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SashulF [63]
3 years ago
6

if you are told to get 100 mL of stock solution to use to prepare smaller size sample for an experiment, which piece of glasswar

e would you use?

Chemistry
1 answer:
fgiga [73]3 years ago
6 0

Answer:

A beaker  

Step-by-step explanation:

Specifically, I would use a 250 mL graduated beaker.

A beaker is appropriate to measure 100 mL of stock solution, because it's easy to pour into itscwide mouth from a large stock bottle.

You don't need precisely 100 mL solution.

If the beaker is graduated, you can easily measure 100 mL of the stock solution.

Even if it isn't graduated, 100 mL is just under half the volume of the beaker, and that should be good enough for your purposes (you will be using more precise measuring tools during the experiment).

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djyliett [7]

Answer:

Explanation:

1. The amount of CaCO3 must be so small that  

P

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P

CO

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3. The change in enthalpy may be used. If the reaction is exothermic, the heat produced can be thought of as a product. If the reaction is endothermic the heat added can be thought of as a reactant. Additional heat would shift an exothermic reaction back to the reactants but would shift an endothermic reaction to the products. Cooling an exothermic reaction causes the reaction to shift toward the product side; cooling an endothermic reaction would cause it to shift to the reactants’ side.

5. No, it is not at equilibrium. Because the system is not confined, products continuously escape from the region of the flame; reactants are also added continuously from the burner and surrounding atmosphere.

7. Add N2; add H2; decrease the container volume; heat the mixture.

9. (a) ΔT increase = shift right, ΔP increase = shift left; (b) ΔT increase = shift right, ΔP increase = no effect; (c) ΔT increase = shift left, ΔP increase = shift left; (d) ΔT increase = shift left, ΔP increase = shift right.

11. (a)  

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13. (a)  

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[

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; (b) [H2O] no change, [CO] no change, [H2] no change; (c) [H2O] decreases, [CO] decreases, [H2] decreases; (d) [H2O] increases, [CO] increases, [H2] decreases; (f) [H2O] decreases, [CO] increases, [H2] increases. In (b), (c), (d), and (e), the mass of carbon will change, but its concentration (activity) will not change.

15. Only (b)

17. Add NaCl or some other salt that produces Cl− to the solution. Cooling the solution forces the equilibrium to the right, precipitating more AgCl(s).

19. (a)

Hope this helps :)

3 0
3 years ago
Each atom of an element has the following electron configuration. 1s22s22p63s23p64s23d104p65s24d105p5 What is the name of the el
Temka [501]

Answer;

Iodine

Explanation;

Electron configurations are a way of keeping track of the location of the electrons around the nucleus.

Iodine is an element which belongs to the halogen family. The halogen group includes fluorine, chlorine, bromine, astatine, and iodine.

A neutral iodine atom would also have 53 electrons. Its ground state electron configuration would be:

1s22s22p63s23p64s23d104p65s24d105p5

5 0
3 years ago
Read 2 more answers
If the temperature changes in a chemical reaction, what has occurred?
ch4aika [34]
A reaction has happened
8 0
3 years ago
A solution that contains many dissolved molecules in a fixed amount of solution is called
Nezavi [6.7K]

Answer:

  • <em>A solution that contains many dissolved molecules in a fixed amount of solution is called</em> <u>concentrated</u>.

Explanation:

Solutions are homogeneous mixtures.

A solution contains at least one solute component and one solvent component all in the same phase.

The term solubility is used to express the maximum amount of solute that can be dissolved in certain amount of solvent, and is measured at a given temperature and pressure.

You may refer to a solution as <em>concentrated</em> or diluted. These are kind of vague terms, in the sense that they do not express how much solute is dissolved. They just tell if there are many dissolved particles (molecules or ions), which is expressed as concentrated, or just a few particle, which is express as diluted.

Other more specific terms used to refer the amount of solute dissolved in a solution are: unsaturated solution, saturated solution, and supersaturated solution.

<u>Unsaturated solution</u>: the solution contains less solute than what it can have. The solution may dissolve more solute.

<u>Saturated solution</u>: the solution has the maximum amount of solute that it can dissolve, at certain temperature and pressure. If you add more solute to a saturated solution, it will not get dissolved (unless you change the temperature or pressure).

<u>Supersaturated solution</u>: a special condition where the solution contains more solute than the saturated solution, at the same temperature and pressure. This is a very unstable situation and any perturbation will make that the excess solute precipitate.

4 0
3 years ago
Which one of these is a gas<br> NaNo3<br> KL<br> KCL<br> NH3
Deffense [45]

Answer:

nano3 is a solid so its not that one it has to be NH3

Explanation:

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}

3 0
3 years ago
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