You are confronted with the following question: One mole of an ideal gas is sealed in a 22.4- container at a pressure of 1 and a temperature of 273 . The temperature is then increased to 305 , but the container does not expand. What will the new pressure be?
Part A
The most appropriate formula for solving this problem includes which variables?
Pv=nRT
for both the initial and final state.
Only thing your changing are temperature and since moles, R and volume are constant pressure must change.
Thus P1/T1=P2/T2
P2=P1*T2/T1
1.12 atm
To solve this problem, we can use the ideal gas law formula, which is:
PV = nRT
Where:
P represents pressure,
V represents volume,
n represents the number of moles,
R is the ideal gas constant, and
T represents temperature.
In this case, we have the following known values:
Initial condition:
Number of moles (n) = 1 mole
Volume (V) = 22.4 liters
Pressure (P) = 1 atm
Temperature (T) = 273 K
Final condition:
Temperature (T) = 305 K
We need to find the final pressure (P).
To solve for P, we can rearrange the ideal gas law equation to solve for P:
P = (nRT) / V
Now, we can substitute the known values into the equation:
P = (1 mole * 0.0821 L.atm/mol.K * 305 K) / 22.4 L
Finally, we can calculate the value of P.