In the reaction
2HNO3(aq) + Cu(s) + 2H+(aq) �¨ 2NO2(g) + Cu2+(g) + 2H2O(l)
Which of the following statements is correct?
A.HNO3 is the reducing agent, and Cu is the oxidizing agent
B.HNO3 is the reducing agent, and H+ is the oxidizing agent
C.Cu is the reducing agent, and H+ is the oxidizing agent
D.Cu is the reducing agent, and HNO3 is the oxidizing agent
E.H+ is the reducing agent, and Cu is the oxidizing agent
Here is how you can answer.
Oxidation is the loss of electrons. Reduction is the gain of electrons.
The oxidizing agent is reduced; the reducing agent is oxidized.
Look at N in HNO3 and Cu to see which is which. I'll be glad to check your answers.
Well, let's break it down. In a redox (reduction-oxidation) reaction, electrons are transferred between species. The species that loses electrons is the reducing agent, while the species that gains electrons is the oxidizing agent.
Looking at the reaction, we see that Cu is going from a solid state to a copper(II) ion (Cu2+), gaining two electrons in the process. So, Cu is being oxidized, making it the oxidizing agent.
On the other hand, HNO3 is being reduced, as it is losing oxygen and gaining nitrogen dioxide (NO2), meaning it is the reducing agent.
Therefore, the correct answer is A. HNO3 is the reducing agent, and Cu is the oxidizing agent. Keep those electrons moving!
To determine the correct statement, we need to analyze the oxidation states of each element in the reaction.
The oxidation state of Cu in Cu(s) is 0, and in Cu2+(g) is +2, indicating that Cu has been oxidized (its oxidation state has increased).
The oxidation state of hydrogen in HNO3(aq) is +1, and in H2O(l) it is also +1, indicating that hydrogen is not oxidized or reduced.
The oxidation state of nitrogen in HNO3(aq) is +5, and in NO2(g) it is +4, indicating that nitrogen has been reduced (its oxidation state has decreased).
Based on this information, we can conclude that:
A. HNO3 is the reducing agent (because it causes another element, nitrogen, to be reduced)
C. Cu is the reducing agent (because it causes another element, hydrogen, to be oxidized)
Therefore, the correct statement is C. Cu is the reducing agent, and H+ is the oxidizing agent.
To determine the correct statement, we need to understand the concepts of reducing agents and oxidizing agents in a redox reaction.
In a redox reaction, one species loses electrons (is oxidized) while another species gains electrons (is reduced). The species that loses electrons is the reducing agent, while the species that gains electrons is the oxidizing agent.
Looking at the given reaction:
2HNO3(aq) + Cu(s) + 2H+(aq) → 2NO2(g) + Cu2+(g) + 2H2O(l)
We can see that Cu(s) is being oxidized since it goes from being in its metallic form (Cu(s)) to being in its ionic form (Cu2+(g)). This means that Cu is the reducing agent.
On the other hand, the H+ ions (from the HNO3(aq) and 2H+(aq)) are involved in the reduction as they are gaining electrons to form water (2H2O(l)). This means that H+ is the oxidizing agent.
Therefore, from the given options, the correct statement is:
C. Cu is the reducing agent, and H+ is the oxidizing agent.