what is the volume in liters of 3.0 moles CH4, at 26C and 1.48atm?
PV=nRT
change temp to K
watch units with R
thanks...the whole R thing is throwing me off...
To find the volume in liters of 3.0 moles of CH4 at 26°C and 1.48 atm, we can use the Ideal Gas Law equation: PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature.
First, let's make sure our units are consistent. The pressure is given in atm, and we want the volume in liters. The gas constant R is 0.0821 L·atm/(mol·K), which is commonly used for atm pressure and liter volume.
Next, we need to convert the temperature from Celsius to Kelvin since the Ideal Gas Law requires temperature in Kelvin. To convert Celsius to Kelvin, we simply add 273.15 to the Celsius temperature. So, 26°C + 273.15 = 299.15 K.
Now, we can plug all the values into the Ideal Gas Law equation:
PV = nRT
V = (nRT) / P
V = (3.0 mol) * (0.0821 L·atm/(mol·K)) * (299.15 K) / (1.48 atm)
Calculating this expression will give you the volume in liters.
Please note that this calculation assumes ideal gas behavior and that the CH4 is a perfect gas at the given conditions.