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3 years ago

Which of the following types of electromagnetic energy carries the most energy

Chemistry

2 answers:

Dmitrij [34]3 years ago

7 0

<h2><em>it is X-rays. because i had it on a question and got it right.</em></h2>

netineya [11]3 years ago

5 0

<span>Radio waves have photons with low energies, microwave photons have a little more energy than radio waves, infrared photons have still more, then visible, ultraviolet, X-rays, and, the most energetic of all, gamma-rays.</span>

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If 15 grams of Carbon dioxide is produced in a chemical reaction, how many grams of Carbon must be consumed in the reaction if w

guajiro [1.7K]

Answer:

Quantity of Carbon is 4.09 gm

Explanation:

Equation of carbon reacting with oxygen to give carbon dioxide is given by

C + $O_{2}$ ⇒ C $O_{2}$

One mole of carbon reacts with one mole of Oxygen in this reaction to give One mole of Carbon dioxide.

So, 12 gm of carbon reacts with 32 gm of Oxygen in this reaction to give 44 gm of carbon dioxide.

15 gm of C $O_{2}$ was formed in this reaction

Oxygen used in this reaction = $\frac{15}{44}$ ×32 = 10.91 gm ,

Thus Oxygen is in sufficient quantity in the reaction.

Now,

Carbon that must be used = $\frac{15}{44}$ ×12 = 4.09 gm.

5 0

3 years ago

How can you determine the quantities of reactants and products in a chemical reaction

prohojiy [21]

Use the balanced equation.

5 0

3 years ago

Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 to the n

Gre4nikov [31]

Answer:

The wavelength of the light emitted by a hydrogen atom for the given transition is 2166 nm.

Explanation:

The energy of nth energy levels of the H atom is given as:

$E_n = -2.18 \times 10^{-18} \times \frac{1}{n^2} J$

Energy of the seventh energy level = $E_7$

$E_7=-2.18 \times 10^{-18} \times \frac{1}{7^2} J$

$E_7=-2.18 \times 10^{-18} \times \frac{1}{7^2} J=-4.4490\times 10^{-20} J$

Energy of the seventh energy level = $E_4$

$E_4=-2.18 \times 10^{-18} \times \frac{1}{4^2} J$

$E_4=-2.18 \times 10^{-18} \times \frac{1}{16} J=-1.3625\times 10^{-19} J$

Energy of the light emitted will be equal to the energy difference of the both levels.

$E=E_7-E_4=-4.4490\times 10^{-20} J-(-1.3625\times 10^{-19} J)$

$E=9.176\times 10^{-20} J$

Wavelength corresponding to energy E can be calculated by using Planck's equation:

$E=\frac{hc}{\lambda }$

$\lambda =\frac{hc}{E}=\frac{6.626\times 10^{-34} Js\times 3\times 10^8 m/s}{9.176\times 10^{-20} J}=2.166\times 10^{-6} m=2166 nm$

The wavelength of the light emitted by a hydrogen atom for the given transition is 2166 nm.

8 0

3 years ago

What volume measured in stp will 3.75 grams of helium gas occupy?

Andre45 [30]

Molar mass helium gas :

He = 4.0 g/mol

number of moles: 3.75 / 4.0 => 0.9375 moles

1 mole ------ 22.4 ( at STP)
0.9375 ------ ?

volume = 0.9375 x 22.4 / 1

Volume = 21 / 1

Volume = 21 L

hope this helps!

6 0

3 years ago

How many grams of oxygen is needed to completely react with 9.30 moles of aluminum

Orlov [11]

Balanced chemical equation:

* moles of oxygen

4 Al + 3 O2 = 2 Al2O3

4 moles Al -------------- 3 moles O2
9.30 moles Al ---------- moles O2

moles O2 = 9.30 * 3 / 4

moles O2 = 27.9 / 4 => 6.975 moles of O2

Therefore:

Molar mass O2 = 31.9988 g/mol

n = m / mm

6.975 = m / 31.9988

m = 6.975 * 31.9988

m = 223.19 of O2

5 0

3 years ago