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BigorU [14]
3 years ago
14

Place the following transitions of the hydrogen atom in order from longest to shortest wavelength of the photon emitted. Rank fr

om longest to shortest wavelength. To rank items as equivalent, overlap them. n=7 to n=4 n=5 to n=3 n=4 to n=2 n=3 to n=2
Chemistry
1 answer:
gizmo_the_mogwai [7]3 years ago
3 0

Answer:

7 to 4     (higher  \lambda)

5 to 3

3 to 2

4 to 2   (lower  \lambda)

Explanation:

We can use the Rydberg formula which relates the wavelength of the photon emissions to the principle quantum numbers involved in the transition:

\frac{1}{\lambda}=R((\frac{1}{n_1^2})-(\frac{1}{n_2^2}))

with n_1 final n, and n_2 initial n

evaluating for each transition:

7 to 4 \frac{1}{\lambda} = R((\frac{1}{4^2})-(\frac{1}{7^2}))= R(1/16-1/49)=R(0.042)

5 to 3 \frac{1}{\lambda}= R(1/9-1/25)=R(0.071)

4 to 2 \frac{1}{\lambda}= R(1/4-1/16)=R(0.1875)

3 to 2 \frac{1}{\lambda}= R(1/4-1/9)=R(0.139)

Note that the above formula is written for \frac{1}{\lambda}, so lower \frac{1}{\lambda} value obtained involves higher \lambda.

So we should order from lower to higher \frac{1}{\lambda}

7 to 4     (higher  \lambda)

5 to 3

3 to 2

4 to 2   (lower  \lambda)

Note: Take into account that longer wavelength involves lower energy (E=\frac{hc}{\lambda}).

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41 to
tia_tia [17]

Answer:

d = 0.9 g/L

Explanation:

Given data:

Number of moles = 1 mol

Volume = 24.2 L

Temperature = 298 K

Pressure = 101.3 Kpa (101.3/101 = 1 atm)

Density of sample = ?

Solution:

PV = nRT     (1)

n = number of moles

number of moles = mass/molar mass

n = m/M

Now we will put the n= m/M in equation 1.

PV = m/M RT   (2)

d = m/v

PM = m/v RT ( by rearranging the equation 2)

PM = dRT

d = PM/RT

The molar mass of neon is = 20.1798 g/mol

d = 1 atm × 20.1798 g/mol / 0.0821 atm. L/mol.K × 273K

d = 20.1798 g/22.413 L

d = 0.9 g/L

4 0
3 years ago
What is the mass, in grams, of 1.4 mol W
algol [13]
Atomic mass W = 183.84 u.m.a

1 mole --------- 183.84
1.4 moles ---- ?

1.4 x 183.84 / 1 = 257.376 g

hope this helps!
3 0
3 years ago
How many grams in 6.20 x 10^25 atoms of bromine (Br) ? image attached , will give brainliest
Deffense [45]

Answer:

8239.2g

Explanation:

Given parameters:

Number of atoms in Br  = 6.2 x 10²⁵atoms

Unknown:

Mass of Br = ?

Solution:

From mole concepts, we know that:

       1 mole of a substance contains 6.02 x 10²³ atoms/mol

 Molar mass of Br  = 80g/mol

6.2 x 10²⁵atoms  x \frac{1}{6.02 x 10^{23} } \frac{mol}{atoms} x  80 x \frac{g}{moles}  

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8 0
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Evgesh-ka [11]

Answer: The ionization of pure water forms <u><em>hydroxide and hydronium ions.</em></u>

Explanation:

Ionization is a reaction in the pure water in which water breaks down into its constituting ions that hydronium ion and hydroxide ions.

H_2O+H_2O\rightleftharpoons H_3O^++OH^-

One molecule of water looses its proton to form hydroxide ion and l=the lost protons get associated with another water molecule to form hydronium ion.

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3 years ago
How do I calculate the sum of 6.078 g and 0.3329 g ?
Vesnalui [34]
The answer is 6.4109 grams
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