# Chemistry

Ik this has been answered, but doesn't the copper oxide have something to do with it? And could you explain it in simpler terms? I'm just confused because you said forget the copper oxide, but your using it somehow, what puzzles me is the carbon dioxide, because the copper oxide plus the carbon make the copper, but also the carbon dioxide. Could you explain it simpler and explain how you got that answer (simpler)

Copper Oxide + Carbon -> Copper + Carbon Dioxide

Calculate the mass of carbon needed to obtain 63.5g of copper from 79.5g of Copper Oxide

1. 0
2. 0
3. 7
1. balance the equation

2CuO+C>>2Cu + CO2

each mole of carbon yields 2mmoles Cu

how many moles of Copper is 63.5 grams?
so you need half that number of moles of Carbon, or .5 moles of carbon, or six grams.

1. 0
2. 0
posted by bobpursley
2. 2CuO + C ==> 2Cu + CO2
1. I ignored the CuO because the problem states you want 63.5 g Cu. How many mols Cu is that? mols Cu = grams/atomic mass = 63.5/63.5 = 1 mol Cu is what you want.
2. If it comes from the equation above then 2 mols Cu is obtained for every mol C or 1/2 mol C for 1 mol Cu. So 1 mol Cu I will get from 1/2 mol C.
3. Since g = mols x atomic mass, then g C = mols C x atomic mass C = 0.5 x 12 = 6 grams C.
4. Note I didn't use CuO anywhere except in the equation. If it follows all of the laws of chemistry, knowing Cu I want will tell me how much CuO I need, how much C I need, and how much CO2 will be produced. But the problem didn't ask anything about CO2, or CuO so I didn't use them anywhere.
5. There COULD be a complicating factor IF (and only IF) the CuO would not give the amount of Cu you want in the problem BUT 1 mol CuO is 63.5 + 16 = 79.5; however, in that case I would have pointed out that it couldn't be done; i.e., 60 g CuO for example could not produce 63.5 g Cu so we were spinning our wheels.

To work a simple stoichiometry problem (as opposed to a limiting reagent problem) you need four steps.
1. Write and balance the equation.
2. Convert grams of what you have to mols. mols = grams/atomic mass in this case or grams/molar mass in the case of molecules. That's the 63.5/63.5 = 1 mol Cu step above.
3. Using the coefficients in the balanced equation, convert mols of what you have (in this case mols Cu) to mols of what you want (in this case C). That's the 1 mol Cu x (1 mol C/2 mols Cu) = 1 x 1/2 = 0.5 mols C
4. Then convert mols of what you want (the C) to grams. g = mols x atomic mass = 0.5 x 12 = 6.

These four steps will take care of any non-limiting reagent problem you have.

1. 0
2. 0
posted by DrBob222

## Similar Questions

1. ### Chemistry

You synthesized copper (I) chloride and copper (I) oxide. How do they differ from their copper (II) analogs? comment on the stability of these moist solids in air. If unstable, what is the likely product of decomposition? -I'm not
2. ### Chemistry

is it easy to distinguish between between the different oxidation states of copper? why? -I answered yes because copper (I) is not as stable as copper (II), and there is a noticeable colour difference You synthesized copper (I)
3. ### Chemistry

Copper dissolves in nitric acid, producing copper (ll) nitrate. After reaction with sodium hydroxide and heating, copper nitrate changes to copper (ll) oxide. Calculate the percent yield of this process if 1.235 g of copper
4. ### Chemistry

When copper(II) oxide is heated in the presence of hydrogen gas, elemental copper and water are produced. What mass of copper can be obtained if 34.0 g copper(II) oxide is used?
5. ### chemistry

When copper(II) oxide is heated in the presence of hydrogen gas, elemental copper and water are produced. What mass of copper can be obtained if 22.8 g copper(II) oxide is used?

One of the reactions involved in the smelting of copper sulfide ores involves copper (I) oxide and copper (I) sulfide: 2Cu2O2 + Cu2S ---> 6Cu + SO2 Assuming that 35.00 g of copper (I) oxide is heated with 25.00 g of copper (I)
7. ### chemistry

One of the reactions involved in the smelting of copper sulfide ores involves copper(I) oxide and copper (I) sulfide: 2Cu2O(solid) + Cu2S(solid) ---> 6Cu(solid) + SO2(gas) Assuming that 35.00 g of copper (I) oxide is heated with
8. ### science

How do i separate the mixture of zinc oxide and copper oxide to obtain pure copper oxide
9. ### Chemistry

ammonia gas reacts with copper (ii) oxide at high temperatures to produce elemental nitrogen, copper metal, and water vapor. Assume that 36.2g ammonia reacts with 180.8 g copper ii oxide. (balanced equation: 2 NH4 (ammonium) (g) +
10. ### Chemistry

Can you tell me if these are right please? When 2.50g of copper reacts with oxygen the copper oxide product has a mass of 2.81g. What is the simplest formula of the copper oxide. I got Cu2O (copper (I) oxide). Aluminum and oxygen

More Similar Questions