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jenyasd209 [6]
4 years ago
11

Compare green and red light from the visible spectrum. which has: the longer wavelength? the greater frequency? the greater ener

gy?
Chemistry
2 answers:
Artist 52 [7]4 years ago
6 0
The spectrum goes as follows:
red, orange, yellow, green, blue, indigo and violet
Red has the lowest frequency.
Since frequency is inversely proportional to the wavelength, therefore, red has the longest wavelength.

Now, consider, the equation:
E = (hc) / lambda
Since the energy is inversely proportional to the wavelength, therefore, red will have the lowest energy.

Based on this, for the mentioned question:
1- Red has longer wavelength
2- Green has greater frequency
3- Green has greater energy
Romashka-Z-Leto [24]4 years ago
4 0
<span>Red light will have the longer wavelength (in fact, has the longest wavelength in the visible spectrum). As frequency is the inverse of wavelength, this means that green will have the greater frequency. In addition, since frequency and energy have a direct relationship, green light will also have the greater amount of energy.</span>
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How many moles are in 1.0 x 109 atoms of Zn?
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Answer:

1.66×10^-15

Explanation:

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8 0
3 years ago
How many moles of caco3 are there in an antacid tablet containing 0.515 g caco3?
MaRussiya [10]
The  moles  of  CaCO3  which  are  there  in  antacid  tablet  that  contain  0.515g  CaCO3  is  calculated  as  follows

moles  =mass/molar  mass

the  molar  mass  of  CaCO3 =  ( 40  x1)+  (12  x  1)  + (16 x  3)=  100  g/mol

moles  is  therefore=  0.515g/100 g/mol=  5.15  x10^-3  moles


8 0
3 years ago
Read 2 more answers
If the Sun were much smaller than its current size, what effect would this have on eclipses?
sergiy2304 [10]
Total solar eclipses would be more common, because it would be easier for the moon to cover it, which is a solar eclipse.
8 0
3 years ago
The compound known as diethyl ether, commonly referred to as ether, contains carbon, hydrogen, and oxygen. A 1.751 g sample of e
fredd [130]

<u>Answer:</u> The empirical formula for the given compound is C_{4}H_{10}O

<u>Explanation:</u>

The chemical equation for the combustion of ether follows:

C_xH_yO_z+O_2\rightarrow CO_2+H_2O

where, 'x', 'y' and 'z' are the subscripts of carbon, hydrogen and oxygen respectively.

We are given:

Mass of CO_2=4.159g

Mass of H_2O=2.128g

Mass of sample = 1.751 g

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

<u>For calculating the mass of carbon:</u>

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 4.159 g of carbon dioxide, \frac{12}{44}\times 4.159=1.134g of carbon will be contained.

<u>For calculating the mass of hydrogen:</u>

In 18 g of water, 2 g of hydrogen is contained.

So, in 2.128 g of water, \frac{2}{18}\times 2.128=0.236g of hydrogen will be contained.

Mass of oxygen in the compound = (1.751) - (1.134 + 0.236) = 0.381 g

To formulate the empirical formula, we need to follow some steps:

  • <u>Step 1:</u> Converting the given masses into moles.

Moles of Carbon = \frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{1.134g}{12g/mole}=0.0945moles

Moles of Hydrogen = \frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{0.236g}{1g/mole}=0.236moles

Moles of Oxygen = \frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{0.381g}{16g/mole}=0.0238moles

  • <u>Step 2:</u> Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.0238 moles.

For Carbon = \frac{0.0945}{0.0238}=3.97\approx 4

For Hydrogen = \frac{0.236}{0.0238}=9.91\approx 10

For Oxygen = \frac{0.0238}{0.0238}=1

  • <u>Step 3:</u> Taking the mole ratio as their subscripts.

The ratio of C : H : O = 4 : 10 : 1

Hence, the empirical formula for the given compound is C_{4}H_{10}O

7 0
3 years ago
The oxidation state for Cl is A. -1 as a reactant and +1 as a product B. -1 as a reactant and 0 as a product C. -1 as a reactant
Harlamova29_29 [7]

Answer:

no sure

Explanation:

8 0
3 years ago
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