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Chapter 3: Problem 71

If chlorine bleach is mixed with other cleaning products containing ammonia, the toxic gas \(\mathrm{NCl}_{3}(g)\) can form according to the equation $$3 \mathrm{NaClO}(a q)+\mathrm{NH}_{3}(a q) \longrightarrow 3 \mathrm{NaOH}(a q)+\mathrm{NCl}_{3}(g)$$ When \(2.94 \mathrm{~g}\) of \(\mathrm{NH}_{3}\) reacts with an excess of \(\mathrm{NaClO}\) according to the preceding reaction, how many grams of \(\mathrm{NCl}_{3}\) are formed?

Short Answer

Expert verified
So, when 2.94 grams of \(NH_{3}\) reacts with an excess of \(NaClO\), 12.32 grams of \(NCl_{3}\) are formed.

Step by step solution

01

Identify the Balanced Chemical Equation

The balanced chemical equation is given as: \(3 NaClO(aq) + NH_{3}(aq) \to 3 NaOH(aq) + NCl_{3}(g)\). From the balanced equation, it can be observed that 1 mole of \(NH_{3}\) reacts to form 1 mole of \(NCl_{3}\). Therefore, the stoichiometry of the reaction between \(NH_{3}\) and \(NCl_{3}\) is 1:1.
02

Calculate the number of moles of \(NH_{3}\)

The number of moles of \(NH_{3}\) can be calculated using its molar mass (17.03 g/mol) and given mass (2.94 g) as follows: \(\frac{2.94 \, g}{17.03 \, g/mol} = 0.1727 \, mol\)
03

Calculate the number of moles of \(NCl_{3}\) formed

Since the stoichiometry between \(NH_{3}\) and \(NCl_{3}\) is 1:1, the number of moles of \(NCl_{3}\) that forms is equal to the number of moles of \(NH_{3}\) reacted, which is 0.1727 moles.
04

Calculate the mass of \(NCl_{3}\) formed

The mass of \(NCl_{3}\) can be calculated using its molar mass (71.37g/mol) and number of moles (0.1727 mol) as follows: \(0.1727 \, mol \times 71.37 \, g/mol = 12.32 \, g\)

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Most popular questions from this chapter

Octane \(\left(\mathrm{C}_{8} \mathrm{H}_{18}\right)\) is a component of gasoline. Complete combustion of octane yields \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{CO}_{2} .\) Incomplete combustion produces \(\mathrm{H}_{2} \mathrm{O}\) and CO, which not only reduces the efficiency of the engine using the fuel but is also toxic. In a certain test run, 1.000 gal of octane is burned in an engine. The total mass of \(\mathrm{CO}, \mathrm{CO}_{2},\) and \(\mathrm{H}_{2} \mathrm{O}\) produced is \(11.53 \mathrm{~kg} .\) Calculate the efficiency of the process; that is, calculate the fraction of octane converted to \(\mathrm{CO}_{2}\). The density of octane is \(2.650 \mathrm{~kg} / \mathrm{gal}\)

Avogadro's number has sometimes been described as a conversion factor between atomic mass units and grams. Use the fluorine atom ( 19.00 amu) as an example to show the relation between the atomic mass unit and the gram.

Propane \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)\) is a component of natural gas and is used in domestic cooking and heating. (a) Balance the following equation representing the combustion of propane in air.$$\mathrm{C}_{3} \mathrm{H}_{8}+\mathrm{O}_{2} \longrightarrow \mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}$$ (b) How many grams of carbon dioxide can be produced by burning 3.65 moles of propane? Assume that oxygen is the excess reactant in this reaction.

Carbon dioxide \(\left(\mathrm{CO}_{2}\right)\) is the gas that is mainly responsible for global warming (the greenhouse effect). The burning of fossil fuels is a major cause of the increased concentration of \(\mathrm{CO}_{2}\) in the atmosphere. Carbon dioxide is also the end product of metabolism (see Example 3.13 ). Using glucose as an example of food, calculate the annual human production of \(\mathrm{CO}_{2}\) in grams, assuming that each person consumes \(5.0 \times 10^{2} \mathrm{~g}\) of glucose per day. The world's population is 7.2 billion, and there are 365 days in a year.

A research chemist used a mass spectrometer to study the two isotopes of an element. Over time, she recorded a number of mass spectra of these isotopes. On analysis, she noticed that the ratio of the taller peak (the more abundant isotope) to the shorter peak (the less abundant isotope) gradually increased with time. Assuming that the mass spectrometer was functioning normally, what do you think was causing this change?
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