a 0.296g of CO2 has a volume of 565ml and a pressure of 425mmHG, what is the temperature??????
PV=nRT
find n, given mass. Then find temp. Watch units of R and your other units to make certain they are in the same units.
Use PV = nRT
thanks.. tried this formula several times, must be putting numbers in the wrong place..if R equals 0.0821L x atm per mole x K..and I don't know what the temp is?
To determine the temperature in this scenario, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles of gas
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature (in Kelvin)
First, we need to convert the given values to the appropriate units.
1 atm = 760 mmHg
1 mL = 0.001 L
Pressure: 425 mmHg * (1 atm / 760 mmHg) = 0.559 atm
Volume: 565 mL * (0.001 L / 1 mL) = 0.565 L
Next, we need to calculate the number of moles of CO2. To do this, we can use the molar mass of CO2, which is 44.01 g/mol.
Mass = 0.296 g
Molar mass of CO2 = 44.01 g/mol
Number of moles (n) = Mass / Molar mass = 0.296 g / 44.01 g/mol
Now, we have all the required values to solve for temperature.
PV = nRT
Substituting the values:
(0.559 atm) * (0.565 L) = (moles) * (0.0821 L·atm/mol·K) * T
Solving for T:
T = (0.559 atm * 0.565 L) / (moles * 0.0821 L·atm/mol·K)
Now, substitute the value of moles into the equation and calculate the temperature.