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2 years ago

Entropy of a system decreases with decrease in Temperature T/F

Chemistry

1 answer:

Svet_ta [14]2 years ago

3 0

Answer: The given statement is true.

Explanation:

Entropy means the measure of randomness present in a substance. That is, an increase in temperature will lead cause more motion in the particles of a substance more will be their kinetic energy.

As a result, there will occur more collisions due to which randomness of molecules will increase. Hence, there will be increase in entropy.

So, when we decrease the temperature then there will be decrease in motion of particles. As a result, lesser number of collisions will take place between them. Hence, degree of randomness will also decrease.

Thus, we can conclude the statement entropy of a system decreases with decrease in temperature, is true.

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Consider the reaction given below.

Drupady [299]

Answer:

K = 0.167 s⁻¹

Explanation:

1) Rate law, at a given temperature:

Since all the data are obtained at the same temperature, the equilibrium constant is the same.

Since only reactants A and B participate in the reaction, you assume that the form of the rate law is:

r = K [A]ᵃ [B]ᵇ

2) Use the data from the table

Since the first and second set of data have the same concentration of the reactant A, you can use them to find the exponent b:

r₁ = (1.50)ᵃ (1.50)ᵇ = 2.50 × 10⁻¹ M/s

r₂ = (1.50)ᵃ (2.50)ᵇ = 2.50 × 10⁻¹ M/s

Divide r₂ by r₁: [ 2.50 / 1.50] ᵇ = 1 ⇒ b = 0

Use the first and second set of data to find the exponent a:

r₁ = (1.50)ᵃ (1.50)ᵇ = 2.50 × 10⁻¹ M/s

r₃ = (3.00)ᵃ (1.50)ᵇ = 5.00 × 10⁻¹ M/s

Divide r₃ by r₂: [3.00 / 1.50]ᵃ = [5.00 / 2.50]

2ᵃ = 2 ⇒ a = 1

3) Write the rate law

r = K [A]¹ [B]⁰ = K[A]

This means, that the rate is independent of reactant B and is of first order respect reactant A.

4) Use any set of data to find K

With the first set of data

r = K (1.50 M) = 2.50 × 10⁻¹ M/s ⇒ K = 0.250 M/s / 1.50 M = 0.167 s⁻¹

Result: the rate constant is K = 0.167 s⁻¹

6 0

3 years ago

Ammonia can be produced via the chemicalreaction

otez555 [7]

Answer:

3)The reaction is not at equilibrium and willproceed to the right.

Explanation:

The reaction quotient of an equilibrium reaction measures relative amounts of the products and the reactants present during the course of the reaction at particular point in the time.

It is the ratio of the concentration of the products and the reactants each raised to their stoichiometric coefficients. The concentration of the liquid and the gaseous species does not change and thus is not written in the expression.

Q < Kc , reaction will proceed in forward direction.

Q > Kc , reaction will proceed in backward direction.

Q = Kc , reaction at equilibrium.

Given that:

Q = $3.56\times 10^{-4}$

K = $6.02\times 10^{-2}$

Since, Q < K , reaction is not at equilibrium and will proceed to right, in forward direction.

3 0

3 years ago

13. How many moles of sodium hydroxide are needed to neutralize 50grams of sulfuric acid?

Phoenix [80]

Answer:

1.02mole

Explanation:

The reaction equation is given as:

2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O

Given:

Mass of H₂SO₄ = 50g

Unknown:

Number of moles of NaOH = ?

Solution:

To solve this problem, we first find the number of moles of the acid given;

Number of moles = $\frac{mass}{molar mass}$

Molar mass of H₂SO₄ = 2(1) + 32 + 4(16) = 98g/mol

Now;

Number of moles = $\frac{50}{98}$ = 0.51mole

From the balanced reaction equation:

1 mole of H₂SO₄ will be neutralized by 2 mole of NaOH

0.51 mole of H₂SO₄ will be neutralized by 2 x 0.51 = 1.02mole of NaOH

6 0

2 years ago

According to the periodic table, which of these elements will form an ion with a –2 charge? calcium

Serga [27]

Answer:

hfjfuufhdhdhjdjdjjdjjdudjfjfjjfjfjjfjf

6 0

2 years ago

Which of the following would be expected to have the lowest first ionization energy?

scoundrel [369]

Explanation:

o2- Due to lowest Zeff.

I had that question and my answer was this. because you did not put options.

4 0

2 years ago