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Contact [7]
3 years ago
9

A 5.024 mg sample of an unknown organic molecule containing carbon, hydrogen, and nitrogen only was burned and yielded 13.90 mg

of CO2 and 6.048 mg of H2O. What is the empirical formula
Chemistry
1 answer:
Dafna1 [17]3 years ago
8 0

Answer:

C8H17N

Explanation:

Mass of the unknown compound = 5.024 mg

Mass of CO2 = 13.90 mg

Mass of H2O = 6.048 mg

Next, we shall determine the mass of carbon, hydrogen and nitrogen present in the compound. This is illustrated below:

For carbon, C:

Molar mass of CO2 = 12 + (2x16) = 44g/mol

Mass of C = 12/44 x 13.90 = 3.791 mg

For hydrogen, H:

Molar mass of H2O = (2x1) + 16 = 18g/mol

Mass of H = 2/18 x 6.048 = 0.672 mg

For nitrogen, N:

Mass N = mass of unknown – (mass of C + mass of H)

Mass of N = 5.024 – (3.791 + 0.672)

Mass of N = 0.561 mg

Now, we can obtain the empirical formula for the compound as follow:

C = 3.791 mg

H = 0.672 mg

N = 0.561 mg

Divide each by their molar mass

C = 3.791 / 12 = 0.316

H = 0.672 / 1 = 0.672

N = 0.561 / 14 = 0.040

Divide by the smallest

C = 0.316 / 0.04 = 8

H = 0.672 / 0.04 = 17

N = 0.040 / 0.04 = 1

Therefore, the empirical formula for the compound is C8H17N

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2.3 x 10²¹ particles H = __________ mol H (round to the nearest thousandth)
Natalka [10]

Taking into account the definition of avogadro's number, 3.82×10⁻³ moles of H are 2.3×10²¹ particles of H.

<h3>Avogadro's Number</h3>

Avogadro's Number or Avogadro's Constant is called the number of particles that make up a substance (usually atoms or molecules) and that can be found in the amount of one mole of said substance. Its value is 6.023×10²³ particles per mole. Avogadro's number applies to any substance.

<h3>This case</h3>

Then you can apply the following rule of three: if 6.023×10²³ particles are contained in 1 mole of H, then 2.3×10²¹ particles are contained in how many moles of H?

amount of moles of H= (2.3×10²¹ particles × 1 mole)÷ 6.023×10²³ particles

<u><em>amount of moles of H= 3.82×10⁻³ moles</em></u>

Finally, 3.82×10⁻³ moles of H are 2.3×10²¹ particles of H.

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7 0
2 years ago
How to find the Ka of an acid?
bonufazy [111]
We know that acids have a pH of under 7. 

We also need to:
Set up an ICE table for the chemical reaction.  Solve for the concentration of H3O+ using the equation for pH  Use the concentration of H3O+ to solve for the concentrations of the other products and reactants.
7 0
3 years ago
A 15.50 gram sample of a gas exerts a pressure of 1.40 atmospheres when held in an 8.00 liter at 22 °C. What is the molar mass (
Lostsunrise [7]

Answer:

33.5 g/mol

Explanation:

PV=nRT

(1.40 atm)(8.00 L)=n(0.08206)(295 K)

n=0.463 mol

15.50 g/0.463 mol=33.5 g/mol

3 0
3 years ago
PLEASE HELP ASAP
Lapatulllka [165]

Answer:

See explanation

Explanation:

We must first write the equation of the reaction as follows;

C3H8 + 5O2 ----> 3CO2 + 4H2O

Now;

We obtain the number of moles of C3H8 = 132.33g/44g/mol = 3 moles

So;

1 mole of C3H8 yields 3 moles of CO2

3 moles of C3H8 yields 3 × 3/1 = 9 moles of CO2

We obtain the number of moles of oxygen = 384.00 g/32 g/mol = 12 moles

So;

5 moles of oxygen yields 3 moles of CO2

12 moles of oxygen yields 12 × 3/5 = 7.2 moles of CO2

We can now decide on the limiting reactant to be C3H8

Therefore;

Mass of CO2 produced = 9 moles of CO2 × 44 g/mol = 396 g of CO2

Again;

1 moles of C3H8 yields 4 moles of water

3 moles of C3H8 yields 3 × 4/1 = 12 moles of water

Hence;

Mass of water = 12 moles of water × 18 g/mol = 216 g of water

In order to obtain the percentage yield from the reaction, we have;

b) Actual yield = 269.34 g

Theoretical yield = 396 g

Therefore;

% yield = actual yield/theoretical yield × 100/1

Substituting values

% yield = 269.34 g /396 g × 100

% yield = 68%

8 0
3 years ago
How many grams of hydrogen are necessary to react completely with 50.0 g of nitrogen
nlexa [21]

Answer:

25.0 grams

Explanation:

7 0
3 years ago
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