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Alona [7]
2 years ago
13

Because rusting is a spontaneous process under standard conditions, which of the following is a correct conclusion about the pro

cess?
OA "Delta G' is positive and 'DeltaH' is greater than the product of temperature and Deltas
OB. "Delta' is positive and the product of temperature and Deltas' is greater than 'DeltaH'.
O c.
Deltag'is negative and the product of temperature and Deltas" is greater than "Delta".
Delta G' is negative and 'DeltaH' is greater than the product of temperature and Deltas.
OD
Chemistry
2 answers:
lawyer [7]2 years ago
5 0

The correct conclusion about the process is that "DeltaG" is negative and the product of temperature and "DeltaS" is greater than "DeltaH". That is option C

Spontaneous reaction are natural reactions that occurs without depending on energy from external sources.

A typical example of a spontaneous reaction is the rusting of iron.

To know if a reaction is spontaneous, second law of thermodynamics is used through Gibbs free energy.

At standard conditions ( constant temperature and pressure), Gibbs free energy(G) is equal to enthalpy change(ΔH) minus product of temperature(T) and the entropy change (ΔS) of the system.

That is, ΔG =ΔH −TΔS,

Entropy (S) is a measure of the degree of disorderliness of a system.

Enthalpy (H) is the heat of the reaction which is positive when heat is given out or negative when heat is absorbed.

From the formula, when ∆G is less than 0, the reaction is said to be spontaneous.

For ∆G to be less than 0, this means ∆H(DeltaH) is less than 0 and T∆ S( product of temperature and "DeltaS") is greater than 0 to achieve a negative value for ∆G(DeltaG)

Therefore, DeltaG" is negative and the product of temperature and "DeltaS" is greater than "DeltaH".

Learn more about spontaneous reaction here:

brainly.com/question/24376583

bezimeni [28]2 years ago
3 0

A spontaneous reaction is known by the fact that ΔG is negative and the product of temperature and ΔS is greater than ΔH.

<h2>Spontaneity in chemical reactions</h2>

A chemical reaction is said to be spontaneous when it can proceed on its own without any further input of energy. Recall that;

ΔG = ΔH - TΔS

Where;

  • ΔG = change in free energy
  • ΔH = change in enthalpy
  • T = temperature
  • ΔS = change in entropy

Hence, a reaction is spontaneous when ΔG is negative and the product of temperature and ΔS is greater than ΔH.

Learn more about spontaneous reaction:brainly.com/question/1217654

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Which types of electron orbitals will have higher energy than a 4d orbital?
alexdok [17]

Answer:

D) 4f

Explanation:

To determine which electron orbital that will have higher energy than a 4d orbital, we write the electron configuration starting with s-orbital.

1s

2s         2p

3s         3p          3d       3f

4s         4p          4d       4f

5s         5p           5d       5f

6s         6p          6d       6f

7s         7p           7d       7f

In ascending order, 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 3f, <u>4d</u><em>,</em> 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 6f, 7d, 7f.

From the electronic configuration formula above, the electron orbitals that have higher energy than a 4d orbital are 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 6f, 7d, 7f.

Therefore, 4f is the correct answer.

8 0
3 years ago
1) Which of the following is the best example of a physical change?
never [62]

1 is b and 2 is also b

4 0
3 years ago
A radioactive isotope of potassium (K) has a half-life of 20 minutes. If a 40.0 gram sample of this isotope is allowed to decay
Ivahew [28]

Answer: 2.5 grams

Explanation:

5 0
3 years ago
Read 2 more answers
Using this formula, to find K, what does E0 represent?
Marysya12 [62]
The correct answer would be A. The symbol Eo would represent the cell potential of an electrolytic cell. This potential is being created by two metals that possess different properties. The energy per charge that is available from the reaction of the metals is the measure of this potential and is related to the equilibrium constant, K.
6 0
3 years ago
Read 2 more answers
Using the van der Waals equation, determine the pressure of 500.0 g of SO2(g) in a 6.30-L vessel at 633 K. For SO2(g), a = 6.865
dem82 [27]

Answer:

The pressure is 58.75 atm.

Explanation:

From Vanderwaal's equation,

P = nRT/(V-nb) - n^2a/V^2

n is the number of moles of SO2 = mass/MW = 500/64 = 7.81 mol

R is gas constant = 0.0821 L.atm/mol.K

T is temperature of the vessel = 633 K

V is volume of the vessel = 6.3 L

a & b are Vanderwaal's constant = 6.865 L^2.atm/mol^2 and 0.0567 L/mol respectively.

P = (7.81×0.0821×633)/(6.3 - 7.81×0.05679) - (7.81^2 × 6.865)/6.3^2 = 69.30 - 10.55 = 58.75 atm

4 0
3 years ago
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