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3 years ago

In the bohr model of the hydrogen atom, how does the radius of the electron’s orbit depend on the principal quantum number?

1 answer:

3 0

The radius of the electron's or basically the energy level for which the electron is found orbiting the nucleus of he hydrogen atom, as the principal quantum number tells us primarily the energy level that the electron will be found, is it the 1st, 2nd, and 3rd. The other quantum numbers tells us more specifically as per the subshell of the main shell the electron is in, the spin of the electron etc.

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piece of copper iron silver and gold are dropped into a solution of iron sulphate the piece that will get a coating of a copper

torisob [31]

Pieces of copper, silver and gold are dropped into a solution of iron sulphate. The piece that will get a coating of copper is. ... Therefore, none of the three metals can displace iron from its salt solution. Hence, we observe that no reaction takes place and none of the pieces get coated.

5 0

3 years ago

Read 2 more answers

How many moles are in a 12.0 g sample of NiC12

Nady [450]

Answer:

0.17 moles

Explanation:

In the elements of the periodic table, the atomic mass = molar mass. <u>Ex:</u> Atomic mass of Carbon is 12.01 amu which means molar mass of Carbon is also 12.01g/mol.

In order to find the # of moles in a 12 g sample of NiC-12, we will need to multiply the number of each atom by its molar mass and then add the masses of both Nickel and C-12 found in the periodic table:

Molar Mass of Ni (Nickel): 58.69 g/mol

Molar Mass of C (Carbon): 12.01 g/mol

Since there's just one atom of both Carbon and Nickel, we just add up the masses to find the molar mass of the whole compound of NiC-12.

58.69 g/mol of Nickel + 12.01 g/mol of Carbon = 70.7 g/mol of NiC-12

There's 12g of NiC-12, which is less than the molar mass of NiC-12, so the number of moles should be less than 1. In order to find the # of moles in NiC-12, we need to do some dimensional analysis:

12g NiC-12 (1 mol of NiC-12/70.7g NiC-12) = 0.17 mol of NiC-12
The grams cancel, leaving us with moles of NiC-12, so the answer is 0.17 moles of NiC-12 in a 12 g sample.

<em>P.S. C-12 or C12 just means that the Carbon atom has an atomic mass of 12amu and a molar mass of 12g/mol, or just regular carbon.</em>

5 0

3 years ago

Which of these electron transitions correspond to absorption of energy and which to emission?

Keith_Richards [23]

The electron transitions representing absorption of energy are:

(a) n = 2 to n = 4

(d) n = 3 to n = 4

and those which represents emissions of energy are:

(b) n = 3 to n = 1

An electron emits energy when it jumps from a higher energy level to a lower energy level transitions.

An electron absorbs energy to jump from a lower energy level to a higher energy level transitions.

(a) n = 2 to n = 4

Here, the initial level (2) is lower than the final level (4).

Hence energy is absorbed.

(b) n = 3 to n = 1

Here, the initial level (3) is higher than the final level (1).

Hence energy is released.

Here, the initial level (5) is higher than the final level (2).

Hence energy is released.

(d) n = 3 to n = 4

Here, the initial level (3) is lower than the final level (4).

Hence energy is absorbed.

The question is incomplete. Find the complete question here:

Which of these electron transitions correspond to absorption of energy and which to emission?

(a) n = 2 to n = 4

(b) n = 3 to n = 1

(d) n = 3 to n = 4

Learn more about electron transitions at brainly.com/question/2079874

#SPJ4

4 0

2 years ago

Like all equilibrium constants, the value of Kw depends on temperature. At body temperature (37°C), Kw = 2.4 * 10-14. What are t

Aleksandr [31]

Answer:

pH = 6.8124

Explanation:

We know pH decreases with increase in temperature.

At room temperature i.e. 25⁰c pH of pure water is equal to 7

We know

Kw = [H⁺][OH⁻]...............(1)

where Kw = water dissociation constant

At equilibrium [H⁺] = [OH⁻]

So at 37⁰c i.e body temperature Kw = 2.4 × 10⁻¹⁴

From equation (1)

[H⁺]² = 2.4 × 10⁻¹⁴

[H⁺] = √2.4 × 10⁻¹⁴

[H⁺] = 1.54 × 10⁻⁷

pH = - log[H⁺]

= - log{1.54 × 10⁻⁷}

= 6.812

5 0

3 years ago

How long would it take for 1.50 mol of water at 100.0 ∘c to be converted completely into steam if heat were added at a constant

Aleksandr-060686 [28]

To determine the time it takes to completely vaporize the given amount of water, we first determine the total heat that is being absorbed from the process. To do this, we need information on the latent heat of vaporization of water. This heat is being absorbed by the process of phase change without any change in the temperature of the system. For water, it is equal to 40.8 kJ / mol.

Total heat = 40.8 kJ / mol ( 1.50 mol ) = 61.2 kJ of heat is to be absorbed

Given the constant rate of 19.0 J/s supply of energy to the system, we determine the time as follows:

Time = 61.2 kJ ( 1000 J / 1 kJ ) / 19.0 J/s = 3221.05 s

5 0

3 years ago

Read 2 more answers