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3 years ago

The red line of the hydrogen emission spectrum has a wavelength of 656.1 nm. Calculate the energy of one photon

Chemistry

1 answer:

Effectus [21]3 years ago

4 0

The formula we can use here is the Plancks equation:

E = h c / ʎ

where h is Plancks constant = 6.626 × 10-34 m2 kg / s, c is speed of light = 3 x 10^8 m/s and ʎ is wavelength = 656.1 x 10^-9 m

Therefore E is:

E = (6.626 × 10-34 m2 kg / s) * (3 x 10^8 m/s) / 656.1 x 10^-9 m

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What elements are being reduced and oxidized in this chemical formula?

dangina [55]

Answer: The element Na (Sodium) is getting oxidized and Hydrogen is getting reduced.

Explanation:

Oxidation reactions are the reactions in which addition of oxygen takes place.

Reduction reactions are the reactions in which loss of oxygen takes place.

For a given reaction:

$2Na(s)+2H_2O(l)\rightarrow H_2(g)+2NaOH(aq.)$

Sodium is getting oxidized because there is an addition of reaction with that element.

Hydrogen is getting reduced because there is a removal of oxygen with that element.

3 0

3 years ago

2C2H2(g)+5O2(g)=4CO2(g)+2H2O(g)

balandron [24]

The volume of ethyne, C₂H₂ required to produce 12 moles of CO₂ assuming the reaction is at STP is 134.4 L

<h3>Balanced equation</h3>

2C₂H₂(g) + 5O₂(g) --> 4CO₂(g) + 2H₂O(g)

From the balanced equation above,

4 moles of CO₂ were produced by 2 moles of C₂H₂

<h3>How to determine the mole of C₂H₂ needed to produce 12 moles of CO₂</h3>

From the balanced equation above,

4 moles of CO₂ were produced by 2 moles of C₂H₂

Therefore,

12 moles of CO₂ will be produce by = (12 × 2) / 4 = 6 moles of C₂H₂

<h3>How to determine the volume (in L) of C₂H₂ needed at STP</h3>

At standard temperature and pressure (STP),

1 mole of C₂H₂ = 22.4 L

Therefore,

6 moles of C₂H₂ = 6 × 22.4

6 moles of C₂H₂ = 134.4 L

Thus, we can conclude that the volume of C₂H₂ needed for the reaction at STP is 134.4 L

Learn more about stoichiometry:

brainly.com/question/14735801

#SPJ1

3 0

2 years ago

19. When an atom of iron loses all of its 4s electrons and one of its 3d electrons, what is its charge?

Snowcat [4.5K]

Its charge would be the amount of electrons that are lost in total, which the information is not stated

7 0

3 years ago

What is the total amount of heat released when 94.0 g water at 80.0 °C cools to form ice at −30.0 °C?

Wewaii [24]

Answer:

The total amount of heat released is 68.7 kJ

Explanation:

Given that:

mass of water = 94.0 g

moles of water = 94 / 18.02 = 5.216

80⁰C ------> 0⁰C --------> -30⁰C

Q1 = m Cp dT

= 94 x 4.184 x (0 - 80)

= -31463.68 J

= -31.43 kJ

Q2 = 6.01 x 10^3 x 5.216

= - 31348.16 J

= -31.35 kJ

Q3 = - 94 x 2.09 x 30

= - 5893.8 J

= -5.894 kJ

Total heat = Q1 + Q2 + Q3 = -31.43 kJ + (-31.35 kJ ) + (-5.894 kJ ) = -68.7 kJ

Total heat released = -68.7 kJ

Note that the "negative sign" simply indicates heat released, therefore no need to put it in the answer.

6 0

3 years ago

How many kj of heat are needed to completely vaporize 1.30 moles of h2o? the heat of vaporization for water at the boiling point

Cerrena [4.2K]

The Kj of heat that are needed to completely vaporize 1.30 moles of H2O if the heat of vaporization for water is 40.6 Kj/mole is calculated as below

Q(heat) = moles x heat of vaporization)

=1.30 mol x40.6 kj/mol= 52.78 Kj is needed

6 0

3 years ago

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