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Molodets [167]
3 years ago
14

Determine the number of moles of compound and the number of moles of each type of atom in each of the following:

Chemistry
1 answer:
den301095 [7]3 years ago
5 0

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}     .....(1)

  • <u>For a:</u>

Mass of propylene = 25 g

Molar mass of propylene = 42 g/mol

Putting values in equation 1, we get:

\text{Moles of }C_3H_8=\frac{25g}{42g/mol}=0.6mol

In 1 mole of propylene, 3 moles of carbon atoms and 8 moles of hydrogen atoms are present.

So, in 0.6 moles of propylene, (3\times 0.6)=1.8mol of carbon atoms and (8\times 0.6)=4.8mol of hydrogen atoms are present.

Thus, the number of moles of compound is 0.6 moles and number of moles of carbon and hydrogen atoms are 1.8 moles and 4.8 moles respectively.

  • <u>For b:</u>

Mass of glycine = 3.06\times 10^{-3}g

Molar mass of glycine = 75 g/mol

Putting values in equation 1, we get:

\text{Moles of glycine}=\frac{3.06\times 10^{-3}g}{75g/mol}=4.08\times 10^{-5}mol

In 1 mole of glycine, 2 moles of carbon atoms, 5 moles of hydrogen atoms, 1 mole of nitrogen atom and 2 moles of oxygen atoms are present.

So, in 4.08\times 10^{-5}mol of glycine, (2\times 4.08\times 10^{-5})=8.16\times 10^{-5}mol of carbon atoms, (5\times 4.08\times 10^{-5})=2.04\times 10^{-4}mol of hydrogen atoms, (1\times 4.08\times 10^{-5})=4.08\times 10^{-5}mol of nitrogen atoms and (2\times 4.08\times 10^{-5})=8.16\times 10^{-5}mol of oxygen atoms are present.

Thus, the number of moles of compound is 4.08\times 10^{-5}mol moles and number of moles of carbon, hydrogen, nitrogen and oxygen atoms are 8.16\times 10^{-5}mol, 2.04\times 10^{-4}mol, 4.08\times 10^{-5}mol and 8.16\times 10^{-5}mol respectively.

  • <u>For c:</u>

Mass of Treflan = 25 lbs = 11350 g   (Conversion factor: 1 lbs = 454 g)

Molar mass of Treflan = 283.28 g/mol

Putting values in equation 1, we get:

\text{Moles of Treflan}=\frac{11350g}{283.28g/mol}=40mol

In 1 mole of treflan, 13 moles of carbon atoms, 16 moles of hydrogen atoms, 2 mole of nitrogen atom, 4 moles of oxygen atoms and 1 mole of fluorine are present.

So, in 40.03 moles of treflan, (13\times 40)=520mol of carbon atoms, (16\times 40)=640mol of hydrogen atoms, (2\times 40)=80mol of nitrogen atoms, (4\times 40)=160mol of oxygen atoms and (1\times 40)=40mol of fluorine atoms are present.

Thus, the number of moles of compound is 40 moles and number of moles of carbon, hydrogen, nitrogen, oxygen and fluorine atoms are 520 moles, 640 moles, 80 moles, 160 moles and 40 moles respectively.

  • <u>For d:</u>

Mass of Paris green = 0.125 kg = 125 g    (Conversion factor: 1 kg = 1000 g)

Molar mass of Paris green = 618.11 g/mol

Putting values in equation 1, we get:

\text{Moles of Paris green}=\frac{125g}{618.11g/mol}=0.202mol

In 1 mole of Paris green, 4 moles of carbon atoms, 6 moles of hydrogen atoms, 4 moles of copper atom, 10 moles of oxygen atoms and 2 moles of arsenic are present.

So, in 0.202 moles of Paris green, (4\times 0.202)=0.808mol of carbon atoms, (6\times 0.202)=1.212mol of hydrogen atoms, (4\times 0.202)=0.808mol of copper atoms, (10\times 0.202)=2.02mol of oxygen atoms and (2\times 0.202)=0.404mol of arsenic atoms are present.

Thus, the number of moles of compound is 0.202 moles and number of moles of carbon, hydrogen, copper, oxygen and arsenic atoms are 0.808 moles, 1.212 moles, 0.808 moles, 2.02 moles and 0.404 moles respectively.

  • <u>For e:</u>

Mass of Aspirin = 325 mg = 0.325 g    (Conversion factor: 1 g = 1000 mg)

Molar mass of aspirin = 180.16 g/mol

Putting values in equation 1, we get:

\text{Moles of aspirin}=\frac{0.325g}{180.16g/mol}=0.0018mol

In 1 mole of aspirin, 9 moles of carbon atoms, 8 moles of hydrogen atoms and 4 moles of oxygen atoms are present.

So, in 0.0018 moles of aspirin, (9\times 0.0018)=0.0162mol of carbon atoms, (8\times 0.0018)=0.0144mol of hydrogen atoms and (4\times 0.0018)=0.0072mol of oxygen atoms are present.

Thus, the number of moles of compound is 0.0018 moles and number of moles of carbon, hydrogen and oxygen are 0.0162 moles, 0.0144 moles and 0.0072 moles respectively.

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determine the frequency and wavelength (in nm) of the light emitted when the e- fell from n=4 and n=2
Lostsunrise [7]

Answer:

Frequency = 6.16 ×10¹⁴ Hz

λ = 4.87×10² nm

Explanation:

In case of hydrogen atom energy associated with nth state is,

En =  -13.6/n²

For n = 2

E₂ = -13.6 / 2²

E₂ = -13.6/4

E₂ = -3.4 ev

Kinetic energy of electron = -E₂ = 3.4 ev

For n = 4

E₄ = -13.6 / 4²

E₄ = -13.6/16

E₄ = -0.85 ev

Kinetic energy of electron = -E₄ = 0.85 ev

Wavelength of radiation emitted:

E = hc/λ = E₄ - E₂

hc/λ = E₄ - E₂

by putting values,

6.63×10⁻³⁴Js × 3×10⁸m/s / λ = -0.85ev   - (-3.4ev )

6.63×10⁻³⁴ Js× 3×10⁸m/s / λ = 2.55 ev

λ = 6.63×10⁻³⁴ Js× 3×10⁸m/s  /2.55ev

λ = 6.63×10⁻³⁴ Js× 3×10⁸m/s  /2.55× 1.6×10⁻¹⁹ J

λ = 19.89 ×10⁻²⁶ Jm / 2.55× 1.6×10⁻¹⁹ J

λ = 19.89 ×10⁻²⁶ Jm / 4.08×10⁻¹⁹ J

λ = 4.87×10⁻⁷ m

m to nm:

4.87×10⁻⁷ m ×10⁹nm/1 m

4.87×10² nm

Frequency:

Frequency = speed of electron / wavelength

by putting values,

Frequency = 3×10⁸m/s /4.87×10⁻⁷ m

Frequency = 6.16 ×10¹⁴ s⁻¹

s⁻¹ = Hz

Frequency = 6.16 ×10¹⁴ Hz

3 0
3 years ago
In which system does a spontaneous redox reaction produce electrical energy?
Vladimir [108]
Had to look for the options and here is my answer.
When we say that a redox reaction is spontaneous, this would mean that there is a formation of positive voltage <span>across the electrodes of a voltaic cell. Therefore, the system that this kind of reaction produces electrical energy is in a GALVANIC CELL. Hope this helps.</span>
3 0
3 years ago
How many grams of HNO3 are produced when 59.0 g of NO2 completely reacts?
Anettt [7]

Answer:

53.7 grams of HNO3 will be produced

Explanation:

Step 1: Data given

Mass of NO2 = 59.0 grams

Molar mass NO2 = 46.0 g/mol

Step 2: The balanced equation

3NO2 + H2O→ 2HNO3 + NO

Step 3: Calculate moles NO2

Moles NO2 = 59.0 grams / 46.0 g/mol

Moles NO2 = 1.28 moles

Step 4: Calculate moles HNO3

For 3 moles NO2 we need 1 mol H2O to produce 2 moles HNO3 and 1 mol NO

For 1.28 moles NO2 we'll have 2/3 * 1.28 =0.853 moles HNO3

Step 7: Calculate mass HNO3

Mass HNO3 = 0.853 moles * 63.01 g/mol

Mass HNO3 = 53.7 grams

53.7 grams of HNO3 will be produced

3 0
3 years ago
Determine the empirical formula of the compound formed when 1.2g of magnesium reacts with 3.55g of chlorine.Take the molar mass
masha68 [24]

Explanation:

For Mg, (1.2 g Mg/24 g Mg) = 0.05 mol Mg.

For Cl, (3.55 g Cl/35.5 g Cl) = 0.1 mol Cl

So the ratio now is

Mg:Cl = 0.05 : 0.1 = 1:2

I got the 1:2 ratio by dividing both by the smallest number, which is 0.05 mol. Therefore, the empirical for formula of the substance is MgCl_2

5 0
3 years ago
Rays used to take pictures of bones in the human body are:
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Answer:

B

Explanation:

Because when you go to the doctors they say, "You need to get your x-rays done" not microwave

5 0
3 years ago
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