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Chapter 3: Problem 44

Nickel reacts with sulfur to form a sulfide. If \(2.986 \mathrm{~g}\) of nickel reacts with enough sulfur to form \(5.433\) g of nickel sulfide, what is the simplest formula of the sulfide? Name the sulfide.

Short Answer

Expert verified
Answer: The simplest formula of the nickel sulfide compound is Ni₂S₃ and its name is Nickel(III) sulfide.

Step by step solution

01

Calculate moles of each element

Given the mass of nickel and nickel sulfide, we can determine the moles of nickel and sulfur in the compound by using their respective molar masses. The molar mass of nickel (Ni) is approximately 58.69 g/mol. Moles of Ni = \(\frac{2.986 \mathrm{~g}}{58.69 \mathrm{~g/mol}}\) = 0.0509 mol Now, we can find the mass of sulfur in the compound: Mass of S = Mass of nickel sulfide - Mass of nickel = 5.433 g - 2.986 g = 2.447 g The molar mass of sulfur (S) is approximately 32.06 g/mol. Moles of S = \(\frac{2.447 \mathrm{~g}}{32.06 \mathrm{~g/mol}}\) = 0.0763 mol
02

Determine mole ratio

Now we have the moles of nickel and sulfur in the sulfide compound. To find the simplest whole number ratio, we can divide both values by the smallest number of moles (in this case, moles of nickel). Mole ratio = \(\frac{0.0509 \mathrm{mol \: Ni}}{0.0509 \mathrm{mol \: Ni}}\) : \(\frac{0.0763 \mathrm{mol \: S}}{0.0509 \mathrm{mol \: Ni}}\) = 1:1.50 Since we want the simplest whole number ratio, we will multiply the mole ratio by 2: Simplified mole ratio = 2:3
03

Determine the simplest formula

Based on the mole ratio calculated in Step 2, the simplest formula of the nickel sulfide compound will have 2 nickel atoms and 3 sulfur atoms. Simplest formula: Ni\(_2\)S\(_3\)
04

Name the sulfide

Finally, let's name the sulfide according to the rules of naming chemical compounds. The compound is made up of nickel(Ni) and sulfur(S). The name of the compound will be: Nickel(III) sulfide So, the simplest formula of the sulfide is Ni\(_2\)S\(_3\) and its name is Nickel(III) sulfide.

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Most popular questions from this chapter

The isotope Si-28 has a mass of \(27.977\) amu. For ten grams of Si-28, calculate (a) the number of moles. (b) the number of atoms. (c) the total number of protons, neutrons, and electrons.

Cyanogen gas, \(\mathrm{C}_{2} \mathrm{~N}_{2}\), has been found in the gases of outer space. It can react with fluorine to form carbon tetrafluoride and nitrogen trifluoride. $$ \mathrm{C}_{2} \mathrm{~N}_{2}(g)+7 \mathrm{~F}_{2}(g) \longrightarrow 2 \mathrm{CF}_{4}(g)+2 \mathrm{NF}_{3}(g) $$ (a) How many moles of fluorine react with \(1.37\) mol of cyanogen? (b) How many moles of \(\mathrm{CF}_{4}\) are obtained from \(13.75 \mathrm{~mol}\) of fluorine? (c) How many moles of cyanogen are required to produce \(0.8974 \mathrm{~mol}\) of \(\mathrm{NP}_{3} ?\) (d) How many moles of fluorine will yield \(4.981 \mathrm{~mol}\) of nitrogen trifluoride?

One way to remove nitrogen oxide (NO) from smoke stack emissions is to react it with ammonia. $$ 4 \mathrm{NH}_{3}(g)+6 \mathrm{NO}(g) \longrightarrow 5 \mathrm{~N}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) $$ Calculate (a) the mass of water produced from \(0.839\) mol of ammonia. (b) the mass of NO required to react with \(3.402\) mol of ammonia. (c) the mass of ammonia required to produce \(12.0 \mathrm{~g}\) of nitrogen gas. (d) the mass of ammonia required to react with \(115 \mathrm{~g}\) of NO.

Write a balanced equation for (a) the reaction between fluorine gas and water to give oxygen difluoride and hydrogen fluoride gases. (b) the reaction between oxygen and ammonia gases to give nitrogen dioxide gas and water. (c) the burning of gold(III) sulfide in hydrogen to give gold metal and dihydrogen sulfide gas. (d) the decomposition of sodium hydrogen carbonate to sodium carbonate, water, and carbon dioxide gas. (e) the reaction between sulfur dioxide gas and liquid hydrogen fluoride to give sulfur tetrafluoride gas and water.

Write balanced equations for the reaction of sulfur with the following metals to form solids that you can take to be ionic when the anion is \(\mathrm{S}^{2-}\). (a) potassium (b) magnesium (c) aluminum (d) calcium (e) iron (forming \(\mathrm{Fe}^{2+}\) ions)
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