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2 years ago

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Chemistry

1 answer:

vichka [17]2 years ago

7 0

Answer:

1. 0.1683 mol

2. 1.191 g

3. 0.02695 mol

4. Na₂Cl₃

5. The empirical formula obtained is not correct. This is likely due to experimental errors, since much precision was required (the masses are determined in thousandths of grams).

Explanation:

1. How many moles of elemental sodium were used in the reaction?

Since all of the solid sodium is used up by the reaction, you can cancluate the number of moles of elemental sodium used dividing the mass by the molar mass:

number of moles = mass in grams / atomic mass

mass in grams = 0.3870 g (given)

atomic mass = 22.990 g/mol

number of moles = 0.3870 g / 22.990 g/mol = 0.1683 mol

2. What is the mass of chlorine gas used in the reaction?

a) Mass of chlorine gas introduced in the flask = mass of the stoppered flask after filling it with chlorine gas - mass of the empty flask with the sopper

Mass of chlorine gas introduced = 158.1743g - 156.1870g = 1.9873 g

b) Mass of chlorine gas unreacted = 0.7962 g (given)

c) Mass of chlorine gas used = mass of chorine gas introduced in the flask - mass of chlorine gass un reacted

Mass of chlorine gas used = 1.9873g - 0.7962g = 1.1911g

3. How many moles of chlorine were used in the reaction?

molar mass of chlorine gas, Cl₂ = 2 × 35.453 g/mol = 70.906 g/mol

number of moles = mass in grams / molar mass = 1.911g / 70.906g/mol = 0.02695 mol

4. What is the empirical formula of sodium chloride based on the experimental data?

Divide the number of moles of each element by the smalles number of moles:

Na: 0.01683 / 0.01683 = 1

Cl = 0.02695 / 0.01683 = 1.6

Multiply by 2 to obtain whole numbers:

Na = 2

Cl = 3.2 = 3

Empirical formula Na₂Cl₃

5. Was the empirical formula you obtained correct using the chemists data correct? Why?

No, the empirical formula you obtained using the chemists data is not correct, because the correct empirical formula of sodium chloride is NaCl.

That is, there is 1 atom of sodium per every atom of chlorine in one chemical formula of NaCl, but that is not reflected by the empirical formula Na₂Cl₃.

That is a demostration of big experimental errors. You can speculate that the errors are likely due to problems of procedure collecting the gas or errors in measuring the masses.

As you see, the masses are measured to thousandths of grams, which requires much precision; thus smalls absolute errors could produce huge relative errors.

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Here we have to calculate the heat required to raise the temperature of water from 85.0 ⁰F to 50.4 ⁰F.

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