investigation 51. for each pair listed, which has more representative particles?a. 1 mol $ ext{ocl}_2$ or 1 mol $ ext{h}_2 ext{o}$b. 0.5 mol $ ext{o}_2$ or 0.75 mol $ ext{h}_2$c. 1.5 mol $ ext{sno}$ or 3.0 mol $ ext{sno}_2$d. 0.33 mol $ ext{fe}_2 ext{o}_3$ or 0.66 mol $ ext{feo}$2. would you expect one mole of solid sodium, $ ext{na}$, to have the same volume as one mole of liquid bromine, $ ext{br}_2$? explain.3. how does the concept of the mole help chemists?4. explain how a mole of hydrogen peroxide ($ ext{h}_2 ext{o}_2$) and a mole of hydrogen chloride ($ ext{hcl}$) are the same but different.5. if one mole of an unknown substance is 200.59 g/mol, what is the mass of 0.33 mol of the substance?6. if you had one mole of avocados, then how many avocados would you have?7. a chemist has $3.45 imes 10^{22}$ molecules of $ ext{p}_2 ext{o}_5$. how many grams of $ ext{p}_2 ext{o}_5$ does the chemist have?8. calculate the number of moles of each substance.a. $5.45 imes 10^{26}$ molecules of methane, $ ext{ch}_4$b. $3.22 imes 10^{23}$ atoms of xenon, $ ext{xe}$c. $9.6 imes 10^{23}$ formula units of sodium chloride, $ ext{nacl}$9. how many moles of hydrogen atoms are in 7.10 mol of $ ext{h}_2 ext{o}$?10. how many moles of oxygen atoms are in 3.60 mol of $ ext{sio}_2$?11. what is the molar mass of molecular oxygen, $ ext{o}_2$?12. what is the molar mass of barium chloride, $ ext{bacl}_2$?13. what is the molar mass of $ ext{caco}_3$?14. what is the molar mass of $ ext{sf}_6$?15. calculate the number of moles of each substance.a. 6.00 g oxygen, $ ext{o}_2$b. 450.0 g of iron(iii) oxide, $ ext{fe}_2 ext{o}_3$c. 45.5 g of calcium chloride, $ ext{cacl}_2$

Question

investigation 51. for each pair listed, which has more representative particles?a. 1 mol $	ext{ocl}_2$ or 1 mol $	ext{h}_2	ext{o}$b. 0.5 mol $	ext{o}_2$ or 0.75 mol $	ext{h}_2$c. 1.5 mol $	ext{sno}$ or 3.0 mol $	ext{sno}_2$d. 0.33 mol $	ext{fe}_2	ext{o}_3$ or 0.66 mol $	ext{feo}$2. would you expect one mole of solid sodium, $	ext{na}$, to have the same volume as one mole of liquid bromine, $	ext{br}_2$? explain.3. how does the concept of the mole help chemists?4. explain how a mole of hydrogen peroxide ($	ext{h}_2	ext{o}_2$) and a mole of hydrogen chloride ($	ext{hcl}$) are the same but different.5. if one mole of an unknown substance is 200.59 g/mol, what is the mass of 0.33 mol of the substance?6. if you had one mole of avocados, then how many avocados would you have?7. a chemist has $3.45 	imes 10^{22}$ molecules of $	ext{p}_2	ext{o}_5$. how many grams of $	ext{p}_2	ext{o}_5$ does the chemist have?8. calculate the number of moles of each substance.a. $5.45 	imes 10^{26}$ molecules of methane, $	ext{ch}_4$b. $3.22 	imes 10^{23}$ atoms of xenon, $	ext{xe}$c. $9.6 	imes 10^{23}$ formula units of sodium chloride, $	ext{nacl}$9. how many moles of hydrogen atoms are in 7.10 mol of $	ext{h}_2	ext{o}$?10. how many moles of oxygen atoms are in 3.60 mol of $	ext{sio}_2$?11. what is the molar mass of molecular oxygen, $	ext{o}_2$?12. what is the molar mass of barium chloride, $	ext{bacl}_2$?13. what is the molar mass of $	ext{caco}_3$?14. what is the molar mass of $	ext{sf}_6$?15. calculate the number of moles of each substance.a. 6.00 g oxygen, $	ext{o}_2$b. 450.0 g of iron(iii) oxide, $	ext{fe}_2	ext{o}_3$c. 45.5 g of calcium chloride, $	ext{cacl}_2$

Accepted Answer

### Question 1
# Explanation:
## Step1: Compare mole counts (equal moles)
1 mol of any substance has $6.022 	imes 10^{23}$ particles. For a: 1 mol $	ext{OCl}_2$ and 1 mol $	ext{H}_2	ext{O}$ have equal particles.
## Step2: Compare mole counts (higher mole)
For b: $0.75 > 0.5$, so 0.75 mol $	ext{H}_2$ has more particles.
## Step3: Compare mole counts (higher mole)
For c: $3.0 > 1.5$, so 3.0 mol $	ext{SnO}_2$ has more particles.
## Step4: Calculate total particles per compound
For d: 0.33 mol $	ext{Fe}_2	ext{O}_3$ has $0.33 	imes 5 = 1.65$ mol of particles; 0.66 mol $	ext{FeO}$ has $0.66 	imes 2 = 1.32$ mol of particles.
# Answer:
a. They have the same number of representative particles
b. 0.75 mol $	ext{H}_2$
c. 3.0 mol $	ext{SnO}_2$
d. 0.33 mol $	ext{Fe}_2	ext{O}_3$

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### Question 2
# Brief Explanations:
No, they would not have the same volume. Solids have much closer, tightly packed particles than liquids, and sodium (a solid) has a much higher density than liquid bromine. Molar volume depends on state of matter and density, so 1 mol of solid Na will have a far smaller volume than 1 mol of liquid $	ext{Br}_2$.
# Answer:
No, they would not have the same volume.

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### Question 3
# Brief Explanations:
The mole provides a standardized, measurable unit to convert between the microscopic (atoms/molecules) and macroscopic (mass/volume) scales. It lets chemists count large numbers of tiny particles using measurable mass values, making stoichiometry and chemical calculations feasible.
# Answer:
It links microscopic particles to macroscopic measurable quantities, enabling chemical calculations.

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### Question 4
# Brief Explanations:
They are the same because 1 mole of any substance contains exactly $6.022 	imes 10^{23}$ representative particles (molecules, in this case). They are different because $	ext{H}_2	ext{O}_2$ and $	ext{HCl}$ are distinct compounds with different molar masses, different chemical properties, and different numbers of atoms per molecule.
# Answer:
Same: 1 mole of each has $6.022 	imes 10^{23}$ molecules. Different: They are distinct compounds with different molar masses and atomic compositions.

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### Question 5
# Explanation:
## Step1: Use mass-mole formula
Mass = moles $	imes$ molar mass
## Step2: Substitute values
$	ext{Mass} = 0.33\ 	ext{mol} 	imes 200.59\ 	ext{g/mol}$
# Answer:
$66.19\ 	ext{g}$

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### Question 6
# Brief Explanations:
By definition, 1 mole of any substance is equal to Avogadro's number of that substance.
# Answer:
$6.022 	imes 10^{23}$ avocados

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### Question 7
# Explanation:
## Step1: Convert molecules to moles
Moles = $\frac{	ext{number of molecules}}{6.022 	imes 10^{23}\ 	ext{molecules/mol}}$
$	ext{Moles of } 	ext{P}_2	ext{O}_5 = \frac{3.45 	imes 10^{22}}{6.022 	imes 10^{23}} = 0.0573\ 	ext{mol}$
## Step2: Calculate molar mass of $	ext{P}_2	ext{O}_5$
$	ext{Molar mass} = (2 	imes 30.97) + (5 	imes 16.00) = 61.94 + 80.00 = 141.94\ 	ext{g/mol}$
## Step3: Convert moles to mass
$	ext{Mass} = 0.0573\ 	ext{mol} 	imes 141.94\ 	ext{g/mol}$
# Answer:
$8.13\ 	ext{g}$

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### Question 8
# Explanation:
## Step1: Moles of $	ext{CH}_4$
Moles = $\frac{	ext{number of molecules}}{6.022 	imes 10^{23}}$
$	ext{Moles} = \frac{5.45 	imes 10^{26}}{6.022 	imes 10^{23}} = 905\ 	ext{mol}$
## Step2: Moles of Xe
Moles = $\frac{	ext{number of atoms}}{6.022 	imes 10^{23}}$
$	ext{Moles} = \frac{3.22 	imes 10^{23}}{6.022 	imes 10^{23}} = 0.535\ 	ext{mol}$
## Step3: Moles of NaCl
Moles = $\frac{	ext{number of formula units}}{6.022 	imes 10^{23}}$
$	ext{Moles} = \frac{9.6 	imes 10^{23}}{6.022 	imes 10^{23}} = 1.59\ 	ext{mol}$
# Answer:
a. $905\ 	ext{mol}$
b. $0.535\ 	ext{mol}$
c. $1.59\ 	ext{mol}$

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### Question 9
# Explanation:
## Step1: Find H atoms per $	ext{H}_2	ext{O}$ molecule
Each $	ext{H}_2	ext{O}$ has 2 H atoms.
## Step2: Calculate moles of H
$	ext{Moles of H} = 7.10\ 	ext{mol } 	ext{H}_2	ext{O} 	imes 2$
# Answer:
$14.2\ 	ext{mol}$

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### Question 10
# Explanation:
## Step1: Find O atoms per $	ext{SiO}_2$ molecule
Each $	ext{SiO}_2$ has 2 O atoms.
## Step2: Calculate moles of O
$	ext{Moles of O} = 3.60\ 	ext{mol } 	ext{SiO}_2 	imes 2$
# Answer:
$7.20\ 	ext{mol}$

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### Question 11
# Explanation:
## Step1: Calculate molar mass of $	ext{O}_2$
Molar mass = $2 	imes 16.00\ 	ext{g/mol}$
# Answer:
$32.00\ 	ext{g/mol}$

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### Question 12
# Explanation:
## Step1: Calculate molar mass of $	ext{BaCl}_2$
Molar mass = $137.33 + (2 	imes 35.45)$
# Answer:
$208.23\ 	ext{g/mol}$

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### Question 13
# Explanation:
## Step1: Calculate molar mass of $	ext{CaCO}_3$
Molar mass = $40.08 + 12.01 + (3 	imes 16.00)$
# Answer:
$100.09\ 	ext{g/mol}$

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### Question 14
# Explanation:
## Step1: Calculate molar mass of $	ext{SF}_6$
Molar mass = $32.07 + (6 	imes 19.00)$
# Answer:
$146.07\ 	ext{g/mol}$

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### Question 15
# Explanation:
## Step1: Moles of $	ext{O}_2$
Moles = $\frac{	ext{mass}}{	ext{molar mass}} = \frac{6.00\ 	ext{g}}{32.00\ 	ext{g/mol}}$
## Step2: Moles of $	ext{Fe}_2	ext{O}_3$
Molar mass of $	ext{Fe}_2	ext{O}_3 = (2 	imes 55.85) + (3 	imes 16.00) = 159.70\ 	ext{g/mol}$
Moles = $\frac{450.0\ 	ext{g}}{159.70\ 	ext{g/mol}}$
## Step3: Moles of $	ext{CaCl}_2$
Molar mass of $	ext{CaCl}_2 = 40.08 + (2 	imes 35.45) = 110.98\ 	ext{g/mol}$
Moles = $\frac{45.5\ 	ext{g}}{110.98\ 	ext{g/mol}}$
# Answer:
a. $0.188\ 	ext{mol}$
b. $2.82\ 	ext{mol}$
c. $0.410\ 	ext{mol}$

Sovi.AI - AI Math Tutor

QUESTION IMAGE

Question

Explanation:

Question 1

Step1: Compare mole counts (equal moles)

Step2: Compare mole counts (higher mole)

Step3: Compare mole counts (higher mole)

Step4: Calculate total particles per compound

Answer:

Question 2