Balancing Nitric Acid Reactions

The video tutorial explains the process of balancing a chemical equation involving copper and concentrated nitric acid. It highlights the challenges faced in balancing the equation and the steps taken to adjust coefficients to achieve balance. The instructor demonstrates the importance of balancing hydrogen, nitrogen, and oxygen atoms and provides a detailed walkthrough of the process, including common mistakes and solutions.

What is the main reactant added to nitric acid in this reaction?

• Aluminum metal

• Copper metal

• Zinc metal

• Iron metal

What type of nitric acid is used in the reaction?

• Dilute nitric acid

• Concentrated nitric acid

• Aqueous nitric acid

• Fuming nitric acid

What is the initial challenge faced when balancing the equation?

• Balancing the oxygen atoms

• Balancing the copper atoms

• Balancing the hydrogen atoms

• Balancing the nitrogen atoms

What was the first adjustment made to balance the equation?

• Doubling the copper

• Doubling the nitric acid

• Doubling the nitrogen dioxide

• Doubling the water

How many nitrogens are present after the initial adjustment?

• Five

• Four

• Two

• Three

What was the final step to balance the hydrogen atoms?

• Adding more water

• Adding more nitric acid

• Doubling the hydrogen coefficient

• Doubling the nitrogen dioxide

What was the total number of oxygen atoms after balancing?

• Fifteen

• Twelve

• Six

• Nine

What was the final realization about the hydrogen atoms?

• They were not part of the equation

• They were correctly balanced

• They were underbalanced

• They were overbalanced

What is the final product formed along with copper nitrate?

• Nitrogen monoxide

• Nitrous oxide

• Nitrogen dioxide

• Nitric oxide

What is the main takeaway from the balancing process?

• Balancing equations is easy

• Balancing requires trial and error

• Balancing is only for experts

• Balancing is unnecessary