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Is BaTiO4 stronger than Cu?
No, BaTiO4 is not stronger than Cu. Copper (Cu) is a metal known for its strength and durability, making it more suitable for structural applications where strength is crucial. BaTiO4 is a ceramic material that is known for its piezoelectric properties rather than its mechanical strength.
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.
What happens to H in the CuO H2 to Cu H2O?
In the reaction involving copper(II) oxide (CuO) and hydrogen gas (H2), hydrogen acts as a reducing agent. The hydrogen reduces CuO to metallic copper (Cu), while itself being oxidized to form water (H2O). This process involves the transfer of electrons, where CuO gains electrons to form Cu, and H2 loses electrons to form H2O. Overall, the chemical reaction can be summarized as: CuO + H2 → Cu + H2O.
Is BaTiO4 stronger than Cu?
No, BaTiO4 is not stronger than Cu. Copper (Cu) is a metal known for its strength and durability, making it more suitable for structural applications where strength is crucial. BaTiO4 is a ceramic material that is known for its piezoelectric properties rather than its mechanical strength.
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.
How do you make a old magnet stronger?
Run a cu-rent through it
How would you get copper from copper oxide?
you obtain Cu from CuO only by reducing with hydrogen or carbon monooxide: CuO + H2 → Cu + H2O
What is the oxidizing agent for Zn plus CuCl2--ZnCl2 plus Cu?
In the reaction Zn + CuCl2 → ZnCl2 + Cu, CuCl2 is the oxidizing agent because it accepts electrons from Zn, causing zinc to be oxidized and copper to be reduced.CuCl2 itself gets reduced to Cu.
Is 3 cu ft bigger than 4 cu ft?
Is 3 bigger than 4? NO! 4 cu ft is bigger.
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.
What happens to H in the CuO H2 to Cu H2O?
In the reaction involving copper(II) oxide (CuO) and hydrogen gas (H2), hydrogen acts as a reducing agent. The hydrogen reduces CuO to metallic copper (Cu), while itself being oxidized to form water (H2O). This process involves the transfer of electrons, where CuO gains electrons to form Cu, and H2 loses electrons to form H2O. Overall, the chemical reaction can be summarized as: CuO + H2 → Cu + H2O.
How many lbs are in a cu ft?
The answer is specific to the product in the cu ft. A cu ft of water will be different than that of a cu ft of feathers ETC.
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.
