A balloon that contains 0.750 moles of gas has a volume of 16.8 l. if the balloon expands to a volume of 25.4 l at a constant pr
2 answers:
Answer: 1.13 mol
Explanation:
Avogadro's Law: This law states that volume is directly proportional to the number of moles of the gas at constant pressure and temperature.
(At constant temperature and pressure)
where,
= initial volume of gas = 16.8 L
= final volume of gas = 25.4 L
= initial number of moles = 0.750
= final number of moles = ?
Now put all the given values in the above equation, we get the final pressure of gas.
Therefore, the final moles will be 1.13.
You might be interested in
The question is incomplete, here is the complete question:
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy Ea = 71.0 kJ/mol . If the rate constant of this reaction is 6.7 M^(-1)*s^(-1) at 244.0 degrees Celsius, what will the rate constant be at 324.0 degrees Celsius?
<u>Answer:</u> The rate constant at 324°C is
<u>Explanation:</u>
To calculate rate constant at two different temperatures of the reaction, we use Arrhenius equation, which is:
where,
= equilibrium constant at 244°C =
= equilibrium constant at 324°C = ?
= Activation energy = 71.0 kJ/mol = 71000 J/mol (Conversion factor: 1 kJ = 1000 J)
R = Gas constant = 8.314 J/mol K
= initial temperature =
= final temperature =
Putting values in above equation, we get:
Hence, the rate constant at 324°C is