mole of 18.0 g/mol, and each water molecule (H2O) has 10 electrons. (a) How many

Question

mole of 18.0 g/mol, and each water molecule (H2O) has 10 electrons. (a) How many electrons are there in 1.27 liters of water? (1 liter is equivalent to 1.00 × 10-3 m3) (b) What is the net charge of all these electrons? mole of 18.0 g/mol, and each water molecule (H2O) has 10 electrons. (a) How many electrons are there in 1.27 liters of water? (1 liter is equivalent to 1.00 × 10-3 m3) (b) What is the net charge of all these electrons? mole of 18.0 g/mol, and each water molecule (H2O) has 10 electrons. (a) How many electrons are there in 1.27 liters of water? (1 liter is equivalent to 1.00 × 10-3 m3) (b) What is the net charge of all these electrons?

Explanation / Answer

a) First, we are given the number of electrons in each water molecule, but we don't know how
many water molecules we have. So let's figure that out:

One mole (of any substance) has 6.02 x 10^23 molecules (Avogadro's Number)
We have 70.56 moles of water (1270g water divided by 18 grams per mole= 70.56 moles).
So the total number of molecules of water is:
6.02 x 10^23 molecules/mole times 70.56 moles = 424.77 x 10^23 molecules

Now, since each of those molecules has 10 electrons, all we need do is multiply the
number of molecules of water times 10, giving us 4247.7 x 10^23 electrons

b) Charge on these electrons = Q=ne=4247.7 x 10^23*1.6*10^-19 = 6796.32 * 10^4

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