How many atoms are in ErAg

Which one of the atoms shown would be most likely to form a cation with a charge of 1?

olga55 [171]

Ions are stable atoms of elements formed when original atoms loose or gain electrons to form stable configuration. Anions are negatively charged ions formed when atoms gain electrons while cations are the positively charged ions formed when atoms loose electrons. In this case a charge of +1 means an atom lost one electron to form a stable configuration. Therefore, the correct answer is A

6 0

3 years ago

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Does anyone know Coulomb’s law??

Ierofanga [76]

Answer:

the force between charged particles increases when they are in solid form

3 0

2 years ago

Suppose 40.8g of copper(II) acetate is dissolved in 200.mL of a 0.70 M aqueous solution of sodium chromate.

Contact [7]

Answer:

0.42 M

Explanation:

The reaction that takes place is:

Cu(CH₃COO)₂ + Na₂CrO₄ → Cu(CrO₄) + 2Na(CH₃COO)

First we calculate the moles of Na₂CrO₄, using the given volume and concentration:

(200 mL = 0.200L)

0.70 M * 0.200 L = 0.14 moles Na₂CrO₄

Now we calculate the moles of Cu(CH₃COO)₂, using its molar mass:

40.8 g ÷ 181.63 g/mol = 0.224 mol Cu(CH₃COO)₂

Because the molar ratio of Cu(CH₃COO)₂ and Na₂CrO₄ is 1:1, we can directly substract the reacting moles of Na₂CrO₄ from the added moles of Cu(CH₃COO)₂:

0.224 mol - 0.14 mol = 0.085 mol

Finally we calculate the resulting molarity of Cu⁺², from the excess cations remaining:

0.085 mol / 0.200 L = 0.42 M

4 0

3 years ago

How do you find the molar mass of a hydrate

Darya [45]

If you mean hydrate as in MgSO4 · 7H2O, then simply find the molar mass of each element you see.

For the example above, that means you would add the molar mass (found on the periodic table) of Mg, then S, then 4(O), 14(H), and 7(O).

The results would be your molar mass for the hydrate.

I hope this is what you meant by your question!

6 0

3 years ago

Here are some data from a similar experiment, to determine the empirical formula of an oxide of tin. Calculate the empirical for

eduard

Answer:

Empirical formula of the Tin oxide sample is SnO₂

Explanation:

Tin reacts with combines with oxygen to form an oxide of tin.

Mass of crucible with cover = 19.66 g

Mass of crucible, cover, and tin sample = 22.29 g

Mass of crucible and cover and sample, after prolonged heating gives constant weight = 21.76 g

Mass of Tin oxide sample = 22.29 - 19.66 = 2.63 g

Mass of ordinary tin, after heating to breakdown the tin and oxygen = 21.76 - 19.66 = 2.1 g

Meaning that, mass of oxygen in the tin oxide sample = 2.63 - 2.1 = 0.53 g

Mass of Tin in the Tin Oxide sample = 2.1 g

Mass of Oxygen in the Tin oxide sample = 0.53 g

Convert these to number of moles

Number of moles of Tin on the Tin oxide sample = 2.1/118.71 = 0.0177

Number of moles of Oxygen in the Tin oxide sample = 0.53/16 = 0.0335

divide the number of moles by the lowest number

0.0177:0.0335

It becomes,

1:2

SnO₂

Hence, the empirical formula for the Tin oxide sample = SnO₂

7 0

3 years ago