Consider separate 1.0 L samples of the following gases at STP:
Cl2, C2H6, and Xe. Which of the following statements are true
regarding these gas samples?
1. The Xe gas molecules collide with the container walls most
frequently.
2. The Xe gas sample has the largest average kinetic energy.
3. Each Cl2 gas particle collision with the container wall is
more forceful as compared to each C2H6 and Xe collision.
4. The Cl2 gas sample has the most molecules of...
Consider separate 1.0 L samples of the following gases at STP:
Cl2, C2H6, and Xe. Which of the following statements are true
regarding these gas samples?
The C2H6 gas sample has the smallest average kinetic energy.
The mass of the gas in each container is the same.
The C2H6 gas molecules collide with the container walls most
frequently.
The C2H6 gas sample has the lowest density.
Each Cl2 gas particle collision with the container wall is more
forceful as compared...
At 1.00 atm pressure and 273 K one mole of gas should occupy
22.4 L. What volume would one mole of gas occupy at 21
oC and 1.00 atm?
In the Molar Mass of Magnesium experiment:
a) At the end of the reaction, the temperature was 21.5
oC (294.65 K), 99.2 mL of gas were formed, and the
pressure was 1.00 atm in the gas syringe. The Gas Constant has a
value of 0.08206 L atm/ (mol K) (Pay attention...
A 2.55 L sample of gas at STP contains hydrogen and oxygen
gases. The mole fraction of hydrogen is 0.60. When the sample is
combusted to form water, calculate the mass of water formed,
assuming complete reaction.
Calculate the density of oxygen, O2, under each of the following
conditions: STP 1.00 atm and 30.0 ∘C Express your answers
numerically in grams per liter. Enter the density at STP first and
separate your answers by a comma.
Part A
Calculate the density of oxygen, O2, under each of the following
conditions:
STP
1.00 atm and 35.0 ∘C
Express your answers numerically in grams per liter.
Part B
To identify a diatomic gas (X2), a researcher carried out the
following experiment: She weighed an empty 3.6-L bulb, then filled
it with the gas at 2.00 atm and 23.0 ∘C and weighed it
again. The difference in mass was 8.3 g . Identify the gas.
Express your answer as a chemical...
Calculate the density of oxygen, O 2 , under each of the
following conditions: STP 1.00 atm and 35.0 ∘ C Express your
answers numerically in grams per liter. Enter the density at STP
first and separate your answers by a comma.