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Chapter 8: Problem 31

Total number of electrons present in \(4.4 \mathrm{~g}\) oxalate ion \(\left(\mathrm{C}_{2} \mathrm{O}_{4}^{2}\right)\) is (a) \(0.05 N_{\mathrm{A}}\) (b) \(2.3 N_{A}\) (c) \(2.2 N_{\Lambda}\) (d) \(2.1 N_{A}\)

Short Answer

Expert verified
Answer: The total number of electrons in 4.4 g of the oxalate ion is 4.4N_A, where N_A is Avogadro's number. None of the provided options match the correct answer.

Step by step solution

01

Find the number of moles of oxalate ions

First, we need to find the molar mass of the oxalate ion. The molar mass of each element is as follows: C: 12.01 g/mol O: 16.00 g/mol The oxalate ion has 2 carbon atoms and 4 oxygen atoms. So, the molar mass of oxalate ion is: \(2\times 12.01+(4\times 16.00)=44.02 g/mol\) Now, we can find the number of moles of oxalate ions in 4.4g by dividing the mass with the molar mass: = / number of moles = \(\frac{4.4}{44.02} \approx 0.1\)
02

Find the total number of electrons in the oxalate ion

Each atom in the oxalate ion contributes electrons. - Carbon (C) has 6 electrons - Oxygen (O) has 8 electrons The total number of electrons in the oxalate ion: \(2 \times 6 + 4 \times 8 = 44\) electrons
03

Calculate the total number of electrons in 4.4 g of oxalate ions

Now, we have the number of moles of oxalate ions (0.1) and the total number of electrons in each oxalate ion (44). To find the total number of electrons in 4.4g, we need to multiply these two values by Avogadro's number (_N_A_). Total number of electrons = (number of moles) × (total number of electrons in each ion) × _N_A_ Total number of electrons = \(0.1 \times 44 \times N_{A} = 4.4 N_{A}\)
04

Match the final answer with the given choices

By comparing our result with the given choices, we can see that none of the provided options match the correct answer, which is \(4.4 N_{A}\).

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Most popular questions from this chapter

A given mixture consists only of pure substance \(\mathrm{X}\) and pure substance \(\mathrm{Y}\). The total mass of the mixture is \(3.72 \mathrm{~g}\). The total number of moles is \(0.06\). If the mass of one mole of \(Y\) is \(48 \mathrm{~g}\) and there is \(0.02\) mole of \(\mathrm{X}\) in the mixture, what is the mass of one mole of \(\mathrm{X}\) ? (a) \(90 \mathrm{~g}\) (b) \(75 \mathrm{~g}\) (c) \(45 \mathrm{~g}\) (d) \(180 \mathrm{~g}\)

A volume \(V\) of a gaseous hydrocarbon was exploded with an excess of oxygen. The observed contraction was \(2.5 \mathrm{~V}\), and on treatment with potash, there was a further contraction of \(2 V\). What is the molecular formula of the hydrocarbon? (a) \(\mathrm{C}_{2} \mathrm{H}_{6}\) (b) \(\mathrm{C}_{3} \mathrm{H}_{6}\) (c) \(\mathrm{C}_{4} \mathrm{H}_{12}\) (d) \(\mathrm{C}_{2} \mathrm{H}_{4}\)

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A volume of \(1 \mathrm{ml}\) of a gaseous aliphatic compound \(\mathrm{C}_{n} \mathrm{H}_{3 n} \mathrm{O}_{m}\) is completely burnt in an excess of oxygen. The contraction in volume (in \(\mathrm{ml}\) ) is

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