For real gases, how does a change in pressure affect the ratio of PV to nRT?
2 answers:
Answer: Option (b) is the correct answer.
Explanation:
Molecules of a real gas are smaller is size and occupy volume or space. Real gases do not behave like ideal gases.
Mathematically, ratio of is either greater than or smaller than 1.
Hence, when there is increase in pressure then there will be increase in ratio. On the other hand, if there is decrease in ratio then there will be decrease in ratio.
Thus, we can conclude that for real gases, a change in pressure affect the ratio of PV to nRT because the ratio increases as pressure increases.
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The question is incomplete, here is the complete question:
At elevated temperature, nitrogen dioxide decomposes to nitrogen oxide and oxygen gas
The reaction is second order for with a rate constant of
at 300°C. If the initial [NO₂] is 0.260 M, it will take ________ s for the concentration to drop to 0.150 M
a) 1.01 b) 5.19 c) 0.299 d) 0.0880 e) 3.34
<u>Answer:</u> The time taken is 5.19 seconds
<u>Explanation:</u>
The integrated rate law equation for second order reaction follows:
where,
k = rate constant =
t = time taken = ?
[A] = concentration of substance after time 't' = 0.150 M
= Initial concentration = 0.260 M
Putting values in above equation, we get:
Hence, the time taken is 5.19 seconds