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Chapter 1: Problem 16

Select the correct alternative from the given choices. The number of oxygen atoms present in 2 moles of a compound, which consists of a bivalent metal and a perchlorate ion is (a) \(4 \mathrm{~N}\) (b) \(6 \mathrm{~N}\) (c) \(8 \mathrm{~N}\) (d) \(16 \mathrm{~N}\)

Short Answer

Expert verified
Answer: There are \(16 \mathrm{~N}\) oxygen atoms in 2 moles of the compound, where N is Avogadro's number.

Step by step solution

01

Identify the chemical formula for the compound

The compound consists of a bivalent metal (M) and a perchlorate ion (ClO_4^-). Since the metal is bivalent, it will bind with 2 perchlorate ions to form a neutral compound, so the chemical formula for the compound will be M(ClO_4)_2.
02

Calculate the number of oxygen atoms per formula unit

The perchlorate ions each have 4 oxygen atoms, so in M(ClO_4)_2, we would have 2 * 4 = 8 oxygen atoms.
03

Calculate the number of oxygen atoms in 1 mole of the compound

Since there are 8 oxygen atoms per formula unit, and 1 mole of the compound contains Avogadro's number (N) of formula units, there will be 8 * N oxygen atoms in 1 mole of the compound.
04

Calculate the number of oxygen atoms in 2 moles of the compound

Now, we need to find the number of oxygen atoms in 2 moles of the compound. Since there are 8 * N oxygen atoms in 1 mole, there will be 2 * 8 * N = 16 * N oxygen atoms in 2 moles of the compound. So, the correct alternative is (d) \(16 \mathrm{~N}\).

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Most popular questions from this chapter

The number of oxygen atoms present in 2 moles of a compound, which consists of a bivalent metal and a perchlorate ion is (a) \(4 \mathrm{~N}\) (b) \(6 \mathrm{~N}\) (c) \(8 \mathrm{~N}\) (d) \(16 \mathrm{~N}\)

Which of the following is in the correct order according to metal reactivity series? (a) \(\mathrm{Al}<\mathrm{Fe}<\mathrm{Na}<\mathrm{Ca}\) (b) \(\mathrm{Fe}<\mathrm{Ca}<\mathrm{Al}<\mathrm{Na}\) (c) \(\mathrm{Fe}<\mathrm{Al}<\mathrm{Ca}<\mathrm{Na}\) (d) \(\mathrm{Na}<\mathrm{Ca}<\mathrm{Al}<\mathrm{Fe}\)

Dalton's law of partial pressures cannot hold good for (a) \(\mathrm{NO}_{2}+\mathrm{O}_{2}\) (b) \(\mathrm{H}_{2}+\mathrm{Cl}_{2}\) (c) \(\mathrm{CO}_{2}+\mathrm{O}_{2}\) (d) \(\mathrm{NH}_{3}+\mathrm{He}\)

Plumbous ion is represented as (a) \(\mathrm{Pb}^{+2}\) (b) \(\mathrm{Pb}^{+4}\) (c) \(\mathrm{Pb}^{+3}\) (d) \(\mathrm{Pb}^{+1}\)

A \(600 \mathrm{ml}\) vessel containing oxygen at \(800 \mathrm{~mm}\) and a \(400 \mathrm{ml}\) vessel containing nitrogen at \(600 \mathrm{~mm}\) at the same temperature are joined to each other. The final pressure of the mixture is (a) \(1400 \mathrm{~mm}\) (b) \(1000 \mathrm{~mm}\) (c) \(720 \mathrm{~mm}\) (d) \(700 \mathrm{~mm}\)
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