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2 years ago

What is the mass (in grams) of 3.03 × 1024 molecules of carbon dioxide molecules?

1 answer:

5 0

1 mole of CO2 has 6.02 x 10^23 molecules of CO2. Say x moles of CO2 has 3.0x10^23 molecules of CO2. Therefore x = 3/6.02 = 0.50. M = 0.50 * (12 + 2x16) = 0.50 * 44 = 22g

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Chlorine gas reacts with aluminum metal producing aluminum chloride. What mass of chlorine reacts with 9.00g of Al to form AlCl3

Anit [1.1K]

The mass of chlorine that react with 9.00 g of Al to form AlCl3 is 35.465 grams

Explanation
write the equation for reaction
that is
2 Al + 3 Cl2 = 2 Al CL3
find the moles of Al reacted

moles = mass/molar mass

9 g/ 27 g/mol = 0.333 moles of Al

by use of mole ratio between Al to Cl2 which is 2:3 find the moles of Cl2

mole of cl2 = 0.333 x3/2 = 0.4995 moles

mass of Cl2 is therefore = moles x molar mass

= 0.4995 x71 = 35.465 moles

6 0

3 years ago

Which statement best describes visible light?

tekilochka [14]

Answer:

The Visible Spectrum Visible light is the light that we can see, and thus is the only light detectable by the human eye. White light is visible light, and it contains all the colors of the rainbow, from red to violet. The range of visible wavelengths is 400 to 700 nanometers.

Explanation:

6 0

3 years ago

1. Write the balanced chemical reaction for silver metal reacting with phosphoric acid to form

Anon25 [30]

<h3>Answer:</h3>

75.51%

<h3>Solution and Explanation:</h3>

Balanced equation: 6Ag(s) + 2H₃PO₄(aq) → 2Ag₃PO₄(aq) + 3H₂(g)

To determine the percent yield of silver phosphate we will use the following steps;

Step 1: Determine the number of moles of Silver metal used

Mass of silver metal = 50.00 grams

Molar mass of silver is 107.87 g/mol

Therefore;

Moles of silver = 50.0 g ÷ 107.87 g/mol

= 0.464 moles

Step 2: Determine moles of silver phosphate produced

From the equation, 6 moles of Ag reacts with 2 moles of phosphoric acid to yield 2 moles of silver phosphate.

Thus, the mole ratio of silver metal to silver phosphate is 6 : 2

Therefore;

Moles of Ag₃PO₄ = Moles of Ag × 2/6

= 0.464 moles × 2/6

= 0.155 moles

Step 3: Calculate the theoretical mass of silver phosphate produced

Mass = Number of moles × Molar mass

Number of moles of Ag₃PO₄= 0.155 moles

Molar mass of Ag₃PO₄ =418.58 g/mol

Therefore;

Theoretical mass of Ag₃PO₄ = 0.155 moles × 418.58 g/mol

= 64.88 g

Step 4: Calculate the percent yield of Ag₃PO₄

$percent yield=\frac{Actual mass}{Theoretical mass}(100)$

Actual mass of Ag₃PO₄ = 48.99 g

Theoretical mass of Ag₃PO₄ = 64.88 g

Therefore;

% yield of Ag₃PO₄ = (48.99 g ÷ 64.88 g)×100%

= 75.51%

Hence, the percent yield of Ag₃PO₄ is 75.51%

6 0

3 years ago

Is the graph o. the function increasing, decreasing, or constant?

Rainbow [258]

Y you just don’t wanna see it lol I love you

4 0

3 years ago

A ground-state H atom absorbs a photon of wavelength 94.91 nm, and its electron attains a higher energy level. The atom then emi

vitfil [10]

The intermediate energy level that the electron reached from the ground state is; n= 3.

<h3>What are energy levels in an atom?</h3>

The fixed distances from an atom's nucleus where electrons may be found are referred to as energy levels (also known as electron shells). Higher energy electrons have greater energy as you move out from the nucleus.

A region of space within an energy level known as an orbital is where an electron is most likely to be found.

The formula to get the higher level is Rydberg's formula;

1/λ = R(1/n₁² - 1/n₂²)

where;

R is rydberg constant = 1.097 × 10⁷ m⁻¹

We want to find the intermediate level where wavelength = 1281 nm = 1281 × 10⁻⁹ m

Thus;

$\frac{1}{1280(10^{-9})} = 1.097*10^{7}(\frac{1}{n_{2}^{2}}-\frac{1}{5^{2}}) \\0.0712=\frac{1}{n_{2}^{2}}-\frac{1}{25} \\\frac{1}{n_{2}^{2}}=0.0712+\frac{1}{25}\\\frac{1}{n_{2}^{2}}=0.1112$

n₂ = √(1/0.1112)

n₂ ≈ 3

To know more about energy levels, visit: brainly.com/question/10763798

#SPJ4

5 0

2 years ago