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 (LiClO4) to make oxygen and lithium chloride (LiCl):

LiClO4 (s)  2O2 (g) + LiCl (s)
If you have 500 g of LiClO4, 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.)

LiClO4 --> LiCl + 2O2

mols LiClO4 = grams/molar mass
Using the coefficients in the balanced equation, convert mols LiClO4 to mols O2.
Now use PV = nRT and convert mols O2 to L at the conditions listed. Remember T must be in kelvin. If you use kPa for P you must use 8.314 for R.

To solve this problem, we can use the Ideal Gas Law to calculate the number of moles of oxygen produced and then convert that to liters.

Step 1: Convert the mass of LiClO4 to moles.
To do this, we need the molar mass of LiClO4, which can be obtained from the periodic table.
Li = 6.94 g/mol
Cl = 35.45 g/mol
O = 16.00 g/mol

Molar mass of LiClO4 = 6.94 + (35.45 * 4) + (16.00 * 4) = 187.45 g/mol

Number of moles = mass / molar mass = 500 g / 187.45 g/mol = 2.665 moles of LiClO4

Step 2: Determine the stoichiometry of the reaction.
From the balanced equation, we can see that 1 mole of LiClO4 produces 2 moles of O2.

Step 3: Calculate the number of moles of O2 produced.
Number of moles of O2 = 2.665 moles of LiClO4 * (2 moles of O2 / 1 mole of LiClO4) = 5.33 moles of O2

Step 4: Convert moles of O2 to liters using the Ideal Gas Law.
The Ideal Gas Law is PV = nRT, where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature (in Kelvin)

First, convert the temperature from degrees Celsius to Kelvin:
T(K) = T(°C) + 273 = 21 + 273 = 294 K

Now we can calculate the volume of oxygen:
V = (n * R * T) / P
= (5.33 moles * 0.0821 L.atm/mol.K * 294 K) / 101.5 kPa
= 1.235 liters

Therefore, the chemical oxygen generator system will produce approximately 1.235 liters of oxygen at the given operating conditions.

To solve this problem, we need to use the ideal gas law equation:

PV = nRT

Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal gas constant
T = Temperature

Step 1: Calculate the number of moles of oxygen produced
To do this, we need to convert the mass of LiClO4 to moles.

1 mole of LiClO4 = molar mass of LiClO4(g)

The molar mass of LiClO4 is calculated as follows:
Li: 6.941 g/mol
Cl: 35.453 g/mol
O: 16.00 g/mol (12.01 * 3)
The total molar mass of LiClO4: 6.941 + 35.453 + (16.00 * 4) = 124.41 g/mol.

Now we can find the number of moles of LiClO4:
Number of moles = mass / molar mass
Number of moles = 500 g / 124.41 g/mol = 4.02 mol

From the equation, we know that 1 mole of LiClO4 produces 2 moles of O2. Therefore, the number of moles of oxygen produced will be twice the number of moles of LiClO4:
Number of moles of O2 produced = 2 * 4.02 mol = 8.04 mol

Step 2: Convert moles of oxygen to liters using the ideal gas law equation
We need to solve for the volume, so we rearrange the equation as follows:

V = (nRT) / P

Where:
V = volume in liters
n = number of moles
R = ideal gas constant (0.0821 L.atm/K.mol)
T = temperature in Kelvin (21°C + 273.15)
P = pressure in atm (101.5 kPa / 101.325 atm/kPa)

Substituting the values into the equation:
V = (8.04 mol * 0.0821 L.atm/K.mol * (21°C + 273.15)) / (101.5 kPa / 101.325 atm/kPa)

Performing the calculations:
V = 187.27 L

Therefore, the system will produce approximately 187.27 liters of oxygen at the given conditions.