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SVETLANKA909090 [29]
3 years ago
7

Element J is 1s 2s 2p 3s . (i) How many unpaired electrons does J have?

Chemistry
1 answer:
Mama L [17]3 years ago
7 0

Answer:6

Explanation:

3+3

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White gold is used in jewelry and contains two elements, gold and palladium. A jeweler has two different samples that are both i
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Solution : As they have uniform composition throughout they are considered as homogeneous mixture. Both samples are mixture of two metals (gold and palladium) thus are alloys.
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Whats the main difference between a double replacement reaction and a single replacement
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Answer:

a single-replacement reaction replaces one element for another in a compound. A double-replacement reaction exchanges the cations, or the anions, of two ionic compounds.

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3 years ago
Aspirin sun thesis Green Chemistry and Assime the aspirin is prepared by the following reaction and that 10.09. of salicylic aci
klemol [59]

<u>Answer:</u> The percentage yield of aspirin is 38.02 %.

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}      .....(1)

  • <u>For salicylic acid:</u>

Given mass of salicylic acid (C_7H_6O_3) = 10.09 g

Molar mass of salicylic acid (C_7H_6O_3) = 138.12 g/mol

Putting values in equation 1, we get:

\text{Moles of salicylic acid}=\frac{10.09g}{138.12g/mol}=0.0730mol

The chemical equation for the formation of aspirin follows:

C_7H_6O_3+C_4H_6O_3\rightarrow C_9H_8O_4+CH_3COOH

As, acetic anhydride is present in excess. So, it is considered as an excess reagent.

Thus, salicylic acid is a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

1 mole of salicylic acid produces 1 mole of aspirin.

So, 0.0730 moles of salicylic acid will produce = \frac{1}{1}\times 0.0730=0.0730mol of aspirin

Now, calculating the mass of aspirin from equation 1, we get:

Molar mass of aspirin = 180.16 g/mol

Moles of aspirin = 0.073 moles

Putting values in equation 1, we get:

0.073mol=\frac{\text{Mass of aspirin}}{180.16g/mol}\\\\\text{Mass of aspirin}=13.15g

To calculate the percentage yield of aspirin, we use the equation:

\%\text{ yield}=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100

Experimental yield of aspirin = 5.0 g

Theoretical yield of aspirin = 13.15 g

Putting values in above equation, we get:

\%\text{ yield of aspirin}=\frac{5.0g}{13.15g}\times 100\\\\\% \text{yield of aspirin}=38.02\%

Hence, the percent yield of aspirin is 38.01 %.

6 0
3 years ago
Na + Cl --&gt; NaCl
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38.152 g NaCl would be produced.

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\frac{(23 + 35.5) \times 15}{23}  \\  = 38.152 \:  \: g

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