Question

A sample of 4.10 mLmL of diethylether (C2H5OC2H5 ; density=0.7134 g/mL) is introduced into a 5.10...

A sample of 4.10 mLmL of diethylether (C2H5OC2H5 ; density=0.7134 g/mL) is introduced into a 5.10 −L vessel that already contains a mixture of N2 and O2, whose partial pressures are PN2= 0.752 atm and PO2= 0.207 atm. The temperature is held at 35.0 ∘C, and the diethylether totally evaporates.

a.Calculate the partial pressure of the diethylether.

b. Calculate the total pressure in the container.

Hints; In problem 10.64 the diethyl ether starts out as a liquid and is then converted to a gas. Use the volume of the diethyl ether liquid and the density of the diethyl ether liquid to help you find the mass of the diethyl ether liquid which is equal to the mass of the dietheyl ether gas. Convert that mass to the number of moles of the diethyl ether gas. The volume of the container is the volume you use in the ideal gas law for part A. Use Dalton's law for part B.

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Liquid ethyl ether is introduced drop by drop into a 3.0 L closed container at 18...
Liquid ethyl ether is introduced drop by drop into a 3.0 L closed container at 18 degrees Celsius. After 122 drops of ethyl ether are added. No more evaporates and one drop is present in the container. What is the pressure in the container. The volume of one drop is 0.05 ml and the density of ethyl ether is 0.713 g/mL. The molar mass of ethyl ether is 74.12 g/ml. R=0.0821 The answer is 0.46 atm. Can you please show...
1 in = 2.5 cm. 1 atm = 760 torr density of mercy = 13.6 g/mL...
1 in = 2.5 cm. 1 atm = 760 torr density of mercy = 13.6 g/mL at 25 oC gravity = 9.8 m/s2 R = 0.082 L.atm/mol.K    PV = nRT            Force = mass x acceleration Pressure = Force/area Today’s atmospheric pressure is 32.0” of mercury. What is the pressure in ‘atm’ units? The burette used in the lab has a cross-section area of 1 cm2 so that a height of 1 cm provides a volume of 1 cm3 (that is...
Liquid Halothane has a density of 1.87 g/mL, and boils at 50.2 degrees celsius and 1.00...
Liquid Halothane has a density of 1.87 g/mL, and boils at 50.2 degrees celsius and 1.00 atm. A) If Halothane behaved as an ideal gas, what volume would 10.0 mL of Halothane occupy at 60 degrees celsius and 1.00 atm of pressure? (In Liters) B) What is the density in g/L of Halothane vapor at 55 degrees celsius and 1.00 atm of pressure?
A small gas cylinder containing CH4 (methane) gas is found to have a mass of 246.776g,...
A small gas cylinder containing CH4 (methane) gas is found to have a mass of 246.776g, and is used to bubble methane into a container that has been submerged in 22.0 C water. The volume of the gas that is inside the container at the end is 0.228L, and the gas cylinder weighs 246.622g. The barometric pressure of the room is 1.05atm. 1. Calculate the mass of CH4 that was released into the container. 2. Calculate the temperature of the...
A flask with a sample of gas at room temperature and pressure weighs 97.4842 g. The...
A flask with a sample of gas at room temperature and pressure weighs 97.4842 g. The same flask with air (density = 1.17 g/L) weighs 96.8848 g. The same flask filled with water (d = 0.998 g/mL) weighs 345.86 g. The pressure in the room is 0.989 atm and the temperature is 22.2 °C. 1. Calculate the volume of the flask. 2. Calculate the mass of the air that the flask can hold. 3. Calculate the mass of the empty...
96.1 g of solid iron reacts with 0.0500 L of water (density = 0.997 g/mL) to...
96.1 g of solid iron reacts with 0.0500 L of water (density = 0.997 g/mL) to form iron(III)oxide and hydrogen gas. If the reaction takes place in a 10.0 L container at 400.0 K, what pressure in atm would be measured? When 0.62 mols of aluminum metal react with 4.55 mols of HCl according to the reaction below what will be the final pressure (in atm) if the two substances react in a solid steel chamber with a volume of...
PART A A sample of 0.030 grams of magnesium is reacted with excess HCl at 25°C...
PART A A sample of 0.030 grams of magnesium is reacted with excess HCl at 25°C and 1.00 atm. The resulting gas is collected over water using an inverted buret. Will the student need to use a 25.00 mL or a 50.00 mL buret in this experiment? PART B A sample of helium and neon gas occupy 1.50 L container at 45.0ºC. Calculate the partial pressure of each gas if the total pressure is 1.55 atm and the mole fraction...
n this exercise, weighed samples of a solid unknown containing NaCl and NaHCO3 react with hydrochloric...
n this exercise, weighed samples of a solid unknown containing NaCl and NaHCO3 react with hydrochloric acid. The volume of the CO2 liberated by the reaction in the gas phase is measured with a gas collection syringe. From the volume we can calculate the number of moles of CO2 in the gas phase using the ideal gas approximation. Since the CO2 is generated in an aqueous environment (aqueous HCl), some CO2 will dissolve in the liquid phase. The amount of...
1) Use Henry's law to determine the molar solubility of helium at a pressure of 1.9...
1) Use Henry's law to determine the molar solubility of helium at a pressure of 1.9 atm and 25 ∘C. Henry’s law constant for helium gas in water at 25 ∘C is 3.70⋅10−4M/atm. 2) A 2.800×10−2M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.2 mL...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT