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3 years ago

What is the kinetic molecular model?

Chemistry

2 answers:

gulaghasi [49]3 years ago

8 0

Answer:

It's a theory of gases.

Explanation:

It describes a gas as a large number of submicroscopic particles. In which all of them are in constant, rapid, random motion. The randomness arises from the particles' many collisions with each other and with the walls of the container.

saul85 [17]3 years ago

7 0

Answer:

The kinetic theory of gases describes a gas as a large number of submicroscopic particles, all of which are in constant, rapid, random motion. The randomness arises from the particles' many collisions with each other and with the walls of the container

Explanation:

You might be interested in

What factors affect the dynamic state of equilibrium in a chemical reaction and how?

yanalaym [24]

Answer:

Only changes in temperature will influence the equilibrium constant $K_c$ . The system will shift in response to certain external shocks. At the new equilibrium $Q$ will still be equal to $K_c$ , but the final concentrations will be different.

The question is asking for sources of the shocks that will influence the value of $Q$ . For most reversible reactions:

External changes in the relative concentration of the products and reactants.

For some reversible reactions that involve gases:

Changes in pressure due to volume changes.

Catalysts do not influence the value of $Q$ . See explanation.

Explanation:

$\displaystyle K_c = {e}^{\Delta G/(R\cdot T)}$ .

Similar to the rate constant, the equilibrium constant $K_c$ depends only on:

$\Delta G$ the standard Gibbs energy change of the reaction, and
$T$ the absolute temperature (in degrees Kelvins.)

The reversible reaction is in a dynamic equilibrium when the rate of the forward reaction is equal to the rate of the backward reaction. Reactants are constantly converted to products; products are constantly converted back to reactants. However, at equilibrium $Q = K_c$ the two processes balance each other. The concentration of each species will stay the same.

Factors that alter the rate of one reaction more than the other will disrupt the equilibrium. These factors shall change the rate of successful collisions and hence the reaction rate.

Changes in concentration influence the number of particles per unit space.
Changes in temperature influence both the rate of collision and the percentage of particles with sufficient energy of reaction.

For reactions that involve gases,

Changing the volume of the container will change the concentration of gases and change the reaction rate.

However, there are cases where the number of gases particles on the reactant side and the product side are equal. Rates of the forward and backward reaction will change by the same extent. In such cases, there will not be a change in the final concentrations. Similarly, catalysts change the two rates by the same extent and will not change the final concentrations. Adding noble gases will also change the pressure. However, concentrations stay the same and the equilibrium position will not change.

8 0

3 years ago

Nitrogen and water react to form nitrogen monoxide and hydrogen, like this: N2(g) + 2H2O(g) → 2NO(g) +2H2(g) Also, a chemist fin

Thepotemich [5.8K]

Answer:

Kc for this reaction is 0.43

Explanation:

This is the equilibrium:

N₂(g) + 2H₂O(g) → 2NO(g) +2H₂(g)

And we have all the concentration at equilibrium:

N₂: 0.25M

H₂ : 1.3M

NO: 0.33M

H₂: 1.2M

They are ok, because they are in MOLARITY. (mol/L)

Let's make the expression for Kc

Kc = ( [NO]² . [H₂]² ) / ([N₂] . [H₂O]²)

Kc = (0.33² . 1.2²) / (0.25 . 1.2²)

Kc = 0.4356

In two significant digits. 0.43

8 0

3 years ago

Is this right, I feel like its wrong

hjlf

It is correct, next time re-check your answer and don't second guess yourself. ;3

7 0

3 years ago

A reaction mixture initially contains 0.140 MCO and 0.140 MH2O. What will be the equilibrium concentration of CO?

Allushta [10]

Answer:

0.013 M

Explanation:

From the question, we can make the following deductions; we are given mixture that contains two compounds, that is A and B, 0.140 M CO and 0.140 M H2O respectively. Then, we are asked to find the equilibrium concentration of Carbonmonoxide,CO.

So, the equation for the reaction is given below;

CO + H2O <-----------------> CO2 + H2.

Initially: we have 0.14M of CO, 0.14M of H2O and zero (0) concentration of CO2 and H2.

At time,t = CO =0.14 - x , H2O = 0.14 - x, CO2 and H2 = x.

The above reaction consist of the forward reaction and the backward reaction.

Therefore, the equilibrium Concentration of CO;

(Since we are giving that Kc = 102). Then, Kc= [CO2][H2] ÷ [CO][H2O]. Where Kc is the equilibrium constant.

Therefore, 102 = [x^2] / [0.14 - x]^2.

==> 10.1= x/0.14 - x.

====> 0.141 - 10.1 x = x.

x + 10.1 x = 0.141.

===> 11.1 x = 0.141.

===> x = 0.141 ÷ 11.1.

===> x = 0.127 M .

Then, at time,t CO = 0.14 - x.

= 0.14 - 0.127 = 0.013 M

8 0

4 years ago

Read 2 more answers

Leonard designed a parallel circuit to light two light bulbs. But his circuit doesn’t work. Which two items in the circuit must

klasskru [66]

Answer : When a parallel circuit is built the voltage across each of the components remains the same, also the total current passed is the equal to sum of the currents passing through each components in the circuits.

When 2 or more components are tried to be connected in parallel they maintain the same potential difference (in voltage) across their ends of the circuit.

The potential differences across the components are the observed to be same in magnitude, and they have identical polarities between them.

Then, this same voltage is applicable to all circuit components connected in parallel.

So, if each bulb is wired to the battery in a separate loop, the bulbs will be in parallel series.

3 0

3 years ago