Question

For the chemical reaction

2AgNO3+Na2CrO4⟶Ag2CrO4+2NaNO3

what mass of silver chromate is produced from 4.85 mol of silver nitrate?

Answer 1

806.3g

Step-by-step explanation:

Given parameters:

Number of moles of silver nitrate = 4.85mol

Unknown:

Mass of silver chromate = ?

Solution:

2AgNO₃ + Na₂CrO₄ → Ag₂CrO₄ + 2NaNO₃

To solve this problem, we work from the known to the unknown;

• The known specie here is AgNO₃ ;

From the balanced chemical equation;

2 moles of AgNO₃ will produce 1 mole of Ag₂CrO₄

4.85 moles of AgNO₃ will produce
`(4.85)/(2)` = 2.43moles of Ag₂CrO₄

• Mass of silver chromate produced;

mass = number of moles x molar mass

Molar mass of Ag₂CrO₄

Atomic mass of Ag = 107.9g/mol

Cr = 52g/mol

O = 16g/mol

Input the parameters and solve;

Molar mass = 2(107.9) + 52 + 4(16) = 331.8g/mol

So,

Mass of Ag₂CrO₄ = 2.43 x 331.8 = 806.3g