Balance the equation for the production of acetylene (C2 H2) from the reaction of calcium carbid

Balance the equation for the production of acetylene (C2 H2)...

Key Concepts

Chemical Equation Balancing

This concept involves ensuring that the number of atoms for each element is equal on both sides of a chemical reaction equation. It is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. By balancing equations, chemists determine the proper stoichiometric relationships between reactants and products.

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It uses the mole ratios derived from a balanced equation to calculate how much of each substance is needed or produced. This concept is essential for converting between masses of chemicals and the number of moles required for a reaction.

Molar Mass Conversion

Molar mass conversion involves using the molar mass (the mass of one mole of a substance) to convert between the mass of a substance and the amount in moles. This step is critical in stoichiometry, as it connects the measured quantities (in grams) to the number of entities (moles) that participate in the chemical reaction.

Combustion Reaction

A combustion reaction is a type of exothermic reaction in which a substance reacts rapidly with oxygen to form products such as carbon dioxide and water, releasing energy in the process. Understanding combustion is key when analyzing the energy output from burning compounds like acetylene.

Thermochemistry

Thermochemistry focuses on the heat changes that accompany chemical reactions and physical changes. It involves measuring or calculating the energy released or absorbed, often through the use of enthalpy changes. This concept is crucial when determining the total energy produced in a reaction, such as the combustion of acetylene in this context.

Transcript

00:01 So this problem has two parts, and for part a, we're supposed to find the equation for when acetylene is produced when we react calcium carbide and water.

00:11 So we know for sure, or two reactants are calcium carbide and water, and we know that one of the products is acetylene.

00:20 But we are missing a product, and the reason why we know that is because there's an oxygen here in the water, but there's no oxygen on the right side.

00:29 So we need to find out what that missing product is.

00:32 And the way we can do that is we can find how this reaction actually occurs.

00:35 So we know that in this case, when water splits up, we can express that as hoh.

00:43 And we know that the calcium carbide splits into calcium and the carbon.

00:48 And so for the settling here, we know that's formed when the calcium or when the carbon bonds with hydrogen.

00:57 So then logically, the last product has to be when the calcium bonds.

01:02 The hydroxide ion.

01:05 So we can just add that here, calcium hydroxide.

01:10 And the last thing that we need to do is we need to balance this equation.

01:13 So we look at the left side.

01:14 We look at calcium.

01:16 Calcium is balanced.

01:17 One mole of calcium on both sides.

01:20 We look at carbon.

01:21 Carbon is also balanced because we have two on each side.

01:26 Now we look at hydrogen.

01:27 Hydrogen is unbalanced because we only have two on the left side, but we have four on the right.

01:35 So we just added two to correct for that.

01:38 And that also fixes our oxygen problem because now we have two moles of oxygen atoms on both sides.

01:43 So for part a, the final reaction can be written as such.

02:01 That is the final answer.

02:04 Now for part b.

02:06 Part b now asks us for how much heat is released when some amount of acetylene is combust it, starting with 74 .6 grams of c2.

02:18 So the first thing that we need to do is we need to actually write the combustion reaction for acetylene.

02:22 So we know that for combustion reactions, for this one, we are starting with the setylene.

02:29 And then in combustion reactions we always have oxygen as a reactant, and we have liquid water, and carbon dioxide as the products.

02:39 So now we need to balance this.

02:42 We first look to the carbon.

02:44 There's two moles on the left side, only one mole on the right.

02:47 So we added two here to balance...

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