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Vlad1618 [11]
3 years ago
11

Enter the net ionic equation, including phases, for the reaction of AgNO3 (aq) and KCl(aq). Refer to the solubility rules as nee

ded.

Chemistry
2 answers:
ollegr [7]3 years ago
5 0

Answer:

Ag+(aq) + Cl-(aq) -> AgCl(s)

Explanation:

Given the next molecular equation:

AgNO3 (aq) + KCl (aq) -> AgCl(s) + KNO3 (aq)

To get the net ionic equation, first write separate ions for soluble electrolytes, those indicated with a '(aq)':

Ag+(aq) + NO3-(aq) + K+(aq) + Cl-(aq) -> AgCl(s) + K+(aq) + NO3-(aq)

And then cancel any ion on both sides of the previous equation, as follows:

Ag+(aq) + Cl-(aq) -> AgCl(s)

artcher [175]3 years ago
3 0

Answer:

Explanation: you need to remove the subscript of 5

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Determine the empirical formula of a compound containing 1.71 g of silicon and 8.63 g of chlorine.
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Answer:

The answer to your question is: SiCl₄

Explanation:

Data

amount of Si      1.71 g

amount of Cl     8.63 g

MW Si = 28 g

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Process (rule of three)

For Si                                                        For Cl

        28 g of Si ------------------ 1 mol                      35.5 g of Cl --------------- 1 mol

          1.71g of Si  ---------------   x                              8.63 g of Cl --------------  x

         x = 1.71 x 1 / 28 = 0.06 mol                          x = 8.63 x 1 / 35.5 = 0.24 mol

Now, divide both results by the lowest of them.

Si = 0.06 mol / 0.06 = 1 molecule of Si     Cl = 0.24 / 0.06 = 4 molecules of Cl

Finally

                     Si₁ Cl₄ or SiCl₄

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