a 16.2 L sample of CO(g) at 1.50 atm and 200.*C is combined with 15.39g of Fe2O3(s), How many moles of CO(g) are availabe for the reaction
Use PV = nRT. Calculate n = moles. Don't forget to convert T to Kelvin.
To determine the number of moles of CO(g) available for the reaction, we need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure (atm)
V = volume (L)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (Kelvin)
First, let's convert the given temperature from Celsius to Kelvin:
T(K) = 200°C + 273.15 = 473.15 K
Next, we can rearrange the ideal gas law equation to solve for n:
n = PV / RT
Now, let's plug in the known values:
P = 1.50 atm
V = 16.2 L
R = 0.0821 L·atm/(mol·K)
T = 473.15 K
n = (1.50 atm * 16.2 L) / (0.0821 L·atm/(mol·K) * 473.15 K)
n ≈ 1.47 moles of CO(g)
Therefore, there are approximately 1.47 moles of CO(g) available for the reaction.
To find the number of moles of CO(g) available for the reaction, you need to determine the number of moles of CO(g) in the given sample.
First, let's start by calculating the number of moles of Fe2O3(s):
1. Determine the molar mass of Fe2O3:
- Fe: 55.845 g/mol
- O: 16.00 g/mol
Molar mass of Fe2O3 = (2 * 55.845 g/mol) + (3 * 16.00 g/mol) = 159.69 g/mol
2. Convert the mass of Fe2O3(s) to moles:
Number of moles = mass of Fe2O3(s) / molar mass of Fe2O3
Number of moles = 15.39 g / 159.69 g/mol
Calculate the number of moles of CO(g) using the ideal gas law:
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)
1. Convert the temperature from Celsius to Kelvin:
T(Kelvin) = T(Celsius) + 273.15
T(Kelvin) = (200 *C + 273.15)
2. Rearrange the ideal gas law to solve for the number of moles:
n = PV / RT
- Pressure (P): 1.50 atm
- Volume (V): 16.2 L
- Temperature (T): Convert from Celsius to Kelvin (step 1)
Now, plug in the values and calculate the number of moles of CO(g):
n = (1.50 atm * 16.2 L) / (0.0821 L.atm/mol.K * (200 *C + 273.15))
Evaluate this expression to find the moles of CO(g) available for the reaction.