Fox News – Breaking News Updates

latest news and breaking news today

Which substance is the oxidizing agent in this reaction?
2CuO+C→2Cu+CO2?

source : yahoo.com

Which substance is the oxidizing agent in this reaction?
2CuO+C→2Cu+CO2?

Oxidation is an increase in the oxidation state, while reduction is the decrease in oxidation state. The oxidizing agent is the reactant which does the oxidizing and therefore, contains the element reduced. And the reducing agent is the reactant which does the reducing and therefore, contains the element oxidized.

..+2-2………0 ………….0 ……..+4-2

2CuO(s) + C(s) –> 2Cu(s) + CO2(g)

Carbon is oxidized, and therefore, C is the reducing agent.

Cu in CuO is reduced and therefore, CuO is the oxidizing agent.

Answered: Safari File Edit View History Bookmarks… | bartleby

Answered: Safari File Edit View History Bookmarks… | bartleby – Solution for Safari File Edit View History Bookmarks Window Help ) 47% Sun 11:03 AM session.masteringchemistry.com Consider summer class… Inbox (13) -…Solved: Which element is oxidized in this reaction? 2CuO + C arrow 2Cu + CO2 By signing up, you'll get thousands of step-by-step solutions to your…In redox reaction the oxidation number of a molecule, atom, or ion changes by gaining or losing an electron. In the reaction : C u O + H 2 C u + H 2 O n the reaction H 2 is oxidized since it has lost electrons and C u is reduced since it has gained electrons.

Which element is oxidized in this reaction? 2CuO + C arrow – The oxidizing agent is the reactant which does the oxidizing and therefore, contains the element reduced. And the reducing agent is the reactant which does the reducing and therefore, contains the…Identify the substances that are oxidized and reduced, and indicate which is the oxidizing agent and which is the reducing agent. Solution. Analyze: We are given a redox equation and asked to identify the substance oxidized and the substance reduced and to label one as the oxidizing agent and the other as the reducing agent. Plan:The reducing agent is a substance that causes reduction by losing electrons; therefore its oxidation state increases. The simplest way to think of this is that the oxidizing agent is the substance that is reduced, while the reducing agent is the substance that is oxidized as shown in Figure \(\PageIndex{1}\) and summarized in Table \(\PageIndex

Which element is oxidized in this reaction? 2CuO + C arrow

In the reaction CuO + H2 → Cu + H2O which substance gets – What is a process in which a substance acts as both an oxidizing agent and a reducing agent? Which element is oxidized in this reaction? 2CuO+C→2Cu+CO2 Which element is reduced in this reaction? 16H++2Cr2O72−+C2H5OH→4Cr3++11H2O+2CO2. What is the reduction half-reaction for #2Mg + O_2 -> 2MgO#?(1) 2CuO + C → 2Cu + CO2 In this reaction, oxidation number of C changes from 0 to +4. As oxidation no of C increases, C is oxidized from C to C4+. (2) 16H+ + 2Cr2O72− + C2H5OH → 4Cr3+ + 11H2O + 2CO2Which Substance Is The Oxidizing Agent In This Reaction? 2CuO+C 2Cu+CO2 Question: Which Substance Is The Oxidizing Agent In This Reaction? 2CuO+C 2Cu+CO2 This problem has been solved!

Solved: Part B Which Substance Is The Oxidizing Agent In T ...
Solved: Which Substance Is The Oxidizing Agent In This Rea ...
Chemistry Archive | September 11, 2014 | Chegg.com
Solved: Part B Which Substance Is The Oxidizing Agent In T ...

Menentukan oksidator, reduktor pada persamaan redoks – Hi meet with me, now i want to explain how to determine oxidizing agent and reducing agent in chemical equation An chemical equation called redox equation if oxidation-reduction reaction occured in that reaction In this term, called oxidation if oxidation number are increase, and called reduction if oxidation number are decrease .

Reduction of copper oxide – This experiment enables us to find the formula of copper oxide by reducing it in a stream of hydrogen.
The hydrogen removes the oxygen and forms water, which will be steam at
the temperature of the experiment.
This is the apparatus we use. A pyrex reduction tube, which is
essentially a boiling tube, with a small hole in the end to
allow excess hydrogen to escape. Before starting the experiment it's
important to familiarise yourself with how to use a hydrogen cylinder. This valve here, the cylinder valve, is
operated by a spanner. Turning the spanner allows hydrogen gas into the pressure reduction valve gear here. This valve is the pressure reduction valve, turn it on and we'll see a reading on that gauge there, and finally the flow rate of the hydrogen is
regulated using this needle valve here. We first need to weigh the empty reduction tube. The balance used must read to at least two decimal places. We now place about three grams of copper oxide, which is really a couple of spatula-fulls of the powder, into the reduction tube. Try to place this in the centre of the tube. If it's too close to the hole end there's a risk of the hydrogen flow blowing some of it out. If it's too close to this end, then there's a
risk of heating the bung while we heat the copper oxide. Having put the copper oxide into the tube we re-weigh it. The copper oxide should be dry. Old stock may need to be dried in an oven or desiccator. We now use the needle valve to adjust the flow of hydrogen, a rate of flow that you can just feel on your cheek is about right. Now place the hydrogen delivery tube in the end of the reduction tube. The next step is to light the hydrogen but
it's important to wait for about a minute to make sure all the
hydrogen has flushed out any air from the reduction tube
otherwise you could get an explosive mixture in there. For the
lighting process we have safety screens to protect the
demonstrator and the audience. Once something like a minute has passed we now light the hydrogen and adjust the flame until it's about 2 cm or so. At this point there's no more explosion
risk so we can dispense with the safety screens. Now we heat the copper oxide using a roaring Bunsen flame and using the hottest part of the flame,
which is just beyond the blue colour. At this point, a number of interesting observations can be made. These will probably need to be pointed out to the audience. Droplets of water will condense on the
cooler part of the reduction tube near the hole. These will evaporate as the tube gets hotter. The height of the flame will drop as some of the hydrogen is used up reacting with the oxygen in the copper
oxide. The flame may develop a green coloration caused by copper atoms vapourised into the flame. Use the Bunsen burner to chase the glow along the length of the oxide until all the black copper oxide has
been changed to pinkish copper. This will take up to a minute. When
no trace of black remains continue to heat for at least a further
minute to ensure that all the oxide on the inside of the heap has reacted. If in any doubt continue heating for longer. Make sure any condensation has
evaporated. When you're confident that all the copper oxide has been reduced, the flame is back to its original height,
you can stop heating. It's now important to leave the apparatus
exactly as it is with the hydrogen flowing. This is to prevent air from diffusing
back into the reduction tube and converting some of the hot copper back to the oxide. Continue until the tube is cool enough
to touch comfortably. You now blow out the flame, move the hydrogen delivery tube and turn off at the cylinder and re-weigh the tube, which now contains copper. The copper looks pinkish and not
particularly metallic. If students are not convinced that it
actually is metallic copper it's possible to get some of it out of the tube and use a circuit tester to show that it is in fact metallic. Finally, we have to turn off the hydrogen
cylinder. We first close the cylinder valve with a spanner and we then need to use the pressure reduction valve. We turn it on, and the needle valve on to vent any hydrogen from the valve gear. Finally, turn off the pressure reduction
valve and also the needle valve. .