If you mix different amounts of two ideal gases that are originally at different temperatures, what must be true of the final state after the temperature stabilizes? (there may be more than one correct choice.)
a) both gases will reach the same final temperature.
b) the final rms molecular speed will be the same for both gases.
c) the final average kinetic energy of a molecule will be the same for both gases.
i will apply the equation:
2as = v^2 - u^2
v = √ (2a + u^2)
v = √(2 x 4 x 400 + 13 ^2)
v = 58 m/s
the acids react with base and the reaction is known as neutralization
one mole of hydronium ion reacts with one mole of hydroxide ion
a) hi is a monoprotic acid : one mole of hi will give one mole of hydronium ion
b) csoh is a monohydroxide base : one mole of csoh will give one mole of hydroxide ion
so one mole of hi will react with one mole of csoh
the moles of csoh taken will be calculated from molarity and volume as
thus moles of csoh are
moles of hi required is 0.005425 mol
volume of hi required will be
volume of hi required is 9.86 ml
here, we have to get the effect of temperature, the reaction which is exothermic.
as the temperature increase the concentration of n₂o₄ will decrease and the formation of product will be favorable.
the left to right reaction is exothermic.
the reaction is n₂o₄⇄2no₂.
now the reaction from left to right has the heat of reaction 14 kcal. thus this reaction is exothermic.
as per thermodynamics δg = δh - tδs (where, δg = gibbs free energy, δh = heat of the reaction, δs = entropy and t = temperature).
for the favorable reaction δg must be negative. thus the reaction from left to right will be favorable. also as the temperature increase the rate of the reaction from left to right will increase.