Which chart would be accurate? A. Straight Line. B. Curved to the right. C. Curved to the left.
A. Straight Line.
200
How are pressure and volume related?
Inversely
200
What is the formula for Charles Law?
(V1/T1)=(V2/T2).
300
What is the R value for atm?
0.0821 atm * L/ mole * K
300
A 250 mL sample of oxygen is collected over water at 25 C and 760.0 torr presure. What is the presure of the dry gas alone? ( Vapor presure of water at 25 C = 23.8 torr?
760 - 23.8= 736.2 torr
300
How would you solve for P2?
P1*T1=P2*T2
P2= P1*T2/T1
300
A sample of oxygen gas occupies a volume of 250 mL at 740 torr pressure. What volume will it occupy at 800 torr pressure?
740 torr x 250 mL/ 800 torr=231 mL
300
A sample of neon gas occupies a volume of 752ml at 298K. What is the volume the gas will occupy at 323K if the pressure remains constant?
815 ml.
400
What mass of chlorine gas in grams, is contained in a 100.1 L tank at 27 C and 3.50 atm of presure?
n= PV/ RT
Mass = mol * molecular mass of Cl2
101g Cl2
400
That partical pressure of F2 in a mixture of gases where the total presure is 1.00 atm is 300. torr. What is the mole fraction of F2?
Pi = Xi * PT
Pi = initial pressure
Xi= mole fraction
PT = total pressure
Xi = Pi/ PT
1.00 atm = 760 torr/ 300 torr= 2.3 mole fraction
400
What variables are constant when temperature and pressure are directly related?
Mass and Volume
400
If the temperture is constant, as the pressure of a gas increase the volume will?
Decrease
400
A 10 L sample of gas at 300 degrees Celsius is to be cooled at constant pressure until it reaches half its original volume. What is the Kelvin temperature at which the sample will reach half its original volume.
286.5 K
500
List the units for P, V, n, R and T?
P = atm, kPa,mmHg or torr
V = L and ml
n = mol
R = L * atm/ mol * K
L * kPa/ mol * K
T = Kelvin
500
A 32.0 mL sample of hydrogen is collected oer water at 20 C and 750.0 torr pressure. what is the volume of the dry gas at STP? ( Vapor presure of water at 20 C = 17.5 torr)
750.0 torr - 17.5 torr = 732.5 torr
PV = nRT
n = PV/ RT
1 mol= 22.4 L
0.963 atm * 0.032 L/ .0821atm*L/ mol *K * 293 K = 0.00128 mol
0.00128 mol * 22.4 L = 0.0287 L or 28.7 ml
500
The gas in an aerosol can is at a pressur of 3 atm at 25 C. Directions on the can warns the user not to keep the can in a place where the temperature exceeds 52 c. what would the gass pressure in the can be at 52 c?
3.27 atm
500
Chlorine gas occupies a volume of 1.2 liters at 720 torr pressure. What volume will occupy at 1 atm pressure?
A helium-filled balloon has a volume of 2.75 L at 20 degrees Celsius. The volume of the balloon decreases to 2460 ml after it is placed outside on a cold day. What is the outside temperature in Kelvin.