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andriy [413]
3 years ago
12

In a sealed gas-liquid system at constant temperature, eventually...?

Chemistry
1 answer:
SOVA2 [1]3 years ago
4 0
<h2>Let us study about it .</h2>

Explanation:

Evaporation

It is the process of converting liquid into vapors .

Condensation

It is the process of converting  vapors back into liquid state .

  1. Suppose if we have a sealed container and we are supplying it with no or little heat , we will see that as we increase heat , the particles starts moving faster .
  2. When they move they also colloide and transfer energies .
  3. The kinetic energies of certain molecule increase to an extent that they leave the other particles and escape in atmosphere .
  4. That is evaporation occurs .At the same time when these vapors collide with each other or with the walls of container they get cooled and again get converted to liquid state .

It is seen that  a equilibrium is reached when "rate of evaporation becomes equal to rate of condensation ".

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A piece of fossilized wood has a carbon-14 radioactivity that is 1/4 that of new wood. the half-life of carbon-14 is 5730 years.
Marizza181 [45]

Answer:

1.146 x 10⁴ year.

Explanation:

  • The decay of carbon-14 is a first order reaction.
  • The rate constant of the reaction (k) in a first order reaction = ln (2)/half-life = 0.693/(5730 year) = 1.21 x 10⁻⁴ year⁻¹.
  • The integration law of a first order reaction is:

<em>kt = ln [A₀]/[A]</em>

<em></em>

k is the rate constant = 1.21 x 10⁻⁴ year⁻¹.

t is the time = ??? years.

[A₀] is the initial percentage of carbon-14 = 100.0 %.

[A] is the remaining percentage of carbon-14 = 1/4[A₀] = 25.0 %.

∵ kt = ln [Ao]/[A]

∴ (1.21 x 10⁻⁴ year⁻¹)(t) = ln (100.0%)/[25.0 %]

(1.21 x 10⁻⁴ year⁻¹)(t) = 1.386.

∴ <em>t </em>= 1.386/ (1.21 x 10⁻⁴ year⁻¹) =  <em>1.146 x 10⁴ year.</em>

3 0
3 years ago
What could you do if you wanted to slow down the rate of a particular reaction?
hjlf

Answer:

catalyst

Explanation:

this help toalter or speed up the rate of reaction could be the most to slow it

5 0
2 years ago
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