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Chapter 3: Problem 46

Determine the empirical formula of each of the following compounds if a sample contains \((\mathbf{a})0.104 \mathrm{mol} \mathrm{K}, 0.052 \mathrm{mol}\) \(\mathrm{C},\) and \(0.156 \mathrm{mol} \mathrm{O} ;(\mathbf{b}) 5.28 \mathrm{g} \mathrm{Sn}\) and \(3.37 \mathrm{g} \mathrm{F} ;(\mathbf{c}) 87.5 \% \mathrm{N}\) and 12.5\(\% \mathrm{H}\) by mass.

Short Answer

Expert verified
The empirical formulas for the given compounds are: a) K2CO3 b) SnF4 c) NH2

Step by step solution

01

Identify the moles of each element

In this case, we are given the moles directly: 0.104 mol K, 0.052 mol C, and 0.156 mol O.
02

Divide by the smallest mole value

The smallest mole value is 0.052 mol (C). So, divide each mole value by 0.052. - K: 0.104/0.052 = 2 - C: 0.052/0.052 = 1 - O: 0.156/0.052 = 3
03

Write the empirical formula

The empirical formula for part a is K2C1O3 or K2CO3. ##Part b##
04

Convert mass to moles using the molar mass

We have 5.28 g Sn and 3.37 g F. Convert these masses to moles using the molar mass of the elements. - Sn: 5.28 g / 118.71 g/mol (Sn molar mass) ≈ 0.0445 mol - F: 3.37 g / 19.00 g/mol (F molar mass) ≈ 0.177 mol
05

Divide by the smallest mole value

The smallest mole value is 0.0445 mol (Sn). So, divide each mole value by 0.0445. - Sn: 0.0445/0.0445 = 1 - F: 0.177/0.0445 ≈ 4
06

Write the empirical formula

The empirical formula for part b is Sn1F4 or SnF4. ##Part c##
07

Convert mass percentages to moles

Assume a 100 g sample, then we have 87.5 g N and 12.5 g H. Convert these masses to moles using the molar mass of the elements. - N: 87.5 g / 14.01 g/mol (N molar mass) ≈ 6.245 mol - H: 12.5 g / 1.01 g/mol (H molar mass) ≈ 12.375 mol
08

Divide by the smallest mole value

The smallest mole value is 6.245 mol (N). So, divide each mole value by 6.245. - N: 6.245/6.245 = 1 - H: 12.375/6.245 ≈ 2
09

Write the empirical formula

The empirical formula for part c is N1H2 or NH2.

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Most popular questions from this chapter

Without doing any detailed calculations (but using a periodic table to give atomic weights, rank the following samples in order of increasing numbers of atoms: 42 gof NaHCO \(_{3}, 1.5 \mathrm{mol} \mathrm{CO}_{2}, 6.0 \times 10^{24} \mathrm{Ne}\) atoms.

Write a balanced chemical equation for the reaction that occurs when (a) \(\mathrm{Mg}(s)\) reacts with \(\mathrm{Cl}_{2}(g) ;\) (b) barium carbonate decomposes into barium oxide and carbon dioxide gas when heated; (c) the hydrocarbon styrene, \(\mathrm{C}_{8} \mathrm{H}_{8}(l),\) is combusted in air; (d) dimethylether, \(\mathrm{CH}_{3} \mathrm{OCH}_{3}(g),\) is combusted in air.

When a mixture of 10.0 g of acetylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)\) and 10.0 \(\mathrm{g}\) of oxygen \(\left(\mathrm{O}_{2}\right)\) is ignited, the resulting combustion reaction produces \(\mathrm{CO}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\) . (a) Write the balanced chemical equation for this reaction. (b) Which is the limiting reactant? (c) How many grams of \(\mathrm{C}_{2} \mathrm{H}_{2}, \mathrm{O}_{2}, \mathrm{CO}_{2},\) and \(\mathrm{H}_{2} \mathrm{O}\) are present after the reaction is complete?

Define the terms theoretical yield, actual yield, and percent yield. (b) Why is the actual yield in a reaction almost always less than the theoretical yield?(c) Can a reaction ever have 110\(\%\) actual yield?

Give the empirical formula of each of the following compounds if a sample contains (a) 0.0130 mol \(\mathrm{C}, 0.0390 \mathrm{mol}\) \(\mathrm{H},\) and \(0.0065 \mathrm{mol} \mathrm{O} ;\) (b) \(11.66 \mathrm{g}\) iron and 5.01 \(\mathrm{g}\) oxygen; (c) \(40.0 \% \mathrm{C}, 6.7 \% \mathrm{H},\) and 53.3\(\%\) o by mass.
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