Complete and balance the equations for the following reactions: (a) K(s)+I2(g) →(c) Al(s)+S8(s)

Complete and balance the equations for the following...

Key Concepts

Conservation of Mass

This principle states that matter cannot be created or destroyed in a chemical reaction. It forms the basis for balancing chemical equations, ensuring that the total number of atoms of each element is the same in the reactants and products.

Balancing Chemical Equations

This concept involves adjusting the coefficients in a chemical equation so that the number of atoms for each element is equal on both sides of the reaction. It is essential for accurately representing chemical reactions in accordance with the conservation of mass.

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It is used to determine the precise ratios in which substances react and are produced, which is critical for balancing equations and scaling reactions.

Chemical Formulas

Chemical formulas use element symbols and numerical subscripts to represent the composition of compounds. Understanding how to construct and interpret these formulas is crucial for writing balanced equations that accurately reflect the substances involved in a reaction.

Reaction Types (Synthesis Reactions)

Synthesis reactions involve the combination of two or more simple substances to form a more complex compound. Recognizing this type of reaction helps in predicting the products and writing the correct chemical equations.

States of Matter Notation

Chemical equations often include symbols (s for solid, l for liquid, g for gas, aq for aqueous) to indicate the physical states of substances. This notation provides additional information about the conditions under which the reactions occur.

Transcript

00:01 So for this question, we're given four incomplete chemical reactions, and we're asked to complete and balance them.

00:10 So, that further ado, let's begin with the first one, a.

00:13 We have solid potassium and gaseous iodide, or iodine gas.

00:20 So in order to complete these, we need to know the various charges, standard charges of these respective elements, in order to effectively combine them and balance them.

00:33 So potassium will start out has a charge of plus one.

00:40 And iodide, or iodine gas collectively has a charge of zero.

00:45 However, iodine individually has a charge of negative one.

00:52 So we would only need one iodine in order to satisfy and balance out the charge for potassium.

01:00 So our product to this reaction should be potassium iodide.

01:10 But there would be two, because there's already two iodine atoms here.

01:15 So we write two.

01:17 But that means we have one more potassium on this side.

01:21 So that means we have to write two over here.

01:27 Actually, i'm going to write these charges in a different color, just so they can be more easily differentiated.

01:35 Collected like zero, but individually they're minus one.

01:38 And this is plus one.

01:39 Okay.

01:41 So 2ki.

01:44 Potetium iodide can usually exist as a solid.

01:47 I don't believe you need to write the state that this product is in, but i'm going to go ahead and read it anyway.

01:56 So it's solid because it usually comes in the form of white tablets.

02:00 So the second one, we have solid aluminum and solid sulfur.

02:06 There's eight of them.

02:09 So aluminum typically has a charge of plus three, while sulfur has a charge of minus two.

02:26 So we've got to do a little bit of math here.

02:29 Basically, we just have to multiply them in order for these charges to equal each other.

02:35 Our lowest common multiple is six, so we would multiply aluminum by two, and sulfur by 3.

02:49 So our base product is di -aluminum trisulfate, trisulfide, i believe it's trisulfide.

02:59 And we would have to count for these leftovers here...

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