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University of Toronto

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Problem 24

Answer

$\mathrm{N}(\mathrm{O})=1,43^{*} 10^{24}$ atoms

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## Discussion

## Video Transcript

So we have to find a number off all such an atom. Ah, we're being 38. Porn still, Grandma. Oxygen gas, which is also there. My assaulted from the longing around 50 minutes when a person is an address. Okay, First off, for all we have to pay attention that we're looking at the lumber off hostages atom So individual, not attractive. And we have 38 porn, zero grandma sausage in gas and have to remind you that for oxygen, gas is also your molecules is over too. Well, first of all, we had to fire the lumbar More sausages? Yes, first, So ah, number more off oxygen. Uh, molecule. So there's always your safari. Six point Ah, point. Oh, over the morning mass off oxygen. So, facial surgeon, you're 16 or two times six Team Graham Permal and essentially is the floor. It's true. So we have 30 60 Wild by referred me to you for start 48 e y by ferry to you and then we should be able to find that it should be equal. So roughly 1.1, uh, most okay, but this is the number one most off you know to So the actual bone, most off individual oxygen for your for each other, More molecule of two oxygen. So we just wouldn't move by this lumber bites you. So 1.19 times two. We have 2.38 Uh, both. All right. So very comfortable. Most to, um the lumber mark you. So it's number off hostage and walk you. We just need to take the lumber almost multiplied by ivory guys. Your lumber. And then we have to lumber off, um, atoms. All atoms for individual atoms. So and then for this kid, Yes. And then we got going to use our code later. We should be able to find out. Is what? The 1.43 times 10 to the power 24 atoms. And he's the answers.

## Recommended Questions

Determine the number of oxygen atoms present in

25.0 g of carbon dioxide.

The metabolic oxidation of glucose, $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6},$ in our bodies produces $\mathrm{CO}_{2},$ which is expelled from our lungs as a gas:

$$\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(a q)+6 \mathrm{O}_{2}(g) \longrightarrow 6 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l)$$

(a) Calculate the volume of dry $\mathrm{CO}_{2}$ produced at body temperature $\left(37^{\circ} \mathrm{C}\right)$ and 0.970 atm when 24.5 $\mathrm{g}$ of glucose is consumed in this reaction. (b) Calculate the volume of oxygen you would need, at 1.00 $\mathrm{atm}$ and $298 \mathrm{K},$ to completely oxidize 50.0 $\mathrm{g}$ of glucose.

Given the information in Problem 17, calculate the mass of oxygen gas that would be necessary to burn 0.0275 mol of hydrogen gas.

What mass of oxygen is required to burn

688 g of octane, $\mathrm{C}_{8} \mathrm{H}_{18},$ completely?

One liter of oxygen has a mass of $1.4 \mathrm{g},$ and the oxygen molecule has a mass of 32 amu. How many oxygen molecules are in 1 L of oxygen?

When eaten, dietary carbohydrates are digested to yield glucose $\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right),$ which is then metabolized to yield carbon dioxide and water:

$\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}+\mathrm{O}_{2} \longrightarrow \mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O} \quad$ Unbalanced

Balance the equation, and calculate both the mass in grams and the volume in liters of the $\mathrm{CO}_{2}$ produced from 66.3 $\mathrm{g}$ of glucose, assuming that 1 $\mathrm{mol}$ of $\mathrm{CO}_{2}$ has a volume of 25.4 $\mathrm{L}$ at normal body temperature.

Oxygen for First Responders In self-contained breathing devices used by first responders, potassium superoxide, $\mathrm{KO}_{2}$ reacts with exhaled carbon dioxide to produce potassium carbonate and oxygen:

$$4 \mathrm{KO}_{2}(s)+2 \mathrm{CO}_{2}(g) \rightarrow 2 \mathrm{K}_{2} \mathrm{CO}_{3}(s)+3 \mathrm{O}_{2}(g)$$

How much $\mathrm{O}_{2}$ could be produced from $85 \mathrm{g} \mathrm{KO}_{2} ?$

A self-contained breathing apparatus uses canisters containing potassium superoxide. The superoxide consumes the $\mathrm{CO}_{2}$ exhaled by a person and replaces it with oxygen.

$$

4 \mathrm{KO}_{2}(\mathrm{s})+2 \mathrm{CO}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{K}_{2} \mathrm{CO}_{3}(\mathrm{s})+3 \mathrm{O}_{2}(\mathrm{g})

$$

What mass of $\mathrm{KO}_{2}$, in grams, is required to react with $8.90 \mathrm{L}$ of $\mathrm{CO}_{2}$ at $22.0^{\circ} \mathrm{C}$ and $767 \mathrm{mm}$ Hg?

How many grams of oxygen gas are necessary to react completely with $3.01 \times 10^{21}$ atoms of magnesium to yield magnesium oxide?

Glucose is the major fuel for most living cells. The oxidative breakdown of glucose by our body to produce energy is called respiration. The reaction for the complete combustion of glucose is

$$

\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(s)+6 \mathrm{O}_{2}(g) \longrightarrow 6 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l)

$$

If this combustion reaction could be harnessed as a fuel cell, calculate the theoretical voltage that could be produced at standard conditions. (Hint: Use $\Delta G_{\mathrm{f}}^{\circ}$ values from Appendix 4.)