an iron atom has a mass of 9.27×10⁻²³ g and a cooking pot has a mass of 0.500 kg. use this information to…

Explanation:

Step1: Recall Avogadro's number

Avogadro's number $N_A = 6.022\times 10^{23}\text{ atoms/mol}$.

Step2: Calculate mass of 1 - mole of iron atoms

If one iron - atom has a mass $m = 9.27\times 10^{-23}\text{ g}$, then the mass of 1 mole of iron atoms $M$ is given by $M=m\times N_A$. [ \begin{align*} M&=(9.27\times 10^{-23}\text{ g/atom})\times(6.022\times 10^{23}\text{ atoms/mol})\ &=(9.27\times6.022)\text{ g/mol}\ & = 55.82394\text{ g/mol}\approx55.8\text{ g} \end{align*} ]

Step3: Convert mass of cooking pot to grams

The mass of the cooking pot $m_{pot}=0.500\text{ kg}=500\text{ g}$.

Step4: Calculate number of moles of iron atoms in the cooking - pot

The number of moles $n$ of iron atoms with mass equal to the mass of the cooking pot is $n=\frac{m_{pot}}{M}$. [ n=\frac{500\text{ g}}{55.8\text{ g/mol}}\approx8.96\text{ mol}\approx9.00\text{ mol} ]

Answer:

55.8 9.00