The gaseous product of a reaction is collected in a 64-L container at 27oC. The pressure in the container is 1.45 atm. How many moles of the gas are in the container?
since 1 mole occupies 22.4L at STP, and PV/nT is constant, you want n such that
1.45*64/((27+273)n) = 1*22.4/(273n)
I would use PV = nRT and
n = PV/RT = 1.45*64/0.08205*(273+27)
Looks simpler to me.
To determine the number of moles of gas in the container, we can use the Ideal Gas Law equation:
PV = nRT
where:
P is the pressure in atm (1.45 atm),
V is the volume in liters (64 L),
n is the number of moles,
R is the gas constant (0.0821 L·atm/K·mol), and
T is the temperature in Kelvin (27°C + 273.15 = 300.15 K).
Rearranging the equation:
n = PV / RT
Substituting the given values:
n = (1.45 atm) * (64 L) / (0.0821 L·atm/K·mol) * (300.15 K)
Calculating:
n ≈ 3.02 moles
Therefore, there are approximately 3.02 moles of gas in the container.
To find the number of moles of a gas in a container, we can use the ideal gas law equation:
PV = nRT
Where:
P is the pressure of the gas (in atmospheres)
V is the volume of the gas (in liters)
n is the number of moles of gas
R is the ideal gas constant (0.0821 L·atm/mol·K)
T is the temperature of the gas (in Kelvin)
First, let's convert the given temperature from Celsius to Kelvin. The equation to convert Celsius to Kelvin is:
T(K) = T(°C) + 273.15
So, 27oC + 273.15 = 300.15 K
Now, we can plug the given values into the ideal gas law equation:
1.45 atm × 64 L = n × 0.0821 L·atm/mol·K × 300.15 K
Simplifying, we have:
92.8 = 0.0821 × 300.15 × n
To solve for n, divide both sides of the equation by (0.0821 × 300.15):
n = 92.8 / (0.0821 × 300.15)
n ≈ 3.76 moles
Therefore, there are approximately 3.76 moles of gas in the container.