Question

Calculate the number of formula units in 159g of PbCrO4

Answer 1

The molecular weight of pbcro4 is = 323.2n the given weight is = 159 g let's divide given at upon mol= 323.2n/159 = 0.49195545×10²8 Ans is 0.49195545×10²8.

Answer 2

Answer: The number of formula units in the given amount of lead chromate is $2.963\times 10^{23}$

Explanation:

Formula units is defined as lowest whole number ratio of ions in an ionic compound. It is calculate by multiplying the number of moles by Avogadro's number which is $6.022\times 10^{23}$

To calculate the number of moles, we use the equation:

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

Given mass of $PbCrO_4$ = 159 g

Molar mass of $PbCrO_4$ = 323.2 g/mol

Putting values in above equation, we get:

$\text{Moles of }PbCrO_4=\frac{159g}{323.2g/mol}=0.492mol$

So, the number of formula units = $0.492\times 6.022\times 10^{23}=2.963\times 10^{23}$

Hence, the number of formula units in the given amount of lead chromate is $2.963\times 10^{23}$