what is the volume in liters of 4.2 moles methane gas, at 26degree C and 1.40 atm?
assuming that the gas is ideal, we use the formula for ideal gases:
PV = nRT
where
P = pressure (in atm)
V = volume (in L)
n = number of moles
R = gas constant (0.0821 L*atm/mol-K)
T = temperature (in Kelvin)
we first convert the 26 degrees Celsius to Kelvin:
26 + 273.15 = 299.15 K
substituting,
(1.40)(V) = (4.2)(0.0821)(299.15)
V = (4.2)(0.0821)(299.15)/(1.40)
V = 73.68 L
hope this helps~ :)
An ideal Gas is allowed to expand from 7.40 L to 62.9 L at a constant temperature.
by what factor does the volume increase?
The pressure will (increase/decrease) by that same factor?
If the initial pressure was 137 atm, what is the final pressure?
To find the volume of 4.2 moles of methane gas at 26 degrees Celsius and 1.40 atm, you 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, convert the temperature from Celsius to Kelvin by adding 273.15:
26 °C + 273.15 = 299.15 K
Now, substitute the given values into the equation, and solve for V:
(1.40 atm) * V = (4.2 mol) * (0.0821 L·atm/(mol·K)) * (299.15 K)
Simplifying the equation:
1.40V = 103.0697
Finally, solve for V (volume):
V = 103.0697 / 1.40
V ≈ 73.62 liters
Therefore, the volume of 4.2 moles of methane gas at 26 °C and 1.40 atm is approximately 73.62 liters.