the gas mixture and the partial pressure of each constituent gas if the mixture is in a 7.0 L vessel at 27 degrees celsius. A) Total pressure in the vessel (atm) B) Pressure of H2 (atm) C) Pressure of N2 (atm) D) Pressure of CH4 (atm)
A mixture of 0.200 g of H2, 0.800 g of N2, and 0.600 g of Ar...
A mixture of 0.200 g of H2, 0.800 g of N2, and 0.600 g of Ar is stored in a closed container at 2.0 atm and 10°C. What is the partial pressure of N2 in the container? ans: 0.40 atm please explain
A gas mixture contains 1.18 g N2 and 0.94 g O2in a 1.50-L container at 14...
A gas mixture contains 1.18 g N2 and 0.94 g O2in a 1.50-L container at 14 ∘C.​ A. Calculate the mole fraction of N2 B. Calculate the mole fraction of O2 C. Calculate the partial pressure of N2
At 2000 degrees celcius, the gas-phase equilibrium 2NO(g)=N2(g)+o2(g) has an equilibrium constant of Kc=2.4X10^3. Use this...
At 2000 degrees celcius, the gas-phase equilibrium 2NO(g)=N2(g)+o2(g) has an equilibrium constant of Kc=2.4X10^3. Use this information to answer the following. a) Determine the relationship between Kc and Kp for this equilibrium. What is the value of Kp? b) Determine the value of Kc for the reaction 1/2N2(g)+1/2O2(g)=NO(g). c) Determine the equilibrium concentrations of NO, N2, O2 when 0.200 mol NO(g) is placed into a (n evacuated) 1.000 L container and heated to 2000 degrees celcius.
At STP, air can be considered to be a mixture of ideal gases: 21.0% O2, 78.0%...
At STP, air can be considered to be a mixture of ideal gases: 21.0% O2, 78.0% N2, and 1.00% Ar by volume. a. Calculate the partial pressure of each gas at STP. b. Calculate the density of air in g L at STP.
1.) The equilibrium constant for the chemical equation N2(g)+3H2(g) <--> 2NH3(g) is Kp = 1.09 at...
1.) The equilibrium constant for the chemical equation N2(g)+3H2(g) <--> 2NH3(g) is Kp = 1.09 at 209 °C. Calculate the value of the Kc for the reaction at 209 °C. 2.) At a certain temperature, 0.3411 mol of N2 and 1.581 mol of H2 are placed in a 1.50-L container. N2(g)+3H2(g) <--> 2NH3(g) At equilibrium, 0.1801 mol of N2 is present. Calculate the equilibrium constant, Kc. 3.) At a certain temperature, the Kp for the decomposition of H2S is 0.748....
Part A: What is the mole fraction of O2 in a mixture of 15.1 g of...
Part A: What is the mole fraction of O2 in a mixture of 15.1 g of O2, 8.17 g of N2, and 2.45 g of H2? Part B: What is the mole fraction of N2 in a mixture of 15.1 g of O2, 8.17 g of N2, and 2.45 g of H2? Part C: What is the mole fraction of H2 in a mixture of 15.1 g of O2, 8.17 g of N2, and 2.45 g of H2? Part D:...
9. A 900 mL chamber contains 2.184 g of N2 and 1.45 g of O2 at...
9. A 900 mL chamber contains 2.184 g of N2 and 1.45 g of O2 at 22 °C. Calculate: a) the mole fractions of each gas b) the total gas pressure exerted by the mixture c) the partial pressures of each gas
At a certain temperature, 0.3611 mol of N2 and 1.701 mol of H2 are placed in...
At a certain temperature, 0.3611 mol of N2 and 1.701 mol of H2 are placed in a 4.50 L container. N2(g)+3H2(g)↽−−⇀2NH3(g) N 2 ( g ) + 3 H 2 ( g ) ↽ − − ⇀ 2 NH 3 ( g ) At equilibrium, 0.1401 0.1401 mol of N2 N 2 is present. Calculate the equilibrium constant, ?c K c .
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT