Question

question 11 of 14 > a zinc ring is composed of 2.59×10²³ atoms. calculate the mass of the ring in grams. mass:

Explanation:

Step1: Recall Avogadro's number

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

Step2: Calculate the number of moles of zinc

The number of moles $n$ of zinc is given by $n=\frac{N}{N_A}$, where $N = 2.59\times 10^{23}$ atoms. So $n=\frac{2.59\times 10^{23}}{6.022\times 10^{23}\text{ atoms/mol}}\approx0.430\text{ mol}$.

Step3: Recall the molar - mass of zinc

The molar - mass of zinc $M$ is $M = 65.38\text{ g/mol}$.

Step4: Calculate the mass of zinc

The mass $m$ of zinc is calculated using the formula $m = n\times M$. So $m=0.430\text{ mol}\times65.38\text{ g/mol}\approx28.1\text{ g}$.

Answer:

$28.1$ g