Term
| 1atm is equal to how many mmHg and how much torr? |
|
Definition
| 1atm = 760mmHg = 760 torr |
|
|
Term
| If a bicycle tire has a pressure of 72psi how many atmospheres would this be? (1atm = 14.7psi) |
|
Definition
| 72psi x (1atm/14.7psi) = 4.9atm |
|
|
Term
| The atmospheric pressure in San Fransisco on a certain day was 732mmHg. What was the pressure in kPa? (1atm = 1.01325 x 105Pa) (1000Pa = 1kPa) |
|
Definition
732mmHg x (1atm/760mmHg) x (1.01325 x 105Pa/1atm) = 9.76 x 104Pa
9.76 x 104Pa x (1kPa/1000Pa) = 97.6kPa |
|
|
Term
|
Definition
P α (1/v)
PV = constant
P1V1 = P2V2
P↑V↓ |
|
|
Term
| A sample of chlorine gas occupies a volume of 946mL at a pressure of 726mmHg. What is the pressure of the gas (in mmHg) if the volume is reduced at constant temperature to 154mL? |
|
Definition
P1V1 = P2V2
P1 = 726mmHg
V1 = 946mL
P2 = ?
V2 = 154mL
P2 = (P1V1/V2)
P2 = (726mmHg)(946mL)/(154mL)
P2 = 4460mmHg |
|
|
Term
|
Definition
V α T
V = constant x T
V1/T1 = V2/T2
T↓V↓ |
|
|
Term
| A sample of carbon monoxide gas occupie 3.20L at 125oC. At what temperature will the gas occupy a volume of 1.54L if the pressure remains constant? |
|
Definition
V1/T1 = V2/T2
V1 = 3.20L
T1 = 125oC + 273 = 398K
V2 = 1.54L
T2 = ?
T2 = (V2)(T1)/(V1)
T2 = (1.54L)(398K)/(3.20L)
T2 = 192K |
|
|
Term
|
Definition
P α T
P = constant x T
P1/T1 = P2/T2 |
|
|
Term
| An aerosol can has pressure of 1.4atm at 25oC. What pressure would it attain at 1200oC, assuming the volume remained constant? |
|
Definition
P1/T1 = P2/T2
P2 = (P1V2)/(T1)
P2 = (1.4atm)(1473L)/(298K)
P2 = 6.9atm |
|
|
Term
|
Definition
|
|
Term
| A sample of carbon dioxide occupies 4.5L at 30oC and 650mmHg. What volume would it occupy at 800mmHg and 200oC? |
|
Definition
P1V1/T1 = P2V2/T2
P1 = 650mmHg
V1 = 4.5L
T1 = 30oC +273 = 303K
P2 = 800mmHg
V2 = ?
T2 = 200oC + 273 = 473K
V2 = (P1V1T2)/(P2T1)
V2 = (650mmHg)(4.5L)(473K)/(800mmHg)(303K)
V2 = 5.7L |
|
|
Term
|
Definition
V α number of moles (n)
V = constant x n
V1/n1 = V2/n2 |
|
|
Term
At constant temperature and pressure, 16L of N2 and 48L of H2 are mixed. Assuming all the reactants are consumed, how many liters of NH3 will be produced?
N2(g) + 3H2(g) --> 2NH3(g) |
|
Definition
1 mol N2 + 3 mol H2 --> 2mol NH3
16L N2 + 48L --> 32L NH3
or
16L N2 x (2L NH3/1L N2) = 32L NH3 |
|
|
Term
|
Definition
V α (nT/P)
V = constant x (nT/P)
V = R (nT/P)
R = gas constant
PV = nRT |
|
|
Term
|
Definition
|
|
Term
| What is the volume (in liters) occupied by 49.8g of HCl at STP? (HCl = 36.45g/mol) |
|
Definition
PV = nRT
P = 1atm
V = ?
n = 49.8g HCl x (1mol HCl/36.45g) = 1.37mol
R = 0.0821 (L atm/mol K)
T = 273K
V = nRT/P
V = (1.37mol)(0.0821L atm/mol K)(273K)/(1atm)
V = 30.6L |
|
|
Term
What is the temperature, in Kelvins, at which 15.0g O2 will exert a pressure of 785torr in a volume of 5.00L?
(O2 = 32.0g/mol) |
|
Definition
PV = nRT
P = 785torr x (1atm/760torr)
V = 5.00L
n = 15g O2 x (1mol/32g) = 0.469mol
R = 0.0821 (L atm/mol K)
T = ?
T = PV/nR
T = (785/760atm)(5.00L)/(0.469mol)(0.0821L atm/mol K)
T = 134K |
|
|
Term
| A sample of flourine gas has a volume of 5.80L at 150.0oC and 10.5atm of pressure. How many moles of flourine gas are present? |
|
Definition
PV = nRT
P = 10.5atm
V = 5.80L
n = ?
R = 0.0821 (L atm/mol K)
T = 423K
n = PV/RT
n = (10.5atm)(5.80L)/(0.0821L atm/mol K)(423K)
n = 1.75mol |
|
|
Term
| What is the density in g/L of UF6 at 779mmHg and 62oC? (UF6 = 352g/mol) |
|
Definition
d = PM/RT
d = (779/760atm)(352g/mol)/(0.0821L atm/mol K)(335K)
d = 13.1g/L |
|
|
Term
| A 2.10L vessel contains 4.65g of a gas at 1.00atm and 27.0oC. What is the molar mass of the gas? |
|
Definition
M = dRT/P
d = m/v
d = 4.65g/2.101L = 2.21g/L
M = (2.21g/L)(0.0821L atm/mol K)(300K)/(1atm)
M = 54.5g/mol |
|
|
Term
What is the volume of CO2 produced at 37oC and 1.00atm when 5.60g of glucose are used up in the reaction:
C6H12O6(s) + 6O2(g) --> 6CO2(g) + 6H2O(l)
(C6H12O6 = 180g/mol) |
|
Definition
gC6H12O6 --> mol C6H12O6 --> mol CO2 --> V CO2
5.6g C6H12O6 x (1mol C6H12O6/180g) x (6mol CO2/1mol C6H12O6) = 0.187mol CO2
PV = nRT
V = nRT/P
V = (0.187mol)(0.821L atm/mol K)(310K)/(1atm)
V = 4.76L |
|
|
Term
Airbags fill with N2 gas in an accident. The gas is generated by the decomposition of sodium azide. How many grams of sodium azide, NaN3, would be required to provide 75.0L of N2 gas at 35.0oC and 748mmHg
6NaN3(s) + Fe2O3(s) --> 3Na2O(s) + 2Fe(s) + 9N2(g)
(NaN3 = 65.01g/mol)
|
|
Definition
mol N2 --> mol NaN3 --> g NaN3
PV = nRT
n = PV/RT
n = (748/760atm)(75L)/(0.821L atm/mol K)(298K)
n = 3.02mol N2
3.02mol N2 x (6mol NaN3/9mol N2) x (65.01g NaN3/1mol) = 131g NaN3 |
|
|
Term
| What is partial pressure? |
|
Definition
| the pressure exerted by a particular gas in a mixture of gases |
|
|
Term
|
Definition
| the total pressure of a mixture of gasses in the sum of the pressures that each gas would exert if it were present alone |
|
|
Term
| A sample of natural gas contains 8.24 moles of CH4, 0.421 moles of C2H6, and 0.116 moles of C3H8. If the total pressure of the gases is 1.37atm, what is the partial pressure of propane (C3H8)? |
|
Definition
PC3H8 = XC3H8 PT
XC3H8 = (0.116mol)/(8.24mol) + (0.421mol) + (0.116mol) = 0.0132
PC3H8 = (0.0132)(1.37atm)
PC3H8 = 0.0181atm |
|
|
