Question

PLEASE HELP ASAP 100 POINTS

Score
The Russian Mir space station used a chemical oxygen generator system to make oxygen for the crew. The
system ignited a tube of solid lithium perchlorate (LICIO4) to make oxygen and lithium chloride (LICI):
LICIO4 (s) → 202 (g) + LiCl (s)
If you have 500 g of LICIO4, then how many liters of oxygen will the system make at the station's standard
operating conditions, a pressure of 101.5 kPa and a temperature of 21°C? (Show the steps involved in your work)

Answer 1

To solve this problem, we need to use the ideal gas law, which relates the pressure, volume, and temperature of a gas to the number of moles of gas present. We can use the balanced chemical equation to determine the number of moles of oxygen produced by the reaction of LICIO4.

The molar mass of LICIO4 is:

LICIO4: Li = 1 x 1 = 1 g/mol, I = 127 g/mol, O4 = 4 x 16 = 64 g/mol

Total molar mass = 1 + 127 + 64 = 192 g/mol

So, 500 g of LICIO4 is equal to:

500 g / 192 g/mol = 2.604 moles of LICIO4

From the balanced chemical equation, we see that for every mole of LICIO4, two moles of oxygen are produced:

1 mol LICIO4 → 2 mol O2

Therefore, 2.604 moles of LICIO4 will produce:

2.604 moles x 2 mol O2/1 mol LICIO4 = 5.208 moles of O2

Now we can use the ideal gas law to calculate the volume of oxygen produced at the given temperature and pressure:

PV = nRT

where P is the pressure (101.5 kPa), V is the volume we want to find, n is the number of moles of oxygen (5.208 moles), R is the ideal gas constant (8.314 J/mol K), and T is the temperature in Kelvin (21°C + 273 = 294 K).

V = (nRT)/P

V = (5.208 mol x 8.314 J/mol K x 294 K)/101.5 kPa

Converting kPa to Pa, we get:

V = (5.208 mol x 8.314 J/mol K x 294 K)/(101.5 x 1000 Pa)

V = 101.92 m3 or 101,920 L

Therefore, the system would produce approximately 101,920 liters of oxygen at the station's standard operating conditions.