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polet [3.4K]
3 years ago
8

The image represents the reaction between a certain number of molecules of N2 and H2

Chemistry
1 answer:
sertanlavr [38]3 years ago
7 0
2 molecules of N2, because the hydrogen is the limiting reactant, leaving there to be more N (4 molecules) so those 4 molecules create 2 N2 molecules.
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. Mitosis allows one cell to grow and split into 2 new cells. Will those 2 new cells split again explain.
Finger [1]

Answer:

Yes

Explanation:

They continue to split and grow and split again until the organism that is carrying them dies.

Sorry I don't really know how to explain:(

4 0
3 years ago
What is the molarity of a solution in which 0.732 moles of hcl are dissolved in 0.975 liters of solution?
posledela
Molarity is moles divided by liters so do .732 divided by .975 liters.
6 0
3 years ago
A piece of asphalt has a volume of 5.0 cm3 and a mass of 7.5 g. What is the density of the asphalt?
strojnjashka [21]
Density = mass / volume
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6 0
2 years ago
Name the compound formed when a copper cation has a 2+ charge combined with a bromine anion that has a 1- charge.
Rashid [163]

Answer: The compound is called copper (II) bromide or cupric bromide

Explanation:

7 0
2 years ago
In the laboratory, a student dilutes 18. 9 ml of a 10. 0 m perchloric acid solution to a total volume of 250. 0 ml. what is the
Sever21 [200]

The concentration of diluted solution is 0.756M.

From the question given above, the following data were obtained:

Volume of stock solution (V1) = 18.9 mL

Molarity of stock solution (M1) = 10 M

Volume of diluted solution (V2) = 250 mL

Molarity of diluted solution (M2) =?

We can obtain the molarity of the diluted solution by using the dilution formula as shown follow:

M1V1 = M2V2

10 × 18.9 = M2 ×250

189 = M2 × 250

Divide both side by 100

M2 = 189 / 250

M2 = 0.756 M

Therefore, the molarity of the diluted solution is 0.756 M.

Thus the concluded that concentration of the dilute acid is 0.756 M.

Learn more about concentration of diluted solution: brainly.com/question/10725862

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7 0
11 months ago
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