which gas will have the most collisions between its particles, methane at 340K, carbon dioxide at 80 C, argon at 265K or helium
2 answers:
Answer: Option (b) is the correct answer.
Explanation:
As it is known that more is the kinetic energy present between the molecules of a gas, more will be the number of collisions take place.
Also, relation between kinetic energy and temperature is as follows.
K.E =
This means that more is the temperature of gas more will be the kinetic energy present withing its molecules or vice-versa.
As methane is at 340 K.
Carbon dioxide is at 80 = (80 +273) K = 353 K
Argon is at 265 K and helium is at 20 = (20 + 273)K = 293 K
Therefore, temperature of carbon dioxide gas is the maximum.
Thus, we can conclude that the carbon dioxide gas at 80 will have the most collisions between its particles.
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Answer:
Explanation:
Hello.
In this case, for this equilibrium problem, we first realize that at the beginning there is just HI, it means that the reaction should be rewritten as follows:
Whereas the law of mass action (equilibrium expression) is:
That in terms of initial concentrations and reaction extent or change turns out:
And the solution via solver or quadratic equation is:
Whereas the correct answer is 0.183 M since the other value yield a negative concentration of HI at equilibrium (0.391-2*0.210=-0.029M).This, the equilibrium concentrations are:
Regards.