Solution :
According to the Graham's law of diffusion, we know that, the rate of the diffusion varies inversely to the molar mass of the gas, i.e.
Rate of diffusion, 
where, the 'M' is the molar mass of the gas.
Now in the case of the isotopes of the Krypton,
Atomic mass of 
= 80 AMU
Atomic mass of 
= 82 AMU
Atomic mass of 
= 83 AMU
So the ratio of the rate of diffusion of the three isotopes are :
Dividing the above three with the smallest number among the three i.e. 0.10976, we get the relative rates of diffusion.
∴
= 1.02 : 1.01 : 1
Hence the relative rate of diffusion are :
Answer:
As the description in the question shows, Kaley is taking careful and regular measurements. Hence, her experimental method is correct.
Kaley has also developed a hypothesis and the experiment she conducted is also valid hence there is no problem in these steps.
There is no mistake being done by her in depicting the results of the experiment.
Hence, the only thing which we can say is missing from the experiment is the past researches which scientists might have made on this topic.
Explanation:
Assuming that nitrogen gas is ideal, we can use the equation PV = nRT to relate first conditions to the second condition. At constant temperature, pressure and volume are indirectly related as follows:
P = k / V
k is equal nRT
P1V1 = P2V2
P2 = 101.325 ( 4.65 ) / .480 = 981.586 kPa
The answer should be...99.318!
