How do you calculate the volume of 66.5 g of carbon monoxide at STP?
At #"1.20 atm"#, and a temperature of #"27"^@"C"#, #"75.0 L NH"_3"# gas is produced by the reaction between #"N"_2"# gas and #"H"_2"# gas. How many moles and what volume of #"N"_2"# and #"H"_2"# are required to produce #"75.0 L NH"_3"#?
At an altitude for which ambient pressure is #0.700*atm#, and a temperature of #270.15*K#, a balloon contains #3.00*mol# of gas... What is the volume of the balloon....?
#CO_2# gas, in the dry state, may be produced by heating calcium carbonate. #CaCO_3 (s)DeltaCaO(s) + CO_2(g)#. What volume of #CO_2#, collected dry at 55 C and a pressure of 774 torr, is produced by complete thermal decomposition of 10.0 g of #CaCO_3#?
What pressure is required to compress 196.0 liters of air at 1.00 atmosphere into a cylinder whose volume is 26.0 liters?
If an ideal gas has a pressure of 4.97 atm, a temperature of 481 K, and has a volume of 29.83 L, how many moles of gas are in the sample?
If an ideal gas has a pressure of 2.65 atm, a temperature of 92.55 Â°C, and has a volume of 51.43 L, how many moles of gas are in the sample?
Using the ideal gas formula, calculate the volume of 1.50 moles of a gas at 115 kPA and a temperature of 298K?
How can I do Charles' law experiment?
What is the new volume for a #50.4*mL# volume of gas, at #742*mm*Hg# pressure and #293.15*K#, for which conditions are changed to #"STP"#?
If the pressure on a gas is decreased by one-half, how large will the volume change be?
500.0 liters of a gas are prepared at 700.0 mmHg and 200.0 C. The gas is placed into a tank under high pressure. When the tank cools to 20.0 C, the pressure of the gas is 30.0 atm. What is the volume of the gas?
An ideal gas is made up of gas particles that have what properties?
If 2.30 g occupies 0.870 L at 690 torr and 37 degrees C. How would you calculate the molar mass?
How do you calculate the final pressure of a gas that is compressed from a volume of #"20.0 dm"^3# to #"10.0 dm"^3# and cooled from #100^@"C"# to #25^@"C"# if the initial pressure is #"1 bar"# ?
How do you calculate the pressure in atmospheres of 1.00 mol of argon in a .500-L container at 29.0Â°C?
What volume will 2.0 moles of nitrogen occupy at 720 torr and 20Â°C?
A gas occupies a volume of 0.2 L at 25 kPa. What volume will the gas occupy at 2.5 kPa?
What how do you find a pressure at STP and SATP?
Explain Boyle's law in terms of the kinetic theory?
Under a pressure of 200 kPa, a confined gas has a volume of 2,500 cubic meters. The pressure acting on the gas is increased to 500 kPa. What is the new volume of the gas if the temperature remains the same?
How does atmospheric pressure affect boiling points?
How many grams of sodium azide are needed to provide sufficient nitrogen gas to fill aÂ 50.0Â Ã—Â 50.0Â Ã— 25.0 cm bag to a pressure ofÂ 1.15Â atm atÂ 25.0Â Â°C?
How does air exert pressure?
What are the postulates of the kinetic-molecular theory?
Which graph shows the relationship between the temperature and volume of a gas according to Charles's law?
8.00 L of a gas is collected at 60.0Â°C. What will be its volume upon cooling to 30.0Â°C?
#0.250*mol# quantities of dinitrogen and sulfur dioxide are enclosed in a #2.5*L# vessel at a temperature of #300*K#. What are the partial pressures of each gas, and what is the total pressure?
How Charles' law was discovered?
Abreathing mixture used by deep sea divers contains helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen at 1 atmosphere if P He- 609.5 mm Hg and P #CO_2# = 0.5 mm Hg?
A gaseous compound composed of sulfur and oxygen, which is linked to the formation of acid rain, has a density of 3.58 g/L at STP. What Is the molar mass of this gas?
How do the gas laws operate in scuba diving? I mean to exclude the rule of never holding your breath...
What is the change in volume when 4.8 L sample of #N_2(g)# is heated from 388.0Â°C to 700Â°C?
The temperature of a balloon increases from 25 K to 50 K. What will the final volume of the balloon be if it was 1 L before the temperature change?
What are 2 assumptions made by ideal gas laws that are violated by real gases?
What is the molar volume of 3.01 x 10(23) molecules of ethane (C2H6)?
A gas sample containing only SO2, PF3, and CO has the following mass percentage: 29.1 % SO2, 61.8 % PF3. How would you calculate the partial pressure in torr, of CO if the total pressure of sample is 684 torr?
How many atoms are in 131.97 liters of water vapor at STP?
How do you graph Boyle's law?
If a sample of 4 moles of gas has a pressure of 567.42 kPa and a volume of 12.0 L, what is its temperature?
A tank contains helium gas at 490 mm Hg, nitrogen gas at 0.75 atm, and neon at 520 torr. What is the total pressure in atm?
What is the change in entropy for an adiabatic expansion against an external pressure for an ideal gas?
The density of air #20# #km# above Earths surface is #92# #g##/##m^3.# The pressure of the atmosphere is #42# #mm# #Hg#, and the temperature is #-63# #Â°C#. What is the average molar mass of the atmosphere at this altitude?
If He(g) has an average kinetic energy of 6670 J/mol under certain conditions, what is the root mean square speed of Cl2(g) molecules under the same conditions?
What is the partial pressure of oxygen?
A certain gas mixture is held at #395^@ "C"# has the following initial partial pressures: #P_(Cl_2) = 351.4#, #P_(CO) = 342.0#, #P_(COCl_2) = 0#, all in #"torr"#. Find #K_P^@#?
If I have 5.6 liters of gas in a piston at a pressure of 1.5 atm and compress the gas until its volume is 4.8 L, what will the new pressure inside the piston be?
Why is Kelvin used in the ideal gas law?
An experiment shows that a 245mL gas sample has a mass of 0.436g at a pressure of 757 mmHg and a temperature of 29C.
What is the molar mass of the gas?
If the density of the gas is #"4 kg/m"^3# and its pressure is #1.2 xx 10^5 "N/m"^2#, how do I calculate the root-mean-square speed?
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