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3 years ago

What should happen when a piece of copper is placed in 1m hcl?

Chemistry

1 answer:

masha68 [24]3 years ago

3 0

D. nothing happens

(Additional oxidizer is necessary for dissolution of copper.)

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The law of reflection states that the angle of incidence and the angle of reflection are always

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Answer:

The law of reflection states that the angle of incidence and the angle of reflection are always equal.

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3 years ago

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What is the correct formula for Tin (IV) chromate nonahydrate?

Mashcka [7]

Answer:

Sn(CrO4)2 or Cr2O8Sn

Explanation:

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3 years ago

The magnitude of an earthquake can range from less than 1 to at least

shusha [124]

The magnitude of an earthquake can range from 1 to at least 8

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3 years ago

2. The power steering in an automobile has a mechanical advantage of roughly 75. If the input force on the steering wheel is 49

sertanlavr [38]

1.53

Explanation:

49/x=75 X or output = 1.53

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3 years ago

A student measures out exactly 0.105 g of salicylic acid and runs the experiment as dictated in the lab manual. They obtain 0.11

scoray [572]

<u>Answer:</u> The percent yield of the reaction is 8.10 %.

<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)

Given mass of salicylic acid = 0.105g

Molar mass of salicylic acid = 138.12 g/mol

Putting values in equation 1, we get:

$\text{Moles of salicylic acid}=\frac{0.105g}{138.12g/mol}=0.0079mol$

The chemical equation for the formation of aspirin from salicylic acid follows:

$\text{Salicylic acid + Acetic anhydride}\rightarrow \text{Aspirin + Acetic acid}$

By Stoichiometry of the reaction:

1 mole of salicylic acid produces 1 mole of aspirin

So, 0.0076 moles of salicylic acid will produce = $\frac{1}{1}\times 0.0076=0.0076mol$ of aspirin

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

Molar mass of aspirin = 180.16 g/mol

Moles of aspirin = 0.0076 moles

Putting values in equation 1, we get:

$0.0076mol=\frac{\text{Mass of aspirin}}{180.16g/mol}\\\\\text{Mass of aspirin}=(0.0076mol\times 180.16g/mol)=1.37g$

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 = 0.111 g

Theoretical yield of aspirin = 1.37 g

Putting values in above equation, we get:

$\%\text{ yield of aspirin}=\frac{0.111g}{1.37g}\times 100\\\\\% \text{yield of aspirin}=8.10\%$

Hence, the percent yield of the reaction is 8.10 %.

6 0

3 years ago