Balance the following equations. (b) Au + H 2 SeO 4 → Au 2 (SeO 4 ) 3 + H 2 SeO 3 + H 2 O

Hey everyone. We're asked to balance the given chemical reaction first. Let's go ahead and count the number of atoms we have on both sides. Starting off with our react inside. We have one of nickel, one of hydrogen, one of nitrogen And three of oxygen. Looking at our product side, we have one of nickel as well, two of hydrogen, three of nitrogen and nine of oxygen only. Our nickel is balanced out. Let's first start off by balancing out our hydrogen. So if we add a coefficient of two prior to our nitric acid, we then are able to change our hydrogen into two, our nitrogen into two as well, And our oxygen's into six. Since we still need to change our nitrogen and oxygen's, this means we have to change The coefficient that we just inputted, which is R two. So instead of two, we can then go ahead and input a four prior to our nitric acid. And when we do that, we change our hydrogen into four, Our nitrogen into four as well. And our oxygen's into 12. Now that we've done this, we can adjust accordingly and look at our product side, we can add a coefficient of two prior to our water. And when we do this, we end up with four of hydrogen and our oxygen's changed from 9 to 10. Lastly, all we need to do is fix our nitrogen and our oxygen's and we can do that by fixing our nitrogen dioxide. So when we add a two prior to nitrogen dioxide, We end up with four of nitrogen And 12 of oxygen. So our balanced chemical reaction is going to be as such. So I hope this made sense and let us know if you have any questions.

Ch.3 - Mass Relationships in Chemical Reactions

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McMurry 8th Edition

Ch.3 - Mass Relationships in Chemical Reactions

Problem 42b

Chapter 3, Problem 42b

Balance the following equations. (b) Au + H₂SeO₄ → Au₂(SeO₄)₃ + H₂SeO₃ + H₂O

Verified step by step guidance

Identify the elements involved in the reaction: Au, H, Se, and O.

Write down the unbalanced equation: Au + H_2SeO_4 → Au_2(SeO_4)_3 + H_2SeO_3 + H_2O.

Count the number of atoms of each element on both sides of the equation.

Start by balancing the element that appears in the fewest compounds, which is Au. Balance Au by ensuring the number of Au atoms is the same on both sides.

Next, balance the Se atoms by adjusting the coefficients of H_2SeO_4 and H_2SeO_3. Finally, balance the H and O atoms by adjusting the coefficients of H_2O.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms of each element is the same on both sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. To balance an equation, coefficients are adjusted in front of the chemical formulas to achieve equal atom counts.

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It allows chemists to predict the amounts of substances consumed and produced in a reaction based on balanced equations. Understanding stoichiometry is essential for calculating yields, determining limiting reactants, and performing conversions between moles and grams.

Polyatomic Ions

Polyatomic ions are charged entities composed of two or more atoms covalently bonded together, which function as a single ion in chemical reactions. In the given equation, sulfate (SO₄²⁻) and hydrogen selenite (H₂SeO₃) are examples of polyatomic ions. Recognizing these ions is crucial for correctly writing and balancing chemical equations involving compounds that contain them.