mole practice
1. you have exactly 6.022 * 10^{24} atoms of iron on your balance. how many moles do you have?
2. you have exactly 100.00 grams of nickel. how many moles do you have?
3. determine the mass in grams of 5.00 moles of he.
4. how many atoms are present in 23.0 moles of ti?
5. how many grams in 1.000 moles of oxygen gas? (hint: not 16.00 g)
6. how many grams in 1.575 moles of fluorine gas?
7. determine the number of atoms of gold in 15.000 grams au.
8. after a very long chemistry assignment, you rubbed off 0.015 grams of carbon from your pencil. how many atoms of carbon have been left on your paper?
9. what is the average mass of an atom of sulfur?

Question

Accepted Answer

# Explanation:
## Step1: Use the formula $n=\frac{N}{N_{A}}$
Given $N = 6.022\times10^{24}$ atoms and $N_{A}=6.022\times10^{23}\text{ atoms/mol}$, then $n=\frac{6.022\times 10^{24}}{6.022\times 10^{23}}$
## Step2: Simplify the expression
$n = 10\space mol$

# Answer:
$10\space mol$

# Explanation:
## Step1: Find the molar mass of nickel
The molar mass of $Ni$, $M = 58.69\space g/mol$
## Step2: Use the formula $n=\frac{m}{M}$
Given $m = 100.00\space g$, then $n=\frac{100.00}{58.69}$
## Step3: Calculate the value
$n\approx1.704\space mol$

# Answer:
$\approx1.704\space mol$

# Explanation:
## Step1: Find the molar mass of $He$
The molar mass of $He$, $M = 4.00\space g/mol$
## Step2: Use the formula $m=n\times M$
Given $n = 5.00\space mol$, then $m=5.00\times4.00$
## Step3: Calculate the value
$m = 20.0\space g$

# Answer:
$20.0\space g$

# Explanation:
## Step1: Use the formula $N=n\times N_{A}$
Given $n = 23.0\space mol$ and $N_{A}=6.022\times10^{23}\text{ atoms/mol}$, then $N=23.0\times6.022\times 10^{23}$
## Step2: Calculate the value
$N = 1.38506\times10^{25}\text{ atoms}$

# Answer:
$1.38506\times10^{25}\text{ atoms}$

# Explanation:
## Step1: Determine the formula of oxygen gas
Oxygen gas is $O_{2}$, and its molar mass $M=(16.00\times2)\space g/mol = 32.00\space g/mol$
## Step2: Use the formula $m=n\times M$
Given $n = 1.000\space mol$, then $m=1.000\times32.00$
## Step3: Calculate the value
$m = 32.00\space g$

# Answer:
$32.00\space g$

# Explanation:
## Step1: Determine the formula of fluorine gas
Fluorine gas is $F_{2}$, and its molar mass $M=(19.00\times2)\space g/mol=38.00\space g/mol$
## Step2: Use the formula $m=n\times M$
Given $n = 1.575\space mol$, then $m=1.575\times38.00$
## Step3: Calculate the value
$m = 59.85\space g$

# Answer:
$59.85\space g$

# Explanation:
## Step1: Find the molar mass of gold
The molar mass of $Au$, $M = 196.97\space g/mol$
## Step2: Use the formula $n=\frac{m}{M}$
Given $m = 15.000\space g$, then $n=\frac{15.000}{196.97}$
## Step3: Use the formula $N=n\times N_{A}$
$N=\frac{15.000}{196.97}\times6.022\times 10^{23}$
## Step4: Calculate the value
$N\approx4.59\times10^{22}\text{ atoms}$

# Answer:
$\approx4.59\times10^{22}\text{ atoms}$

# Explanation:
## Step1: Find the molar mass of carbon
The molar mass of $C$, $M = 12.01\space g/mol$
## Step2: Use the formula $n=\frac{m}{M}$
Given $m = 0.015\space g$, then $n=\frac{0.015}{12.01}$
## Step3: Use the formula $N=n\times N_{A}$
$N=\frac{0.015}{12.01}\times6.022\times 10^{23}$
## Step4: Calculate the value
$N\approx7.52\times10^{20}\text{ atoms}$

# Answer:
$\approx7.52\times10^{20}\text{ atoms}$

# Explanation:
## Step1: Use the concept of molar mass and Avogadro's number
The molar mass of $S$ is $M = 32.07\space g/mol$, and $N_{A}=6.022\times10^{23}\text{ atoms/mol}$
## Step2: Use the formula $m_{atom}=\frac{M}{N_{A}}$
$m_{atom}=\frac{32.07}{6.022\times 10^{23}}$
## Step3: Calculate the value
$m_{atom}\approx5.325\times10^{-23}\space g$

# Answer:
$\approx5.325\times10^{-23}\space g$

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QUESTION IMAGE

Question

Explanation:

Step1: Use the formula \(n=\frac{N}{N_{A}}\)

Step2: Simplify the expression

Step1: Find the molar mass of nickel

Step2: Use the formula \(n=\frac{m}{M}\)

Step3: Calculate the value

Step1: Find the molar mass of \(He\)

Step2: Use the formula \(m=n\times M\)

Step3: Calculate the value

Step1: Use the formula \(N=n\times N_{A}\)

Step2: Calculate the value

Answer: