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dmitriy555 [2]
3 years ago
7

A 100 watt bulb emits monochromatic light of wavelength 400 nm. Calculate the number of photons emitted per second by the bulb.

Chemistry
1 answer:
umka21 [38]3 years ago
4 0

Answer:

f = 7.5 E14 s-1

Explanation:

energy emitted by photon:

  • E = h.c / λ.......(1)
  • E = h.f......(2) Planck-Einstein

∴ λ = (400nm)(m/1 E9 nm) = 4.00 E-7 m

∴ h ( Planck's constant) = 6.626070150 E-34 J.s

∴ c (velocity of light) = 3.00 E8 m/s

∴ f (frequency): photon/s

If (1) = (2):

⇒ f = c / λ = E / h

⇒ f = (3.0 E8 m/s) / ( 4.00 E-7 m) = 7.5 E14 s-1

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Answer:

(8.3×40)+(8.3×71)

921.3grames

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Bauxite must go through two processes to produce aluminum metal. The yield of the Bayer process, which extracts aluminum oxide f
Mashcka [7]

The yield of aluminium obtained from 1 m^3 of bauxite is 419810 g

<h3>What is a Percent yield</h3>

A percent yield of a substance measures the amount of the substance actually obtained as a percentage ratio of expected yield.

Percent yield = actual yield / expected yield × 100%

<h3>How to calculate the mass of aluminium obtained from bauxite </h3>

From the data given:

40 % of the bauxite is converted to aluminium oxide.

Volume of bauxite = 1 m^3

40 % of 1 m^3 = 0.4 m^3

volume of aluminium oxide = 0.4 m^3

density of aluminium oxide = 3965 kg/m^3

  • Using mass = density × volume

mass of aluminium oxide = 0.4 × 3965 kg

mass of aluminium oxide = 1586 kg

Formula of aluminium oxide is Al203

molar mass of aluminium oxide = 102 g

  • percentage mass of aluminium in one mole of aluminium oxide = mass of aluminium / mass of aluminium oxide × 100 %

Percentage mass of aluminium in aluminium oxide = 54/102 × 100

Percentage mass of aluminium in aluminium oxide = 52.94 %

Expected mass of aluminium from aluminium oxide = 52.94 × 1586

Expected mass of aluminium = 839.62 kg

Actual yield = 40 % × 839.62

Actual yield of aluminium = 419.81 kg

mass of aluminium in grams = 419810 g

Therefore, mass of aluminium obtained from 1 m^3 of bauxite is 419810 g

Learn more about percent yield at: brainly.com/question/8638404

3 0
3 years ago
Which sequence represents the relationship between pressure and volume of an ideal gas as explained by the kinetic-molecular the
Nutka1998 [239]
Boyle's law which plays a major role in the kinetic-theory states that Volume and Pressure are inversely proportional 
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4 years ago
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why the total mass of the products would be less than the total weight of the reactant after a chemical reaction?
Lisa [10]
The best explanation would be that Gases were released during the Chemical reaction, causing a loss of Mass. 
4 0
3 years ago
You have 350 mL of 3.4 M hydrochloric acid (HCl). How many grams of HCl gas are dissolved? Bonus: what is the volume of the HCl
Crank

Answer:

1. 43.44g of HCl

2. 26.67 L of HCl

Explanation:

1) Molarity of a solution = number of moles (n) ÷ Volume (V)

According to the provided information in this question,

V = 350 mL = 350/1000 = 0.350L

Molarity = 3.4 M

Using Molarity = n/V

3.4 = n/0.350

n = 3.4 × 0.350

n = 1.19mol

Using the formula below to calculate the mass of HCl;

mole = mass/molar mass

Molar mass of HCl = 1 + 35.5 = 36.5g/mol

mole = mass/MM

mass = 1.19 mol × 36.5g/mol

mass = 43.44g of HCl

2) At STP, HCl has a pressure of 1atm, a temperature of 273K

V = ?

n = 1.19 mol

R = 0.0821 Latm/molK

Using PV = nRT

V = nRT/P

V = 1.19 × 0.0821 × 273/1

Volume = 26.67L

5 0
3 years ago
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