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3 years ago

Why is 1g of cobalt oxide nanoparticles a better catalyst than 1g of cobalt oxide powder?

Chemistry

1 answer:

jeka943 years ago

3 0

Answer;

It is because nano particles have a large surface area compared to the powder.

Explanation;

-The rate of a chemical reaction can be raised by increasing the surface area of a solid reactant. This is done by cutting the substance into small pieces, or by grinding it into a powder.

-If the surface area of a reactant is increased, it means more particles are exposed to the other reactant.

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AL(OH)3+ HCI—> ALCL3 +H2O

UkoKoshka [18]

Answer:

i dont know what you're asking here. But if you're asking what it is then:

Explanation:

Aluminum Hydroxide + Hydrogen Chloride = Aluminum Chloride + Water

Al and Oh3: Aluminum Hydroxide

H and Cl: Hydrogen Chloride

Al and Cl3: Aluminum Chloride

H2O: water

btw the first letter of every element should be capitalized. While the second and theird are lowercased.

4 0

3 years ago

A sample of chlorine gas is at 300K and 1.00 atm. At what temperature and pressure would it behave more like an ideal gas?

Fofino [41]

In lower temperatures, the molecules of real gases tend to slow down enough that the attractive forces between the individual molecules are no longer negligible. In high pressures, the molecules are forced closer together- as opposed to the further distances between molecules at lower pressures. This closer the distance between the gas molecules, the more likely that attractive forces will develop between the molecules. As such, the ideal gas behavior occurs best in high temperatures and low pressures. (Answer to your question: C) This is because the attraction between molecules are assumed to be negligible in ideal gases, no interactions and transfer of energy between the molecules occur, and as temperature decreases and pressure increases, the more the gas will act like an real gas.

3 0

3 years ago

determine mass of water formed when 12.5 L NH3(at298K and 1.50atm) is reacted with 18.9L of O2 (at 323K and 1.1atm)

sasho [114]

The mass of water formed is

<u><em>calculation</em></u>

Use the ideal gas equation to calculate the moles of NH3 and O2

that is Pv= n RT

where; P= pressure,

V= volume,

n = number of moles,

R=gas constant = 0.0821 l .atm/ mol.K

make n the formula of the subject by diving both side by RT

n = PV /RT

The moles of NH3

n= (1.50 atm x 12.5 L) /( 0.0821 L. atm /mol.k x 298 K) =0.766 moles

The moles of O2

=(1.1 atm x 18.9 L) / ( 0.0821 L. atm/ mol.k x 323 K) = 0.784 moles

write the reaction between NH3 and O2

4 NH3 + 5 O2 →4 No +6H2O

from equation above 0.766 moles of NH3 reacted to produce

0.766 x 6/4 =1.149 moles of H2O

0.784 moles of O2 reacted to produce 0.784 x 6/5=0.9408 moles of H20

since O2 is totally consumed, O2 is the limiting reagent and therefore the moles of H2O produced= 0.9408 moles

mass of H2O = moles x molar mass

from periodic table the molar mass of H2O = (1 x2)+16= 18 g/mol

mass = 18 g/mol x 0.9408 moles= 16.93 grams

3 0

3 years ago

PLEASE PLEASE HELP ME

Norma-Jean [14]

The high surface tension helps the paper clip - with much higher density - float on the water. The property of the surface of a liquid that allows it to resist an external force, due to the cohesive nature of its molecules.

Basically it means that there is a sort of skin on the surface of water where the water molecules hold on tight together. If the conditions are right, they can hold tight enough to support your paper clip. The paperclip is not truly floating, it is being held up by the surface tension.

5 0

3 years ago

Read 2 more answers

Calculate the heat energy released when 21.1 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point.

PSYCHO15rus [73]

Heat capacity yea urjjrjrjrbdnsnnend

3 0

3 years ago