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kobusy [5.1K]
2 years ago
6

Calculate the mass of 2.50 mol of CH,OH(1). Show your work. Use the appropriate

Chemistry
1 answer:
Sophie [7]2 years ago
7 0

Answer:

80.1 grams

Explanation:

Find the molar mass of CH3OH first by using the periodic table values.

12.011 g/mol C + (1.008*3 g/mol H) + 15.999g/mol O + 1.008 g/mol H

=32.042 so that is the molar mass

Now that you have 2.50 moles of CH3OH, you can calculate the mass in g

2.50molCH3OH * (32.042g CH3OH / 1 mol CH3OH) = 80.105

32.042g / 1 mol is the same as 32.042 g/mol

Since there are 3 sig figs in the problem (2.50 has 3 sig figs), you round to 80.1 g CH3OH

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In the Proton category: symbol p, and +1 charge
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Which models of the atom include a structure that is mostly made of empty space?
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Thomson proposed this idea. Rutherford disproved it when he shot alpha particles at a gold sheet and they bounced back at him, proving that the alpha particles bounced off something aka the nucleus.

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Analyze and solve this partially completed galvanic cell puzzle. There are 4 electrodes each identified by a letter of the alpha
klasskru [66]

Complete Question

The complete question is shown on the first uploaded image

Answer:

The correct option is  E_{cell}__{AC}} = 0.94

Explanation:

  From the question we are told that

          the cell voltage for AD is  E_{cell}__{AD}} = 1.56V

From the data give we can see that

               E_{cell}__{AD}} - E_{cell}__{BD}} = E_{cell}__{AB}}

i.e           1.56 - 1.53 = 0.03

   In the same way we can say that

              E_{cell}__{AD}}-E_{cell}__{CD}} = E_{cell}__{AC}}

=>        E_{cell}__{AC}}=1.56- 0.62

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5 0
2 years ago
A 5.024 mg sample of an unknown organic molecule containing carbon, hydrogen, and nitrogen only was burned and yielded 13.90 mg
Dafna1 [17]

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

8 0
2 years ago
What would have happened to your results if during the dehydration some of the copper (ii) sulfate splatter out of the crucible-
lidiya [134]

Answer : The results would show more amount of water in the hydrated sample.

Explanation :

The amount of water of crystallization can be found by taking the masses of hydrated copper sulfate and anhydrous copper sulfate.

The difference in masses indicates the mass of water lost during dehydration process.

If during dehydration process, some of the copper sulfate spatters out of the crucible, then this would give us less mass for anhydrous sample than the actual.

As a result, the difference in masses of hydrated sample and the anhydrous sample would be more.

Therefore the results would show more amount of water in the hydrated sample.

4 0
2 years ago
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