Question

Total number of electrons in 2.0 grams of d2o to that of in 1.8 grams of H2O

Answer 1

hey mate here is your answer.

Hope it helps you.

Answer 2

Answer: $\frac{6.023\times 10^{23}}{6.023\times 10^{23}}$

Explanation: To calculate the moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\textMolar mass}}$

$\text{Number of moles of}D_2O=\frac{2g}{20g}=0.1moles$

$\text{Number of moles of}H_2O=\frac{1.8g}{18g}=0.1moles$

According to avogadro's law, 1 mole of every substance occupies 22.4 Liters at STP and contains avogadro's number $6.023\times 10^{23}$ of particles.

$D_2O$ contains 2+8= 10 electrons

Now 1 mole of $D_2O$ contains = $10\times 6.023\times 10^{23}=60.23\times 10^{23}$ electrons

0.1 mole of $D_2O$ molecule contains = $\frac{60.23\times 10^{23}}{1}\times 0.1=6.023\times 10^{23}$ electrons

$H_2O$ contains 2+8= 10 electrons

Now 1 mole of $H_2O$ contains = $10\times 6.023\times 10^{23}=60.23\times 10^{23}$ electrons

0.1 mole of $H_2O$ molecule contains = $\frac{60.23\times 10^{23}}{1}\times 0.1=6.023\times 10^{23}$ electrons