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Chapter 1: Problem 34

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: \(16 \mathrm{~N}\) (16 times the Avogadro's number)

Step by step solution

01

Determine the molecular formula of the compound

The perchlorate ion has the formula ClO4-. Since we have a bivalent metal, it means the charge of the metal is +2. Let's represent this metal by symbol M. Thus, we can write the molecular formula of the compound as M(ClO4)2.
02

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

In the molecular formula M(ClO4)2, we have 2 perchlorate ions, each containing 4 oxygen atoms. Therefore, in one mole of the compound, there will be 2 * 4 = 8 moles of oxygen atoms.
03

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 moles of oxygen atoms in 1 mole of the compound, there will be 2 * 8 = 16 moles of oxygen atoms in 2 moles of the compound. Here, N represents Avogadro's number, which is the number of entities (atoms, molecules, ions, etc.) in one mole. Hence, the number of oxygen atoms in 2 moles of the compound is equal to 16 ℕ. The correct option is: (d) \(16 \mathrm{~N}\)

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Most popular questions from this chapter

Fill in the blanks. The number of oxygen molecules required for the complete combustion of 5 moles of methane is

In a \(2.5 \ell\) flask at \(27^{\circ} \mathrm{C}\) temperature, the pressure of a gas was found to be 8 atm. If \(2.41 \times 10^{23}\) molecules of the same gas are introduced into the container, the temperature changed to \(\mathrm{T}_{2}\). The pressure of gas is found to be \(10 \mathrm{~atm}\). Find out the value of \(\mathrm{T}_{2}\) (a) \(253 \mathrm{~K}\) (b) \(347 \mathrm{~K}\) (c) \(230 \mathrm{~K}\) (d) \(370 \mathrm{~K}\)

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\(\mathrm{KMnO}_{4}+\mathrm{H}_{2} \mathrm{SO}_{4}+\mathrm{FeSO}_{4} \rightarrow \mathrm{K}_{2} \mathrm{SO}_{4}+\mathrm{MnSO}_{4}+\) \(\mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}+\mathrm{H}_{2} \mathrm{O}\) Coefficients of sulphuric acid and ferric sulphate in the balanced equation of above reaction are respectively (a) 8,4 (b) 5,8 (c) 4,3 (d) 8,5

Select the correct alternative from the given choices. When one mole each of \(\mathrm{CO}\) and \(\mathrm{O}_{2}\) are made to react at STP, the total number of moles at the end of the reaction is (a) \(1.5\) moles (b) 1 mole (c) 4 moles (d) 2 moles
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