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Chapter 3: Problem 142

What mass of sodium hydroxide has the same number of oxygen atoms as 100.0 \(\mathrm{g}\) of ammonium carbonate?

Short Answer

Expert verified
The mass of sodium hydroxide (NaOH) that has the same number of oxygen atoms as 100.0 g of ammonium carbonate (NH₄)₂CO₃ is 41.6 g.

Step by step solution

01

Find the molecular mass of ammonium carbonate

In order to find the number of moles of ammonium carbonate in the given mass, we need to determine its molecular mass. Ammonium carbonate has a chemical formula of (NH₄)₂CO₃ which means it has 2(NH₄) and 1(CO₃) in a single molecule. Molecular mass of NH₄ = 1 N + 4 H = 14.01 + 4(1.01) = 18.05 g/mol Molecular mass of CO₃ = 1C + 3O = 12.01 + 3(16.00) = 60.01 g/mol Since there are 2(NH₄) and 1(CO₃), the molecular mass of ammonium carbonate is: Molecular mass of (NH₄)₂CO₃ = 2(18.05) + 60.01 = 36.10 + 60.01 = 96.11 g/mol
02

Calculate the moles of ammonium carbonate and oxygen atoms

Now we will find the moles of ammonium carbonate using the given mass and molecular mass. Moles of ammonium carbonate = Given mass / Molecular mass Moles of ammonium carbonate = 100.0 g / 96.11 g/mol = 1.04 mol Since there is only one oxygen atom (in CO₃) for each ammonium carbonate molecule, the moles of oxygen atoms will also be 1.04 mol.
03

Find the molecular mass of sodium hydroxide

To calculate the mass of sodium hydroxide (NaOH) that has the same number of moles of oxygen atoms, we need to first find the molecular mass of sodium hydroxide. Molecular mass of NaOH = 1 Na + 1 O + 1 H = 22.99 + 16.00 + 1.01 = 40.00 g/mol
04

Calculate the mass of sodium hydroxide with the same moles of oxygen atoms

Now we know that we have 1.04 moles of oxygen atoms, and we will find the mass of sodium hydroxide that has the same number of moles of oxygen atoms using its molecular mass: Mass of NaOH = Moles of oxygen atoms x Molecular mass of NaOH Mass of NaOH = 1.04 mol x 40.00 g/mol = 41.6 g Therefore, the mass of sodium hydroxide that has the same number of oxygen atoms as 100.0 g of ammonium carbonate is 41.6 g.

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Most popular questions from this chapter

Boron consists of two isotopes, 10 \(\mathrm{B}\) and 11 \(\mathrm{B}\) . Chlorine also has two isotopes, 35 \(\mathrm{Cl}\) and 37 \(\mathrm{Cl}\) . Consider the mass spectrum of \(\mathrm{BCl}_{3}\) . How many peaks would be present, and what approximate mass would each peak correspond to in the BCl_ mass spectrum?

Determine the molecular formula of a compound that contains $26.7 \% \mathrm{P}, 12.1 \% \mathrm{N},\( and \)61.2 \% \mathrm{Cl},$ and has a molar mass of 580 \(\mathrm{g} / \mathrm{mol}\)

You take 1.00 g of an aspirin tablet (a compound consisting solely of carbon, hydrogen, and oxygen), burn it in air, and collect 2.20 $\mathrm{g} \mathrm{CO}_{2}\( and 0.400 \)\mathrm{g} \mathrm{H}_{2} \mathrm{O} .$ You know that the molar mass of aspirin is between 170 and 190 $\mathrm{g} / \mathrm{mol}\( . Reacting 1 \)\mathrm{mole}$ of salicylic acid with 1 mole of acetic anhydride \(\left(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{3}\right)\) gives you 1 mole of aspirin and 1 mole of acetic acid $\left(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2}\right)$ Use this information to determine the molecular formula of salicylic acid.

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Consider the following reaction: $$ 4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g) $$ If a container were to have 10 molecules of \(\mathrm{O}_{2}\) and 10 molecules of \(\mathrm{NH}_{3}\) initially, how many total molecules (reactants plus products) would be present in the container after this reaction goes to completion?
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