Question

What mas of cu will contain 3.22×10^24 atoms of copper. Atomic mass if cu = 63.54 amu

Answer 1

Answer:

635.4

Explanation:

No. of atoms=3.22×10^24 = No. of moles of Cu × NA

(No. of moles,n= Given mass (x) /Molar mass

ie., n = x / 63.54)

3.22×10^24= x/63.54 × 6.022 ×10^23

mass of Cu ,x =635.4(approximately)

Answer 2

340 grams of Cu will contain $3.22\times 10^{24}$ atoms of copper.

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number $6.023\times 10^{23}$ of particles.

To calculate the moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given atoms}}{\text {avogadro's number}}=\frac{3.22\times 10^{24}}{6.023\times 10^{23}}=5.35moles$

1 mole of copper has mass = 63.54 amu

5.35 moles of copper has mass = $\frac{63.54}{1}\times 5.35=340g$ of copper

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