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Andru [333]
4 years ago
10

What best describes the collisions between ideal gas molecules?

Chemistry
1 answer:
Serggg [28]4 years ago
5 0

The molecules are continually colliding with each other and with the walls of the container. When a molecule collides with the wall, they exert small force on the wall The pressure exerted by the gas is due to the sum of all these collision forces. The more particles that hit the walls, the higher the pressure.

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How many grams of peroxide are produced from 3.00 mold of oxygen gas​
const2013 [10]

Answer:3 moles of Oxygen atoms weigh 48.00 grams.

Explanation:

7 0
3 years ago
The reaction below is at dynamic equilibrium. Upper N subscript 2 (g) plus 3 upper H subscript 2 (g) double-headed arrow 2 upper
Len [333]

For the reaction below at dynamic equilibrium, it is true that the rate of the forward reaction equals the rate of the reverse reaction.

Let's consider the following reaction at equilibrium.

N₂(g) + 3 H₂(g) = 2 NH₃(g)

<h3>What is the chemical equilibrium?</h3>

Is a state in which the concentrations of reactants and products are constant and the forward reaction rate and constant reaction rate are equal.

<h3>What is the equilibrium constant?</h3>

The equilibrium constant (K) is the ratio of the concentrations of the products to the concentrations of the reactants, all raised to their stoichiometric coefficients.

Let's consider which statement is true for the equilibrium system.

  • The concentration of NH₃ is greater than the concentration of N₂. FALSE. There is not enough information to confirm this, we would need to know the value of K.
  • The concentration of NH₃ equals the concentration of N₂. FALSE. There is not enough information to confirm this, we would need to know the value of K.
  • The rate of the forward reaction equals the rate of the reverse reaction. TRUE. This is always true for a reaction at equilibrium.
  • The rate of the forward reaction is greater than the rate of the reverse reaction. FALSE. At equilibrium, both rates are equal.

For the reaction below at dynamic equilibrium, it is true that the rate of the forward reaction equals the rate of the reverse reaction.

Learn more about chemical equilibrium here: brainly.com/question/5081082

3 0
3 years ago
Read 2 more answers
Mezclar mantequilla y azúcar es químico oh físico ?
klio [65]
<h3>answer:</h3><h3>es un cambio fisico</h3>

8 0
3 years ago
Do you expect the O---O bond in H2O2 to be longer or shorter than the O---O bond in O2?
melomori [17]

Answer : The O-O bond in H_2O_2 will be longer than the O-O bond in O_2.

Explanation :

In the H_2O_2, the two oxygen atoms are bonded by the single bond and in O_2, the two oxygen atoms are bonded by the double bond.

As we know, the bond strength of double bond is greater than the single bond.

And the relation between the bond strength and bond length is,

\text{ Bond strength}\propto \frac{1}{\text{ Bond length}}

That means the higher the strength, the shorter will be the bond length.

Hence, the bond length of single bond will be longer than the double bond.

The structure of given molecule is shown below.

8 0
4 years ago
In addition to those in Table 14.3, other less stable nitrogen oxides exist. Draw a Lewis structure for each of the following:(c
Natalka [10]

Lewis structure for each of the following N₂O₃ with no N¬N bond is attached below.

Even though pi symmetry occupies the antibonding orbitals of NO, this is unimportant after the dimer forms. A sigma connection exists. The enthalpy of the newly formed sigma bond in the dimer is low because the loss of a particularly distinctive set of single-electron resonance forms that were available for no monomer offset the net gain in bond. When the whole free energy is taken into account, there is no gain because the entropic effects are on the order of 1030kJ/mol, and dimerization is entropically disfavored at G=17kJ/mol. Therefore, any little increase in enthalpy is cancelled out by the loss of entropy.

Learn more about dimer here-

brainly.com/question/17152685

#SPJ4

5 0
2 years ago
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