An excess of sodium carbonate, Na, CO3, in solution is added to a solution containing 17.87 g CaCl2. After performing the experiment, 13.19 g of calcium carbonate, CaCO3, is produced. Calculate the percent yield of this reaction.

Approximately .

Explanation:

Balanced equation for this reaction:

.

Look up the relative atomic mass of elements in the limiting reactant, , as well as those in the product of interest, :

Calculate the formula mass for both the limiting reactant and the product of interest:

.

.

Calculate the quantity of the limiting reactant () available to this reaction:

.

Refer to the balanced equation for this reaction. The coefficients of the limiting reactant () and the product () are both . Thus:

.

In other words, for every of formula units that are consumed, of formula units would (in theory) be produced. Thus, calculate the theoretical yield of in this experiment:

.

Calculate the theoretical yield of this experiment in terms of the mass of expected to be produced:

.

Given that the actual yield in this question (in terms of the mass of ) is , calculate the percentage yield of this experiment:

.

warm front forms when a moist, warm air mass slides up and over a cold air mass. as the warm air mass rises, it condenses into a broad area of clouds. a warm front brings gentle rain or light snow, followed by warmer, milder weather.

hope i !