Question

What minimum amount of H2O (in grams) must be added to an empty, sealed 1.00 L...

What minimum amount of H2O (in grams) must be added to an empty, sealed 1.00 L container with normal atmospheric pressure (1.00 atm) to ensure that there is at least some liquid water in it, in addition to the vapor, after the container is heated to 100°C and equilibrium is established. Assume that water vapor approximately obeys the ideal gas law.

Science   Physics   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Since it obeys Ideal gas law, we have

where,

P = Vapor pressure of water = 1.00 atm

V = volume of container = 1.00 L

n = number of moles of water

R = universal gas constant = 8.314 J = 0.082 L. atm/(K.mol)

T = temperature in Kelvin = 100 +273 K = 373 K

thus, we get

the molar mass of water = 18 grams/mol

thus, the minimum amount of water is

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
What minimum amount of H2O (in grams) must be added to an empty, sealed 1.00 L...
What minimum amount of H2O (in grams) must be added to an empty, sealed 1.00 L container with normal atmospheric pressure (1.00 atm) to ensure that there is at least some liquid water in it, in addition to the vapor, after the container is heated to 100°C and equilibrium is established. Assume that water vapor approximately obeys the ideal gas law.
A 2.0 L-closed container at 300 K holds 100 cm3 of H2O(l). The equilibrium vapor pressure...
A 2.0 L-closed container at 300 K holds 100 cm3 of H2O(l). The equilibrium vapor pressure is found to be 0.0328 atm. What pressure of Ar gas must be placed in the container to double the equilibrium water vapor pressure to 0.0656 atm?
Pure NOCl gas was heated at 240°C in a 1.00−L container. At equilibrium the total pressure...
Pure NOCl gas was heated at 240°C in a 1.00−L container. At equilibrium the total pressure was 1.00 atm and the NOCl pressure was 0.64 atm. 2NOCl(g) ⇆ 2NO(g) + Cl2(g) (a) Calculate the partial pressure of NO and Cl2 in the system. b) Calculate the equilibrium constant KP.
If 1.00 mol of argon is placed in a 0.500-L container at 30.0 ∘C , what...
If 1.00 mol of argon is placed in a 0.500-L container at 30.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345(L2⋅atm)/mol2 and b=0.03219L/mol.
If 1.00 mol of argon is placed in a 0.500-L container at 29.0 ∘C , what...
If 1.00 mol of argon is placed in a 0.500-L container at 29.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas law) and the real pressure (as predicted by the van der Waals equation)? For argon, a=1.345(L2⋅atm)/mol2 and b=0.03219L/mol.
An industrial chemist introduces 9.7 atm H2 and 9.7 atm CO2 into a 1.00-L container at...
An industrial chemist introduces 9.7 atm H2 and 9.7 atm CO2 into a 1.00-L container at 25.0°C and then raises the temperature to 700.0°C, at which Keq = 0.534: H2(g) + CO2(g) ⇔ H2O(g) + CO(g) How many grams of H2 are present after equilibrium is established?
An industrial chemist introduces 3.4 atm H2 and 3.4 atm CO2 into a 1.00-L container at...
An industrial chemist introduces 3.4 atm H2 and 3.4 atm CO2 into a 1.00-L container at 25.0°C and then raises the temperature to 700.0°C, at which Keq = 0.534: H2(g) + CO2(g) ⇔ H2O(g) + CO(g) How many grams of H2 are present after equilibrium is established?
An industrial chemist introduces 7.8 atm H2 and 7.8 atm CO2 into a 1.00-L container at...
An industrial chemist introduces 7.8 atm H2 and 7.8 atm CO2 into a 1.00-L container at 25.0°C and then raises the temperature to 700.0°C, at which Keq = 0.534: H2(g) + CO2(g) ⇔ H2O(g) + CO(g) How many grams of H2 are present after equilibrium is established?
An industrial chemist introduces 1.6 atm H2 and 1.6 atm CO2 into a 1.00-L container at...
An industrial chemist introduces 1.6 atm H2 and 1.6 atm CO2 into a 1.00-L container at 25.0°C and then raises the temperature to 700.0°C, at which Keq = 0.534: H2(g) + CO2(g) ⇔ H2O(g) + CO(g) How many grams of H2 are present after equilibrium is established?
A) A 1.00 L flask is filled with 1.25 g of argon at 25 ∘C. A...
A) A 1.00 L flask is filled with 1.25 g of argon at 25 ∘C. A sample of ethane vapor is added to the same flask until the total pressure is 1.450 atm . What is the partial pressure of argon, PAr, in the flask? What is the partial pressure of ethane, Pethane, in the flask? b)To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 2.6-L bulb, then filled it with the...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT