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2 years ago

6.5 Moles of Al reacts with 7.2 Moles of H2O What is the limiting reactant and calculate the Theoretical Yield?

Chemistry

1 answer:

SVEN [57.7K]2 years ago

4 0

Answer:

H₂O is the limiting reactant

Theoretical yield of 240 g Al₂O₃ and 14 g H₂

Explanation:

Find how many moles of one reactant is needed to completely react with the other.

6.5 mol Al × (3 mol H₂O / 2 mol Al) = 9.75 mol H₂O

We need 9.75 mol of H₂O to completely react with 6.5 mol of Al. But we only have 7.2 mol of H₂O. Therefore, H₂O is the limiting reactant.

Now find the theoretical yield:

7.2 mol H₂O × (1 mol Al₂O₃ / 3 mol H₂O) × (102 g Al₂O₃ / mol Al₂O₃) ≈ 240 g Al₂O₃

7.2 mol H₂O × (3 mol H₂ / 3 mol H₂O) × (2 g H₂ / mol H₂) ≈ 14 g H₂

Since the data was given to two significant figures, we must round our answer to two significant figures as well.

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A Carnot cycle operates between the temperatures limits of 400 K and 1600 K, and produces 3600 kW of net power. The rate of entr

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The rate of entropy change:

The rate of entropy change of the working fluid during the heat addition process is 3 kW/K

What is the Carnot cycle?

The Carnot Cycle is a thermodynamic cycle made up of reversible isothermal expansion, adiabatic expansion, isothermal compression, and adiabatic compression processes in succession.
The ratio of the heat absorbed to the temperature at which the heat was absorbed determines the change in entropy.

The entropy of a system:

The rate of heat addition is expressed as,

Q = $\frac{WT_{H}}{T_{H}- T_{L}}$

The entropy of a system is a measure of how disorderly a system is getting. The rate of entropy generation during heat addition is,

$S_{gen} = \frac{Q}{T_{H}} = \frac{W}{T_{H} - T_{L}}$

Calculation:

<u>Given:</u>

$T_{L}$ = 400K

$T_{H}$ = 1600K

W = 3600 kW

Put all the values in the above equation, and we get,

$S_{gen} = \frac{W}{T_{H} - T_{L}}$ = $\frac{3600}{1600-400}$ = 3 kW/K

The rate of entropy change is 3 kW/K

Learn more about the Carnot cycle here,

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1 year ago

How many moles of NaOH are in 13.25 mL of 0.323 M NaOH?

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M=mol/L, 0.323M=mol/0.01325. Rework to solve for mol and bam! (I.e. times the two numbers)

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2 years ago

Which of the following statements is not true of the phases of a given substance ?

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The particles of gases have more kinetic energy than liquids and gases.

Explanation:

We know that in case of solids the molecules are very tightly packed , in case of liquids the molecules are loosely packed and lastly in case of gases the molecules are very loosely packed.
As we known in case of solids energy present is very less and in case of liquids energy present is more than solids and lastly in case of gases the energy present is most.
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2 years ago

Three common gaseous compounds of nitrogen and oxygen of different elementary composition are known: (A) laughing gas containing

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Answer:

Please find how these data prove the law of multiple proportions below

Explanation:

The law of multiple proportions was proposed by an English chemist called John Dalton. The law states that when two elements combine and to form more than one compound. The weights/masses of the second element in the two compounds, which combines with a fixed ratio of the first element, is in a simple whole number ratio.

In this question, Nitrogen is said to combine with oxygen to give three different compounds as follows:

A) laughing gas containing 63.65% nitrogen i.e. 0.6365g

This means that the mass of oxygen will be (1-0.6365) = 0.3635g

B) colorless gas containing 46.68% nitrogen i.e. 0.4668g

This means that the mass of oxygen will be 0.5332g

C) brown toxic gas containing 30.45% nitrogen i.e. 0.3045g

This means that the mass of oxygen will be 0.6955g

The ratios of oxygen in the three compounds is therefore:

0.3635: 0.5332: 0.6955

Divide this ratio by the smallest number (0.3635)

0.3635/0.3635 = 1

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0.6955/0.3635 = 1.913

Multiply this ratio by 2, we have:

2: 2.9 : 3.8

Hence, the simple whole number ratio is 2:3:4.

This proves the law of multiple proportions that oxygen is in simple whole number ratio in the three different compounds.

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