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irakobra [83]
3 years ago
10

If you have 3.48 x 1023 formula units of Lead (II) Permanganate, what is its mass?

Chemistry
1 answer:
Tanya [424]3 years ago
4 0

Answer:

\large \boxed{\text{257 g}}

Explanation:

We can convert the formula units to moles and then use the molar mass to find the mass.

1. Moles of Pb(MnO₄)₂

n = 3.48 \times 10^{23}\text{ formula units} \times \dfrac{\text{1 mol}}{6.022 \times 10^{23}\text{ formula units}} = \text{0.5779 mol}

 

2. Mass of Pb(MnO₄)₂

\text{Mass} = \text{0.5779 mol} \times \dfrac{\text{445.07 g}}{\text{1 mol u}} = \text{257 g}\\\\\text{The mass of lead(II) permanganate is $\large \boxed{\textbf{257 g}}$}

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<h3>Explanation</h3>

For each nucleus:

Mass number = Number of protons + Number of neutrons.

The atomic number of a nucleus is the same as its number of protons. The atomic number of the nucleus here is 31. There are 31 protons in each nucleus.

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Mass number = Number of protons + Number of neutrons.

80 = 31 + Number of neutrons.

Number of neutrons = 80 - 31 = 49.

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