0
What else can I help you with?
Reaction of Cu and Ag plus to yield Cu plus 2 and Ag?
The reaction of copper and silver nitrate produces copper(II) nitrate and silver. This involves the displacement of copper by silver in the reaction. The balanced chemical equation for this reaction is: Cu + 2AgNO3 -> Cu(NO3)2 + 2Ag.
Choose all of the statements that are true about this single replacement reaction Al plus CuCl2?
One product will be AlCl3 Copper metal will be a product
What is the product of Cu plus O2?
Copper has 2 possible valence configurations: Cu+1 or Cu+2. In either case, the products would be Copper oxide but their chemical characteristics, and their formulas, would be different, due to the difference in valence.For Cu+1, the product would be a red powder, of the formula, Cu2O.For Cu+2, the product would be a black powder, of the formula, CuO
How do you balance the equation silver nitrate plus copper metal equals silver metal plus copper nitrate?
If the copper nitrate formed is copper (I) nitrate, the equation balances with one atom of each metal and one formula weight of each nitrate. If the copper nitrate formed is copper (II) nitrate, the balanced equation is: 2 AgNO3 + Cu -> 2 Ag + Cu(NO3)2.
What is the states of each compound in CuSO4 plus 2KOH -- Cu(OH)2 plus K2SO4?
In the reaction CuSO4 + 2KOH, copper sulfate reacts with potassium hydroxide to form copper(II) hydroxide (Cu(OH)2) and potassium sulfate (K2SO4). The state of each compound can be written as follows: CuSO4 (aq) + 2KOH (aq) → Cu(OH)2 (s) + K2SO4 (aq) Here, the reactants (CuSO4 and KOH) are in aqueous solution, while the products (Cu(OH)2 and K2SO4) are in solid and aqueous states, respectively.
Is Cu oxidized or reduced in CuO plus H2 yields Cu plus H2O?
Cu is oxidized. The oxidation number goes from 0 in Cu to +2 in CuSO4. S is reduced. The oxidation number goes from +6 in H2SO4 to +4 in SO2. The oxidizing agent is H2SO4 since it causes Cu to be oxidized. The reducing agent is Cu since it causes S in H2SO4 to be reduced.
Determine which element is oxidized and which is reduced CuSO4 plus Mg- Cu plus MgSO4?
In the reaction between CuSO4 and Mg, magnesium (Mg) is oxidized while copper (Cu) is reduced. Magnesium loses electrons to form Mg²⁺ ions, indicating oxidation, while copper ions (Cu²⁺) gain electrons to form elemental copper, indicating reduction. Thus, Mg is the reducing agent and Cu²⁺ is the oxidizing agent in this reaction.
Is Cu an oxidizing agent?
I'm almost certain that it can be used as an oxidizing agent. It is not as strong persay as Potassium permanganate, but depending on to what extent you are oxidizing something, that may be a good thing.
Systematic name Cu plus 1?
Cu(I), cuprous, Cu+.
Net inonic equation for Mg plus CuCl2 equals MgCl2 plus Cu?
mg + CuCl2 + MgCl2 + Cu Mg + Cu^+2 = Mg^+2 + Cu
What is the name of the Cu plus ion?
Cu+
Cu---Cu plus 2 plus 2e- this equation above represents the type of reaction called?
oxidation
What is being produced when Zn plus CuCl2 equals Cu plus ZnCl2?
Cu and ZnCl2 are being produced.
Which of the substances can act both as oxidising and reducing agent?
The terms "reducing agent" and "oxidizing agent" are relative. It seems that you already know this; that depending on the specific reaction, a given compound may be the reducing agent or the oxidizing agent, and in some reactions the same compound is both the oxidizing agent and the reducing agent. It is very important to remember that in an oxidization/reduction reaction, the reducing agent is oxidized and the oxidizing agent is reduced. Examples: 1) Aldehydes are one example of compounds that can act as reducing agents or oxidizing agents. As reducing agents, aldehydes can reduce Ag(I) in the form of [Ag(NH3)2]+ OH- to Ag metal. They can also reduce Cr(VI) to Cr(III) and Cu(II) to Cu(I). In each case, the aldehyde is oxidized to its corresponding carboxylic acid. As oxidizing agents, aldehydes (and ketones) can oxidize a hydride (H-) in sodium borohydride or lithium aluminumhydride to H+ as the aldehyde (or ketone) is reduced to an alcohol. Aldehydes and ketones are often used to form carbon-carbon bonds in aldol condensation reactions where a carbanion or an enolate ion attacks the carbonyl carbon of the aldehyde or ketone. In these reactions, the aldehyde or ketone is also reduced to an alcohol. 2) The nitrite anion is another example of a species that can serve as an oxidizing agent or a reducing agent in many reactions. Nitrite (formal charge of N+3) is readily oxidized to nitrate (formal charge of N+5) by the permanganate anion or it can be reduced all the way to ammonia (formal charge of N-3) by hydrogen sulfide. That's an impressive difference of six in the respective nitrogen oxidation states. Like aldehydes and ketones, nitrite can oxidize hydride to H+ in certain borohydride compounds in which nitrite is reduced to N2O, also known as laughing gas.
What happens to substance when it is oxidized?
Oxidation is the loss of electrons. Reduction is the gain of electrons. The oxidizing agent is reduced. The reducing agent is oxidized. Cu goes from 0 to +2, it lost electrons S went from +6 to +4, it gained electrons I went from 0 to +5, it lost electrons N went from +5 to +4, it gained electrons.
Show a reactionin which oxidizing agent is getting reduced and reducing agent is getting oxidised?
In the reaction between potassium permanganate (KMnO4) and hydrogen peroxide (H2O2), manganese in KMnO4 is reduced from +7 to +2 in the form of MnO2. The hydrogen peroxide is oxidized to water (H2O), where the oxygen in H2O2 goes from -1 to -2.
What is the chemical equation of copper plus ammonia?
Cu + 2NH3 → [Cu(NH3)2]+
