A sample of nitrogen gas occupies 2.49 L at 19.5°C. The volume of the container changes at constant pressure to 4.29 L. What tem
1 answer:
Answer : The final temperature of the gas must be
Solution : Given,
Initial volume of gas = 2.49 L
Final volume of gas = 4.29 L
Initial temperature of gas =
According to the Charles' law, the volume of gas is directly proportional to the temperature of the gas at constant pressure.
Now put all the given values in this formula, we get the final temperature of the gas.
By rearranging the term, we get
Therefore, the final temperature of the gas must be
You might be interested in
Explanation:
The given data is as follows.
Mass flow rate of mixture = 1368 kg/hr
in feed = 40 mole%
This means that in feed = (100 - 40)% = 60%
We assume that there are 100 total moles/hr of gas in feed stream.
Hence, calculate the total mass flow rate as follows.
40 moles/hr of N_{2}/hr (28 g/mol of ) + 60 moles/hr of
(2 g/mol of
)
= 1120 g/hr + 120 g/hr
= 1240 g/hr
= (as 1 kg = 1000 g)
= 1.240 kg/hr
Now, we will calculate mol/hr in the actual feed stream as follows.
= 110322.58 moles/hr
It is given that amount of nitrogen present in the feed stream is 40%. Hence, calculate the flow of into the reactor as follows.
= 44129.03 mol/hr
As 1 mole of nitrogen has 28 g/mol of mass or 0.028 kg.
Therefore, calculate the rate flow of into the reactor as follows.
= 1235.612 kg/hr
Thus, we can conclude that the the feed rate of pure nitrogen to the mixer is 1235.612 kg/hr.
Answer: d) 164.9 g
Explanation:
To calculate the moles :
The balanced chemical reaction is:
According to stoichiometry :
2 moles of require = 25 moles of
Thus 0.412 moles of will require=
of
Mass of
Thus 164.9 g of oxygen is consumed.