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kherson [118]
2 years ago
9

Balance the equation above please ​

Chemistry
2 answers:
Zepler [3.9K]2 years ago
8 0

Answer:

everything can be found in the picture

Anon25 [30]2 years ago
6 0

Answer:

<h3><em><u>Balanced</u></em><em><u> </u></em><em><u>Equation</u></em><em><u>:</u></em><em><u>-</u></em></h3>

Al2(CO3)3. ---heat---> Al2O3 + <em><u>3</u></em> CO2

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An 85.0 g sample of iron requires 954 J of heat to raise its temperature 25.0°C. What is the specific heat of the iron? \
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Answer:448.9 J/kg °C

Explanation:

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What is the mass of 8.12 × 1023 molecules of CO2 gas? (Atomic mass of carbon = 12.011 u; oxygen = 15.999 u.)
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Answer:

8306.76

Explanation:

you just calcuate 8.12 x 1023 and that will give you the answer

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Which of the following statements is true? Question 2 options: Chemical reaction rates vary with the conditions of the reaction,
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3 years ago
Aspirin can be made in the laboratory by reacting acetic anhydride (C 4H 6O 3) with salicylic acid (C 7H 6O 3) to form aspirin (
Anastasy [175]

<u>Answer:</u> The percent yield of the aspirin is 77.5 %.

<u>Explanation:</u>

To calculate the mass of acetic anhydride, we use the equation:

\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}

Density of acetic anhydride = 1.08 g/mL

Volume of acetic anhydride = 2.80 mL

Putting values in above equation, we get:

1.08g/mL=\frac{\text{Mass of acetic anhydride}}{2.80mL}\\\\\text{Mass of acetic anhydride}=(1.08g/mL\times 2.80mL)=3.024g

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

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

  • <u>For acetic anhydride:</u>

Given mass of acetic anhydride = 3.024 g

Molar mass of acetic anhydride = 102.1 g/mol

Putting values in equation 1, we get:

\text{Moles of acetic anhydride}=\frac{3.024g}{102.1g/mol}=0.0296mol

  • <u>For salicylic acid:</u>

Given mass of salicylic acid = 1.24 g

Molar mass of salicylic acid = 138.12 g/mol

Putting values in equation 1, we get:

\text{Moles of salicylic acid}=\frac{1.24g}{138.12g/mol}=0.0089mol

The chemical equation for the combustion of hexane follows:

C_4H_6O_3+C_7H_6O_3\rightarrow C_9H_8O_4+C_2H_4O_2

By Stoichiometry of the reaction:

1 mole of salicylic acid reacts with 1 mole of acetic anhydride

So, 0.0089 moles of salicylic acid will react with = \frac{1}{1}\times 0.0089=0.0089mol of acetic anhydride

As, given amount of acetic anhydride is more than the required amount. So, it is considered as an excess reagent.

Thus, salicylic acid is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

1 mole of salicylic acid produces 1 mole of aspirin

So, 0.0089 moles of salicylic acid will produce = \frac{1}{1}\times 0.0089=0.0089moles of aspirin

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

Molar mass of aspirin = 180.16 g/mol

Moles of aspirin = 0.0089 moles

Putting values in equation 1, we get:

0.0089mol=\frac{\text{Mass of aspirin}}{180.16g/mol}\\\\\text{Mass of aspirin}=(0.0089mol\times 180.16g/mol)=1.60g

  • 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 = 1.24 g

Theoretical yield of aspirin = 1.60 g

Putting values in above equation, we get:

\%\text{ yield of aspirin}=\frac{1.24g}{1.60g}\times 100\\\\\% \text{yield of aspirin}=77.5\%

Hence, the percent yield of the aspirin is 77.5 %.

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3 years ago
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