Question

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

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

Step-by-step solution

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

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

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\(_3\)

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.

Key concepts

Reaction Stoichiometry

Stoichiometry is an essential concept in chemistry used to predict the amounts of substances consumed and produced in a chemical reaction. It is based on the balanced chemical equation and relies on the conservation of mass principle. In the original exercise, stoichiometry allows us to determine how much sulfur is needed to fully react with a given mass of nickel to form nickel sulfide.

Here are some key points about reaction stoichiometry:

• Stoichiometry calculations start by determining the moles of each reactant involved in the reaction using their respective molar masses.
• The mole ratio between reactants and products is derived from the coefficients in the balanced chemical equation.
• Calculating these ratios helps to identify the limiting reactant and ensures the precise formulation of products like nickel sulfide.

By applying stoichiometry, the calculated mole ratio of nickel to sulfur led to the final determination that the simplest formula for nickel sulfide is Ni environments. To begin with, it's vital to identify the molecular formula of the substance. In this case, nickel sulfide, which informs us about the number of atoms of nickel and sulfur required in the chemical compound. From a stoichiometric point of view, these calculations help predict the exact ratio of nickel to sulfur to achieve the ideal formation of Ni₂S₃.

Nickel Sulfide

Nickel sulfide is a chemical compound formed by the combination of nickel and sulfur. This compound is significant in various industrial and chemical contexts, particularly in fields like metallurgy and electronics. In chemistry, the simplest formula for a compound signifies its most reduced form, representing the ratio of atoms within a molecule.

In the given exercise, nickel sulfide has a simplest formula of Ni effect, making it essential to understand how nickel sulfide reacts and forms.

Nickel sulfide can appear in different stoichiometries, such as NiS, NiS₂, and Ni₃S₂, depending on the specific conditions of the reaction and the initial proportions of nickel and sulfur used. The nickel sulfide discussed here, Ni₂S₃, has a specific structure and stoichiometry, reflective of the experimental data given. Understanding these structures and formulas not only enhances knowledge in chemistry but also has practical applications in industries where precise compound formulation is crucial.

Mole Calculation

Calculating moles is an essential skill in chemistry that allows chemists to quantify the amount of substance they are dealing with. In stoichiometry, it serves as the bridge from mass to the number of entities, such as atoms or molecules. The concept of "mole" is central to quantifying elements and compounds in chemical reactions.

Here's how you can calculate moles effectively:

• Start by measuring the mass of a given element or compound you have. This is your starting point.
• Use the molar mass, which is the mass of one mole of the substance, to convert from mass to moles. For example, nickel has a molar mass of approximately 58.69 g/mol.
• The formula to calculate moles is: Moles = Mass/Molar Mass.

In the original exercise, the number of moles of nickel and sulfur were calculated using these steps. Moles of nickel were found using its mass (2.986 g) and molar mass (58.69 g/mol), resulting in 0.0509 mol. Similarly, the moles of sulfur were derived from subtracting the mass of nickel from the total mass of the compound and dividing by the molar mass of sulfur (32.06 g/mol), which resulted in 0.0763 mol.

These calculations are vital for accurate stoichiometric results, enabling the determination of the simplest chemical formula for nickel sulfide, which is Ni₂S₃. Understanding mole calculations is fundamental to mastering chemistry and predicting reaction behaviors accurately.