A sample of CaCO3 with a mass of 6.35 g is placed in 500.0 mL of 0.31 M HCl , forming CaCl2, H2

A sample of CaCO3 with a mass of 6.35 g is placed in 500.0...

A sample of $\mathrm{CaCO}_{3}$ with a mass of 6.35 $\mathrm{g}$ is placed in 500.0 $\mathrm{mL}$ of 0.31 $\mathrm{M} \mathrm{HCl}$ , forming $\mathrm{CaCl}_{2}, \mathrm{H}_{2} \mathrm{O}$ , and $\mathrm{CO}_{2}$ What mass in grams of $\mathrm{CO}_{2}$ is produced?

Key Concepts

Limiting Reactant

The limiting reactant is the substance in a chemical reaction that is entirely consumed first, thereby restricting the extent of the reaction and the maximum amount of product that can be formed. Identifying the limiting reactant is crucial for accurate yield calculations.

Stoichiometry

Stoichiometry involves using the relationships expressed in a balanced chemical equation to determine the quantities of reactants needed or products formed. This concept is essential in calculating how much product can be obtained from a given amount of reactant.

Balanced Chemical Equation

A balanced chemical equation is one where the number of atoms for each element is equal on both sides of the reaction. This balance ensures the conservation of mass and allows for the proper determination of mole ratios used in stoichiometric calculations.

Molar Mass

Molar mass is the mass of one mole of a substance, serving as a conversion factor from grams to moles. It is essential for linking the measurable mass of a substance to the number of moles, which is required in stoichiometry.

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is used to relate the volume of a solution to the quantity of substance dissolved, which is important in determining the amounts of reactants present in chemical reactions.

Transcript

00:01 We're told in words what happens to this reaction, which is written here as a chemical equation.

00:06 Notice that this is a limiting reactive problem because we're given information about both reactants.

00:12 What we'll do first is to use this information to find moles of each reactant.

00:19 So when we're given mass, we can divide by the molar mass of the substance.

00:24 This is the molar mass of calcium carbonate to help us find 0 .06634 ,000, we can divide by the molar mass of the substance.

00:31 Mole of calcium carbonate.

00:35 We're going to treat hydrochloricastis separately.

00:39 We're told in this case that we have volume and molarity.

00:45 Remember that molarity is mole per meter.

00:50 So we're going to change this into liters first by dividing by 1 ,000.

00:58 And if i multiply these two values together, i find that there are 0 .155 mole of hydrolygasms.

01:15 Here's the problem.

01:16 We can't compare most of the moles because we don't yet have a balanced chemical reaction.

01:20 So to balance chemical reaction, let's balance the calcium atoms first because they only show up one side.

01:29 Next, we'll take care of the carbons.

01:31 There's one carbon here...

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