Answer:

Explanation:
Hello there!
Unfortunately, the question is not given in the question; however, it is possible for us to compute the equilibrium constant as the problem is providing the concentrations at equilibrium. Thus, we first set up the equilibrium expression as products/reactants:
![K=\frac{[NO_2]^2}{[NO]^2[O_2]}](https://tex.z-dn.net/?f=K%3D%5Cfrac%7B%5BNO_2%5D%5E2%7D%7B%5BNO%5D%5E2%5BO_2%5D%7D)
Then, we plug in the concentrations at equilibrium to obtain the equilibrium constant as follows:

In addition, we can infer this is a reaction that predominantly tends to the product (NO2) as K>>>>1.
Best regards!
D) Responds slowly
Good luck. It responds slower them the nervous system
There are two isotopes of uranium abundant in nature
U235 and U238
As given that the sample has average molar mass of 237.482 amu
Let the amount of U235 in 100g sample = x
the amount of U238 in 100 g sample = 100-x
the average molar mass = [235(x) + 238 (100-x)] / 100
237.482 = [235(x) + 238 (100-x)] / 100
237.482 X 100 = [235(x) + 238 (100-x)]
23748.2 = 235 x + 23800 - 238x
51.8 = 3x
x = 17.27 g
So percentage of U-235 = 17.27 %