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Serjik [45]
3 years ago
6

Two gases have the same temperature but different pressures. The kinetic-molecular theory does not predict that a. molecules in

both gases have the same average kinetic energies. b. molecules in the low-pressure gas travel farther before they collide with other molecules. c. both gases have the same densities. d. all collisions of the molecules are elastic.
Chemistry
1 answer:
olganol [36]3 years ago
8 0

Answer: Option (c) is the correct answer.

Explanation:

Kinetic molecular theory states that particles of a matter are continuously in motion and these molecules represent perfect elastic collision.

So, at the same temperature but different pressures the two gases will have all collisions of the molecules as elastic in nature. It is also possible that molecules in both gases have the same average kinetic energies under given conditions as their molecules might be moving with the same speed.

But we cannot determine the densities of these gases.

Thus, we can conclude that the kinetic-molecular theory does not predict that both gases have the same densities.

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Find the mass of 3.00 mol of acetic acid, C2H4O2.
Alexeev081 [22]
Molar mass 

C₂H₄O₂  = 60.0 g/mol

n = mass / molar mass

3.00 = mass / 60.0

m = 3.00 * 60.0

m = 180 g of <span>C₂H₄O₂ 

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5 0
3 years ago
The following data were obtained in a kinetics study of the hypothetical reaction A + B + C → products. [A]0 (M) [B]0 (M) [C]0 (
Vladimir [108]

Answer:

B. First order, Order with respect to C = 1

Explanation:

The given kinetic data is as follows:

A + B + C → Products

     [A]₀     [B]₀    [C]₀       Initial Rate (10⁻³ M/s)

1.   0.4      0.4     0.2       160

2.  0.2      0.4      0.4       80

3.   0.6     0.1       0.2       15

4.   0.2     0.1       0.2        5

5.   0.2     0.2      0.4       20

The rate of the above reaction is given as:

Rate = k[A]^{x}[B]^{y}[C]^{z}

where x, y and z are the order with respect to A, B and C respectively.

k = rate constant

[A], [B], [C] are the concentrations

In the method of initial rates, the given reaction is run multiple times. The order with respect to a particular reactant is deduced by keeping the concentrations of the remaining reactants constant and measuring the rates. The ratio of the rates from the two runs gives the order relative to that reactant.

Order w.r.t A : Use trials 3 and 4

\frac{Rate3}{Rate4}= [\frac{[A(3)]}{[A(4)]}]^{x}

\frac{15}{5}= [\frac{[0.6]}{[0.2]}]^{x}

3 = 3^{x} \\\\x =1

Order w.r.t B : Use trials 2 and 5

\frac{Rate2}{Rate5}= [\frac{[B(2)]}{[B(5)]}]^{y}

\frac{80}{20}= [\frac{[0.4]}{[0.2]}]^{y}

4 = 2^{y} \\\\y =2

Order w.r.t C : Use trials 1 and 2

\frac{Rate1}{Rate2}= [\frac{[A(1)]}{[A(2)]}]^{x}[\frac{[B(1)]}{[B(2)]}]^{y}[\frac{[C(1)]}{[C(2)]}]^{z}

we know that x = 1 and y = 2, substituting the appropriate values in the above equation gives:

\frac{160}{80}= [\frac{[0.4]}{[0.2]}]^{1}[\frac{[0.4]}{[0.4]}]^{2}[\frac{[0.2]}{[0.4]}]^{z}

1 = (0.5)^{z}

z = 1

Therefore, order w.r.t C = 1

8 0
3 years ago
What part of the atom determines if it will combine or break apart from other substances?
anzhelika [568]

<em>Answer:</em>

  • The atom consist of three parts, proton, neutron and electrons. The electrons determine that i will combine or beak from other substances.

<em>Explanation:</em>

The atom consist of three parts which are following

  • proton
  • neutron
  • electron

The proton and neutron form nucleus of an atom. It is present at center of an atom. They have positive charges, while electrons remained outside the nucleus in particular energy levels or shell around the nucleus.

During combination or breaking of substances ,only arrangements of electrons take place. The valence shell electrons decide whether they have to combine or not, while nucleus remained unchanged during any reactions.

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According to the ideal gas law, increasing the volume of a closed reaction container decreases the thermal energy because the
hichkok12 [17]

Answer:

b is ur answer the temputer does increase

Explanation:

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4. What are the characteristics of<br> the particles of matter?
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