what is the temperature (degree celcius) of 1.75g of o2 gas occupying 4.6l at 1.00 atm?
PV=nrT
n=1.75/32
solve for temp. Use the correct gas constant for your units.
To find the temperature of the oxygen 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, let's convert the given values to the appropriate units:
Mass of O2 gas (m) = 1.75 g
Since we know the molar mass of oxygen (O2) is approximately 32 g/mol, we can find the number of moles (n) using the formula:
n = m/M
where M is the molar mass of O2.
n = 1.75 g / 32 g/mol = 0.0547 mol (approximately)
Now we have all the required values for the Ideal Gas Law equation:
P = 1.00 atm
V = 4.6 L
n = 0.0547 mol
R = 0.0821 L·atm/(mol·K)
Rearranging the equation to solve for temperature (T):
T = PV / nR
Plugging in the values:
T = (1.00 atm * 4.6 L) / (0.0547 mol * 0.0821 L·atm/(mol·K))
Now, we can calculate the value of T to find the temperature in Kelvin.