if an ideal gas has a pressure 2.47 atm, a temperature 86.78C and has a volume of 23.83L how many moles are in the sample
Use PV = nRT
To find the number of moles in the sample, we can use the ideal gas law equation:
PV = nRT
where:
P = pressure of the gas (in atm)
V = volume of the gas (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature of the gas (in Kelvin)
First, let's convert the given temperature from Celsius to Kelvin:
T(K) = T(C) + 273.15
T(K) = 86.78 + 273.15
T(K) = 359.93 K
Now, we can substitute the given values into the ideal gas law equation:
2.47 atm * 23.83 L = n * (0.0821 L·atm/(mol·K)) * 359.93 K
Simplifying the equation:
58.9301 = n * 29.5789133
Dividing both sides by 29.5789133:
n = 58.9301 / 29.5789133
n ≈ 1.99 moles
Therefore, there are approximately 1.99 moles in the sample.
To find the number of moles in a gas sample, 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)
In order to use this equation, we need to convert the given temperature from Celsius to Kelvin. The conversion between Celsius and Kelvin is T(K) = T(°C) + 273.15.
Given:
Pressure (P) = 2.47 atm
Temperature in Celsius (T) = 86.78°C
Volume (V) = 23.83 L
First, we convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 86.78 + 273.15
T(K) = 359.93 K
Now we can rearrange the ideal gas law equation to solve for n (number of moles):
n = PV / RT
Substituting the given values:
n = (2.47 atm * 23.83 L) / (0.0821 L·atm/mol·K * 359.93 K)
Now we can calculate the number of moles n:
n ≈ 1.042 mol
Therefore, there are approximately 1.042 moles in the given gas sample.