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Chapter 3: Problem 76

Nitrous oxide \(\left(\mathrm{N}_{2} \mathrm{O}\right)\) is also called "laughing gas." It can be prepared by the thermal decomposition of ammonium nitrate \(\left(\mathrm{NH}_{4} \mathrm{NO}_{3}\right)\). The other product is \(\mathrm{H}_{2} \mathrm{O}\). (a) Write a balanced equation for this reaction. (b) How many grams of \(\mathrm{N}_{2} \mathrm{O}\) are formed if 0.46 mole of \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) is used in the reaction?

Short Answer

Expert verified
The balanced equation for the reaction is NH4NO3 -> 2N2O + 2H2O. The mass of N2O formed is approximately 20.24 grams.

Step by step solution

01

Write the Unbalanced Chemical Equation

First, write down the unbalanced equation for the thermal decomposition of Ammonium nitrate (NH4NO3) producing Nitrous Oxide (N2O) and Water (H2O): \n\nNH4NO3 -> N2O + H2O
02

Balance the Chemical Equation

Now we need to balance the equation. This is done by adjusting the coefficients of the molecules until the number of atoms for each element is the same on both sides of the equation. The balanced chemical equation is as follows: \n\n NH4NO3 -> 2N2O + 2H2O
03

Calculate the Molar Mass of N2O

We need to calculate the molar mass of Nitrous oxide (N2O). We know the atomic masses of Nitrogen (N) and Oxygen (O) are approximately 14 and 16 respectively. Molar mass of N2O is thus calculated as follows: \n\n(2 * 14g/mol (for N)) + 16g/mol (for O) = 44g/mol
04

Calculate the Mass of N2O Formed

We can find the mass of Nitrous Oxide formed, given the number of moles and molar mass as follows: \n\n(0.46 mole) * (44 g/mole) = 20.24 g

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Most popular questions from this chapter

Peroxyacylnitrate (PAN) is one of the components of smog. It is a compound of \(\mathrm{C}, \mathrm{H}, \mathrm{N},\) and \(\mathrm{O} .\) Determine the percent composition of oxygen and the empirical formula from the following percent composition by mass: 19.8 percent \(\mathrm{C}, 2.50\) percent \(\mathrm{H}, 11.6\) percent \(\mathrm{N}\). What is its molecular formula given that its molar mass is about \(120 \mathrm{~g}\) ?

Hydrogen fluoride is used in the manufacture of Freons (which destroy ozone in the stratosphere) and in the production of aluminum metal. It is prepared by the reaction$$\mathrm{CaF}_{2}+\mathrm{H}_{2} \mathrm{SO}_{4} \longrightarrow \mathrm{CaSO}_{4}+2 \mathrm{HF}$$ In one process, \(6.00 \mathrm{~kg}\) of \(\mathrm{CaF}_{2}\) are treated with an excess of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and yield \(2.86 \mathrm{~kg}\) of \(\mathrm{HF}\). Calculate the percent yield of HF.

Nitric oxide (NO) reacts with oxygen gas to form nitrogen dioxide \(\left(\mathrm{NO}_{2}\right)\), a dark-brown gas: $$2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)$$ In one experiment 0.886 mole of NO is mixed with 0.503 mole of \(\mathrm{O}_{2}\). Calculate which of the two reactants is the limiting reactant. Calculate also the number of moles of \(\mathrm{NO}_{2}\) produced.

(a) For molecules having small molecular masses, mass spectrometry can be used to identify their formulas. To illustrate this point, identify the molecule that most likely accounts for the observation of a peak in a mass spectrum at 16 amu, 17 amu, 18 amu, and 64 amu. (b) Note that there are (among others) two likely molecules that would give rise to a peak at 44 amu, namely, \(\mathrm{C}_{3} \mathrm{H}_{8}\) and \(\mathrm{CO}_{2} .\) In such cases, a chemist might try to look for other peaks generated when some of the molecules break apart in the spectrometer. For example, if a chemist sees a peak at 44 amu and also one at 15 amu, which molecule is producing the 44 -amu peak? Why? (c) Using the following precise atomic masses \(-\mathrm{H}\) ( 1.00797 amu), \({ }^{12} \mathrm{C}(12.00000 \mathrm{amu}),\) and \({ }^{16} \mathrm{O}(15.99491 \mathrm{amu})-\) how precisely must the masses of \(\mathrm{C}_{3} \mathrm{H}_{8}\) and \(\mathrm{CO}_{2}\), be measured to distinguish between them?

The following is a crude but effective method for estimating the order of magnitude of Avogadro's number using stearic acid \(\left(\mathrm{C}_{18} \mathrm{H}_{36} \mathrm{O}_{2}\right)\) shown here. When stearic acid is added to water, its molecules collect at the surface and form a monolayer; that is, the layer is only one molecule thick. The crosssectional area of each stearic acid molecule has been measured to be \(0.21 \mathrm{nm}^{2}\). In one experiment it is found that \(1.4 \times 10^{-4} \mathrm{~g}\) of stearic acid is needed to form a monolayer over water in a dish of diameter \(20 \mathrm{~cm} .\) Based on these measurements, what is A vogadro's number?
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