What is the mass of a sample containing 8.53×10 to the 24th power formula units of magnesium phosphate?

Chemistry

1 answer:

Archy [21]3 years ago

5 0

Answer:

Mass = 3732.62 g

Explanation:

Given data:

Number of formula units = 8.53×10²⁴

Mass of sample = ?

Solution:

1 mole of any substance contain 6.022×10²³ formula units.

8.53×10²⁴ formula units ×1 mol / 6.022×10²³ formula units

1.42×10¹ mol

14.2 mol

Mass of magnesium phosphate:

Mass = number of moles × molar mass

Mass = 14.2 mol × 262.86 g/mol

Mass = 3732.62 g

You might be interested in

When NH3(g) reacts with N2O(g) to form N2(g) and H2O(g), 105 kcal of energy are evolved for each mole of NH3(g) that reacts. Wri

Ganezh [65]

Answer : The balanced chemical equation is,

$2NH_3(g)+3N_2O(g)\rightarrow 4N_2(g)+3H_2O(g)+210kcal$

Explanation :

Balanced chemical equation : It is defined as the number of atoms of individual elements present on the reactant side must be equal to the number of atoms of individual elements present on product side.

The given unbalanced chemical reaction is,

$NH_3(g)+N_2O(g)\rightarrow N_2(g)+H_2O(g)+105kcal$

This chemical reaction is an unbalanced reaction because in this reaction, the number of atoms of individual elements are not balanced.

In order to balanced the chemical reaction, the coefficient 2 is put before the $NH_3$ , the coefficient 3 is put before the $N_2O\text{ and }H_2O$ and the coefficient 4 is put before the $N_2$ .