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Chapter 2: Problem 97

When \(10.0 \mathrm{g}\) zinc and \(8.0 \mathrm{g}\) sulfur are allowed to react, all the zinc is consumed, \(14.9 \mathrm{g}\) zinc sulfide is produced, and the mass of unreacted sulfur remaining is (a) \(2.0 \mathrm{g}\) (b) \(3.1 g\) (c) \(4.9 \mathrm{g}\) (d) impossible to predict from this information alone

Short Answer

Expert verified
The mass of the unreacted sulfur remaining is \(3.1 \mathrm{g}\).

Step by step solution

01

Identify the mass of the initial reactants

The mass of the initial reactants are given in the problem statement: 10.0g zinc and 8.0g sulfur. So total mass of the initial reactants is \(10.0 \mathrm{g} + 8.0 \mathrm{g} = 18.0 \mathrm{g}\).
02

Calculate the mass of the zinc sulfide produced

All the zinc is consumed and 14.9g of zinc sulfide is produced. This gives us the total mass of the reaction products.
03

Find the mass of the unreacted sulfur

The mass of unreacted sulfur can be found by subtracting the mass of the zinc sulfide produced from the total mass of the initial reactants. That is \(18.0 \mathrm{g} - 14.9 \mathrm{g} = 3.1 \mathrm{g}\). Thus the remaining mass of sulfur is 3.1g.

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Most popular questions from this chapter

There are three common iron-oxygen compounds. The one with the greatest proportion of iron has one Fe atom for every \(\mathrm{O}\) atom and the formula \(\mathrm{FeO}\). A second compound has 2.327 g Fe per \(1.000 \mathrm{g} \mathrm{O},\) and the third has \(2.618 \mathrm{g}\) Fe per \(1.000 \mathrm{g}\) O. What are the formulas of these other two iron-oxygen compounds?

The following data on isotopic masses are from a chemical handbook. What is the ratio of each of these masses to that of\(^{12}_{6} \mathrm{c}\) ?\( \)^{17}_{35} \mathrm{CL}\( , 34.96885 \mathrm{u} ;\) (b) \(_{12}^{26} \mathrm{Mg}\) 25.98259 u ;\(^{86}_{222} \mathrm{Rn}\) , 222.0175 u.

There are three naturally occurring isotopes of magnesium. Their masses and percent natural abundances are \(23.985042 \mathrm{u}, 78.99 \% ; 24.985837 \mathrm{u}, 10.00 \% ;\) and \(25.982593 \mathrm{u}, 11.01 \% .\) Calculate the weighted-average atomic mass of magnesium.

The mass of a carbon-12 atom is taken to be exactly 12 u. Are there likely to be any other atoms with an exact integral (whole number) mass, expressed in u? Explain.

An isotope with mass number 44 has four more neutrons than protons. This is an isotope of what element?
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