How many moles of a gas at 100 degrees celciuos does it take to fill a 1.00 flask to a pressure of 1.50 atm?
PV = nRT
How many moles of a gas at 100 degrees celciuos does it take to fill a 1.00L flask to a pressure of 1.50 atm?
To find the number of moles of gas, we can use the ideal gas law equation:
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, we need to convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 100°C + 273.15 = 373.15 K
Next, we rearrange the equation to solve for n:
n = (PV) / (RT)
Plugging in the given values:
P = 1.50 atm
V = 1.00 L
R = 0.0821 L.atm/mol.K
T = 373.15 K
n = (1.50 atm * 1.00 L) / (0.0821 L.atm/mol.K * 373.15 K)
Calculating the expression:
n = 0.0607 moles
Therefore, it would take approximately 0.0607 moles of gas to fill the 1.00 L flask to a pressure of 1.50 atm at 100°C.
To answer this question, we need to use the Ideal Gas Law, which states:
PV = nRT
Where:
P = Pressure (in atmospheres)
V = Volume (in liters)
n = Number of moles of gas
R = Ideal gas constant (0.0821 L·atm/mol·K)
T = Temperature (in Kelvin)
To determine the number of moles of gas, we can rearrange the formula:
n = PV / RT
Given:
P = 1.50 atm
V = 1.00 L
R = 0.0821 L·atm/mol·K
T = 100 degrees Celsius
First, we need to convert the temperature from Celsius to Kelvin by adding 273.15:
T = 100 + 273.15 = 373.15 K
Now, we can substitute the values into the equation:
n = (1.50 atm * 1.00 L) / (0.0821 L·atm/mol·K * 373.15 K)
n ≈ 0.046 moles
Therefore, it would take approximately 0.046 moles of gas at 100 degrees Celsius to fill a 1.00 L flask to a pressure of 1.50 atm.