Question

Determine the value of the following gas diffusivities using Hirschfelder equation: 1. Carbon dioxide /air at...

Determine the value of the following gas diffusivities using Hirschfelder equation:

1. Carbon dioxide /air at 310 K and 1.5x105 Pa.

2. Carbon monoxide/air at 310 K and 1.5x105Pa.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

where P = total pressure, atm
Mi = molecular weight
DAB = diffusivity, cm2/s
T = temperature, K
ΣVi = Sum of the diffusion volume for component i

For air:

  1. VA = 20.1.
  2. 2. Molecular weight = 29.0.
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
Carbon monoxide gas reacts with elemental oxygen gas to form carbon dioxide gas. In a 1.00...
Carbon monoxide gas reacts with elemental oxygen gas to form carbon dioxide gas. In a 1.00 L flask, 4.30 atm of carbon monoxide reacts with 2.50 atm of oxygen gas. a) write the balanced equation for this composition reaction b) Determine which is the limiting reactant in this composition reaction c) How many moles of gaseous product are produced by this reaction?
A 18.0-L tank of carbon dioxide gas (CO2) is at a pressure of 9.60 ✕ 105...
A 18.0-L tank of carbon dioxide gas (CO2) is at a pressure of 9.60 ✕ 105 Pa and temperature of 21.0°C. (a) Calculate the temperature of the gas in Kelvin. K (b) Use the ideal gas law to calculate the number of moles of gas in the tank. mol (c) Use the periodic table to compute the molecular weight of carbon dioxide, expressing it in grams per mole. g/mol (d) Obtain the number of grams of carbon dioxide in the...
A 22.0-L tank of carbon dioxide gas (CO2) is at a pressure of 9.90 ? 105...
A 22.0-L tank of carbon dioxide gas (CO2) is at a pressure of 9.90 ? 105 Pa and temperature of 18.0°C. (a) Calculate the temperature of the gas in Kelvin. _______ K (b) Use the ideal gas law to calculate the number of moles of gas in the tank. mol (c) Use the periodic table to compute the molecular weight of carbon dioxide, expressing it in grams per mole. ______ g/mol (d) Obtain the number of grams of carbon dioxide...
Propane gas is burned using air, both are at 25c and 1 atm. excess air is...
Propane gas is burned using air, both are at 25c and 1 atm. excess air is used. The products of combustion are carbon dioxide(gas) and vapor water along with excess oxygen and nitrogen exit the reactor at 1520 k. Predict the percentage of excess air (in % units not fractional) used in the steady flow combustion chamber. (Correct answer is 100% - please explain and show why)
The balanced equation for the reaction of iron (III) oxide with carbon monoxide to produce carbon...
The balanced equation for the reaction of iron (III) oxide with carbon monoxide to produce carbon dioxide and iron metal is given below. Fe2O3 (s) + 3 CO (g) --> 2 Fe (s) + 3 CO2 (g) Using the balanced equation, determine the mass of iron metal (Fe(s)) in grams that can be made if this reaction is performed using 225.3 grams of iron (III) oxide (Fe2O3) and 200.1 grams of carbon monoxide.
Propane gas is burned using air; both are at 25°C and 1 atm. 150% excess air...
Propane gas is burned using air; both are at 25°C and 1 atm. 150% excess air (ie 250% of the theoretical air) is used. The products of the combustion are carbon dioxide(gas) and vapor water along with the excess oxygen. Predict the adiabatic flame temperature, in degrees K, in the steady-flow combustion chamber. Use the thermodynamic data from your textbook, Appendix E for all the required data.
Exhaust gas from a combustion process is 70% Nitrogen, 15% Carbon Dioxide, 10% Carbon monoxide, and...
Exhaust gas from a combustion process is 70% Nitrogen, 15% Carbon Dioxide, 10% Carbon monoxide, and 5% Oxygen. The absolute pressure is 0.8 atmospheres. The temperature of the exhaust gas is T=240oF. Find: The specific gas constant R of the exhaust gas in units of ft*lbf/slug*R
An equilibrium mixture contains 0.500 mol of each of the products (carbon dioxide and hydrogen gas)...
An equilibrium mixture contains 0.500 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-L container. CO(g) +H20 (g) --> <-- CO2 (g) + H2 (g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished?
An equilibrium mixture contains 0.450 mol of each of the products (carbon dioxide and hydrogen gas)...
An equilibrium mixture contains 0.450 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-L container CO(g) + H2O(g) <===> CO2(g) + H2(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished?
An equilibrium mixture contains 0.650 mol of each of the products (carbon dioxide and hydrogen gas)...
An equilibrium mixture contains 0.650 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-L container. CO(g) + H2O(g) <-----> CO2(g) + H2(g) How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT