Balance the following equations. (a) CO(NH 2 ) 2 (aq) + HOCl(aq) --> NCl 3 (aq) + CO 2 (aq) + H 2 O(l)

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

McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook

All textbooks

McMurry 8th Edition

Ch.3 - Mass Relationships in Chemical Reactions

Problem 43a

Chapter 3, Problem 43a

Balance the following equations. (a) CO(NH₂)₂(aq) + HOCl(aq) --> NCl₃(aq) + CO₂(aq) + H₂O(l)

Verified step by step guidance

Identify the number of each type of atom on both sides of the equation. For the reactants: C = 1, O = 1, N = 2, H = 2, Cl = 1. For the products: C = 1, O = 2, N = 3, H = 2, Cl = 3.

Start by balancing the atoms that appear in the least number of compounds. In this case, balance the nitrogen atoms first. Since there are 2 nitrogen atoms in the reactants and 3 in the products, adjust the coefficients to balance the nitrogen.

Next, balance the chlorine atoms. There is 1 chlorine atom in the reactants and 3 in the products, so adjust the coefficient of HOCl to balance the chlorine.

Balance the oxygen atoms. There is 1 oxygen atom in the reactants and 2 in the products, so adjust the coefficients to ensure the oxygen atoms are balanced.

Finally, check the balance of hydrogen atoms. Adjust the coefficients if necessary to ensure that the number of hydrogen atoms is the same on both sides of the equation.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

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 for 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.

Types of Chemical Reactions

Understanding the types of chemical reactions, such as synthesis, decomposition, single replacement, and double replacement, is crucial for predicting products and balancing equations. In the given reaction, the interaction between urea (CO(NH2)2) and hypochlorous acid (HOCl) suggests a redox process, where oxidation states change, leading to the formation of nitrogen trichloride (NCl3), carbon dioxide (CO2), and water (H2O).

State Symbols in Chemical Reactions

State symbols indicate the physical state of the reactants and products in a chemical equation: (s) for solid, (l) for liquid, (g) for gas, and (aq) for aqueous solutions. These symbols provide important information about the conditions of the reaction and can influence the balancing process. In the given equation, recognizing the states helps in understanding the reaction environment and the nature of the products formed.