What mass of calcium chromate is formed when 35 grams of calcium nitrate reacts with sodium carbonate?

Question

Natalie Anton · Accepted Answer

This reaction cannot produce calcium chromate.

This reaction cannot occur. In order for one of the products to be calcium chromate, one of the reactants would have to contain the chromate ion, #"CrO"^(2-)"#. Sodium nitrate and calcium carbonate are the actual products of the chemical reaction between calcium nitrate and sodium carbonate. #"Ca(NO"_3)_2" + Na"_2"CO"_3"##rarr##"2NaNO"_3" + CaCO"_3"#

Owen Ambrose · Answer

undefined To find the mass of calcium chromate formed, first, determine the balanced chemical equation for the reaction between calcium nitrate and sodium carbonate. Then, calculate the molar mass of calcium chromate. Finally, use stoichiometry to find the mass of calcium chromate formed.

The balanced chemical equation for the reaction is:

3Ca(NO3)2 + Na2CO3 → CaCrO4 + 3NaNO3 + 2NaNO2

The molar mass of calcium chromate (CaCrO4) is approximately 156.07 g/mol.

Using stoichiometry, we find that for every 3 moles of calcium nitrate reacting, 1 mole of calcium chromate is formed.

First, calculate the number of moles of calcium nitrate:

$ \text{Moles of Ca(NO}_3\text{)}_2 = \frac{\text{Mass}}{\text{Molar mass}} $

$ \text{Moles of Ca(NO}_3\text{)}_2 = \frac{35 \text{ g}}{164.09 \text{ g/mol}} $

Then, use the mole ratio from the balanced equation to find the moles of calcium chromate:

$ \text{Moles of CaCrO}_4 = \frac{\text{Moles of Ca(NO}_3\text{)}_2}{3} $

Finally, calculate the mass of calcium chromate:

$ \text{Mass of CaCrO}_4 = \text{Moles of CaCrO}_4 \times \text{Molar mass of CaCrO}_4 $

Perform the calculations to find the mass of calcium chromate formed.

Cameron Andrews · Answer

undefined The mass of calcium chromate formed when 35 grams of calcium nitrate reacts with sodium carbonate is approximately 29.2 grams.