Question

In: Chemistry

Calculate the volume of each gas sample at STP. Part A 51.1 g He Part B...

Calculate the volume of each gas sample at STP.

Part A

51.1 g He

Part B

47.0 g Xe

Part C

49.6 mg Cl2

Part D

3.82 kg SO2.

Solutions

Expert Solution

A)

Molar mass of He = 4.003 g/mol

mass(He)= 51.1 g

use:

number of mol of He,

n = mass of He/molar mass of He

=(51.1 g)/(4.003 g/mol)

= 12.77 mol

Given:

P = 51.1 atm

n = 12.7654 mol

T = 273.0 K

use:

P * V = n*R*T

51.1 atm * V = 12.7654 mol* 0.08206 atm.L/mol.K * 273 K

V = 5.5964 L

Answer: 5.60 L

B)

Molar mass of Xe = 131.3 g/mol

mass(Xe)= 47.0 g

use:

number of mol of Xe,

n = mass of Xe/molar mass of Xe

=(47 g)/(1.313*10^2 g/mol)

= 0.358 mol

Given:

P = 51.1 atm

n = 0.358 mol

T = 273.0 K

use:

P * V = n*R*T

51.1 atm * V = 0.358 mol* 0.08206 atm.L/mol.K * 273 K

V = 0.1569 L

Answer: 0.157 L

C)

Molar mass of Cl2 = 70.9 g/mol

mass(Cl2)= 49.6 mg

= 0.0496 g

use:

number of mol of Cl2,

n = mass of Cl2/molar mass of Cl2

=(4.96*10^-2 g)/(70.9 g/mol)

= 6.996*10^-4 mol

Given:

P = 51.1 atm

n = 6.996*10^-4 mol

T = 273.0 K

use:

P * V = n*R*T

51.1 atm * V = 6.996*10^-4 mol* 0.08206 atm.L/mol.K * 273 K

V = 3.07*10^-4 L

Answer: 3.07*10^-4 L

D)

Molar mass of SO2,

MM = 1*MM(S) + 2*MM(O)

= 1*32.07 + 2*16.0

= 64.07 g/mol

mass(SO2)= 3.82 Kg

= 3820.0 g

use:

number of mol of SO2,

n = mass of SO2/molar mass of SO2

=(3.82*10^3 g)/(64.07 g/mol)

= 59.62 mol

Given:

P = 51.1 atm

n = 59.6223 mol

T = 273.0 K

use:

P * V = n*R*T

51.1 atm * V = 59.6223 mol* 0.08206 atm.L/mol.K * 273 K

V = 26.1386 L

Answer: 26.1 L


Related Solutions

how do each of the following affect the calculated volume of hydrogen gas at stp? A:...
how do each of the following affect the calculated volume of hydrogen gas at stp? A: The strip of magnesium used in the experiment was partly oxidized and it was not cleaned before the strip was bent and placed in the buret. B: The bent strip of magnesium dropped out of the end of the buret and some bubbles of H2 from the reaction were not trapped in the buret. C: you did not correct the bariometric pressure for the...
Assuming ideal behavior, which of these gas samples has the greatest volume at STP? 1 g...
Assuming ideal behavior, which of these gas samples has the greatest volume at STP? 1 g of Cl2 1 g of Ar 1 g of Ne Arrange the following gases in order of decreasing density at STP: Rank from largest to smallest. F2 HBr O2 He
What is the mass of 12.0 L of He at STP? A) 2.14 g B) 8.57...
What is the mass of 12.0 L of He at STP? A) 2.14 g B) 8.57 g C) 9.31 g D) 17.1 g E) 22.4
Calculate each of the following quantities for an ideal gas. a. Calculate the volume of the...
Calculate each of the following quantities for an ideal gas. a. Calculate the volume of the gas, in liters, if 1.35 mol has a pressure of 0.995 atm at a temperature of -6 ∘C. b. Calculate the absolute temperature of the gas at which 3.23×10−3 moloccupies 350. mL at 760. torr. c. Calculate the pressure, in atmospheres, if 4.66×10−2 moloccupies 412 mL at 135 ∘C d. Calculate the quantity of gas, in moles, if 54.7 L at 55.0 ∘C has...
Part A Calculate the density of oxygen, O2, under each of the following conditions: STP 1.00...
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 volume of oxygen produced (measured at standard temperature and pressure - STP) at the...
Calculate the volume of oxygen produced (measured at standard temperature and pressure - STP) at the anode during the electrolysis of sodium sulfate solution, if the electrolytic cell is operated at a current of 2.50 amperes for 45 minutes. F = 9.65 x 104 C mol-1 (or 96,500 C mol-1). The molar volume of a gas at STP = 22.4 L mol-1 the two possible reactions at the anode are; O2(g) + 2H2O(l) + 4e- 4OH-(aq) E = 0.40V SO42-...
Calculate the density, in grams per liter, of a gas at STP if 3.16 L of...
Calculate the density, in grams per liter, of a gas at STP if 3.16 L of the gas at 28.5 °C and 734.2 mmHg weighs 0.269 g
Calculate the density, in grams per liter, of a gas at STP if 3.16 L of...
Calculate the density, in grams per liter, of a gas at STP if 3.16 L of the gas at 28.5 °C and 734.2 mmHg weighs 0.269 g.
Part A) A sample of a gas at 25°C and 1.0 atm pressure has a volume...
Part A) A sample of a gas at 25°C and 1.0 atm pressure has a volume of 2.5 L. The container is allowed to expand until the pressure is 0.85 atm and the temperature is 15°C. The final volume of the gas is __________ L. Part B) A reaction is carried out that produces hydrogen gas. The gas is collected in an inverted beaker over water at 25 oC. The vapor pressure of water at 25 oC is 23.78 mmHg....
Part A) Find the pressure in mmHg of a 0.124 g sample of helium gas in...
Part A) Find the pressure in mmHg of a 0.124 g sample of helium gas in a 649 mL container at 34 ∘C. Express the pressure to three significant figures and include the appropriate units. Part B) xture with a total pressure of 770 mmHg contains each of the following gases at the indicated partial pressures: 140 mmHg CO2, 112 mmHg Ar, and 128 mmHg O2. The mixture also contains helium gas. What is the partial pressure of the helium...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT