Question

1) 362.11 g of O2 are contained in a 3.00 L high pressure tank at a...

1) 362.11 g of O2 are contained in a 3.00 L high pressure tank at a temperature of 186°C. What is the pressure of the gas in torr?

2) A gas has a given volume. The moles of gas are doubled then the pressure is 1/3 of the original pressure. After the pressure change, the Kelvin temperature quadruples (increases 4 times of the original Kelvin temperature). By how much has the volume changed? Be specific (i.e. the volume is 1/3 of the original volume, the volume is 8 time greater, etc.). If you need more information to answer, explain what information is needed.

3) A helium balloon has a volume of 2.54 L at 1.04 atm and 24oC. The balloon is then released. Calculate the volume of the balloon (in L) when the pressure is 312 torr and the temperature is–47oC.

4) A vapor occupies a volume of 237.2 mL at a temperature of 90.6°C and a pressure of 734.6 torr. The mass of the condensed vapor is 0.978 g. Calculate the molar mass of the vapor (hint: Use the ideal gas law to find the number of moles).

5) A chemist mixed 10.00 g of a sodium carbonate solution with 10.00 grams of a hydrochloric acid solution in an open beaker. The reaction mixture fizzed. The final mass of the mixture was 19.31 g. Did this reaction violate the Law of Conservation of Mass? Why or why not? Be sure to explain your answer for full credit (hint – think common sense).

Homework Answers

Answer #1

1)

No of mol of O2 = 362.11/32 = 11.31 mol

P = nRT/V = (11.31*0.0821*(273.15+186))/3 =142.11 atm

   = 1.08*10^5 torr

2) n2 = 2 n1

p2 = p1/3

T2 = 4T1

V2 = ?

P1V1/T1n1 = p2v2/T2n2

let p1 = 1 , n1 = 1 , t1 = 1

(1*1/1*1) = (1/3)*V2 / (4*2)

V2 = 24V1

that means 24 times higher than initial

3)

2.54*1.04/(297.15) = (312/760)*V2/(273.15-47)

V2 = 4.89 L


4) PV = nRT

(734.6/760)*(237.2/1000) = (0.978/x)*0.0821*(273.15+90.6)

molarmass of vapour = 127.4 g/mol

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
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...
Part A A sample of ideal gas at room temperature occupies a volume of 27.0 L...
Part A A sample of ideal gas at room temperature occupies a volume of 27.0 L at a pressure of 202 torr . If the pressure changes to 1010 torr , with no change in the temperature or moles of gas, what is the new volume, V2? Express your answer with the appropriate units. Part B If the volume of the original sample in Part A (P1 = 202 torr , V1 = 27.0 L ) changes to 60.0 L...
A .276g sample of a CoCO3 heterogenous mixture was placed into a gas generator, the total...
A .276g sample of a CoCO3 heterogenous mixture was placed into a gas generator, the total mass which is 87.719g (containing the CaCO3 sample and the beaker, an HCl solution, and the test tubes) is connected to a gas collection appartus. The following data were collected following the reaction Volume of wet CO2: 37/7 mL Temperature of wet CO2: 20.0 degrees celcius Pressure of wet CO2: 770 Torr Mass of gas generator after reactionL 87.642g Answer parts A-G and show...
Electrolysis problem. Calculate the partial pressure of H2 (using barometric pressure and vapor pressure of water)...
Electrolysis problem. Calculate the partial pressure of H2 (using barometric pressure and vapor pressure of water) and the Faradays required to generate 0.01358 moles of hydrogen gas given the following information. 10 mL of 3 M H2SO4 was diluted in 100 ml. 49.8 mL of this solution was used in electrolysis (initial buret reading was at 50 mL and final was at 0.2). The electrolysis was conducted at 20 V for seven minutes and forty seconds. I calculated the moles...
In an experiment, 9.25 L of N2 is saturated with water vapor at 22C and then...
In an experiment, 9.25 L of N2 is saturated with water vapor at 22C and then compressed to half its volume at constant temperature. a. What is the partial pressure of H2O in the compressed gas mixture? __________ torr b. What mass of water vapor condenses to liquid? __________ grams
A weather balloon contains 222 L of He gas at 20. °C and 760. mmHg. What...
A weather balloon contains 222 L of He gas at 20. °C and 760. mmHg. What is the volume of the balloon when it ascends to an altitude where the temperature is -40. °C and 540. mmHg? 1 What volume does 12.5 g of Ar gas at a pressure of 1.05 atm and a temperature of 322 K occupy? Would the volume be different if the sample were 12.5 g of He gas under the same conditions? How many moles...
1. A sample of gas with an initial volume of 28.2 L at a pressure of...
1. A sample of gas with an initial volume of 28.2 L at a pressure of 728 mmHg and a temperature of 301 K is compressed to a volume of 14.9 L and warmed to a temperature of 375 K. What is the final pressure of the gas? 2. A gas sample with a volume of 5.3 L has a pressure of 725 mmHg at 24C. What is the pressure of the sample if the volume remains at 5.3 L...
1. A sample of gas occupies 5.27 L at a pressure of 2.63 atm. Determine the...
1. A sample of gas occupies 5.27 L at a pressure of 2.63 atm. Determine the new pressure (in atm) of the sample when the volume changes to 4.56 L at constant temperature. 2. Determine the temperature (in °C) of a 4.77-mol sample of CO2 gas at 6.11 atm in a container with a volume of 47.2 L. 3. Convert the pressure measurement of 2395 mmHg into units of atmospheres. 4. A latex balloon has a volume of 87.0 L...
0.727 g of an unknown metal is reacted with excess concentrated hydrochloric acid according to the...
0.727 g of an unknown metal is reacted with excess concentrated hydrochloric acid according to the reaction below.  0.335 L of hydrogen gas was collected over water on a day when the temperature was 25.0 oC and the pressure was 0.98 atm. The vapor pressure of water at 25.0 oC is 23.8 torr. Report the partial pressure of hydrogen gas in atmospheres, the molar mass of the metal and the atomic symbol for the metal. The ideal gas law constant R...