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Murrr4er [49]
3 years ago
9

Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron mesh impregnated wit

h oxides as a catalyst. For the following reaction, equilibrium constants (Kp values) are seen below as a function of temperature.
N2(g) + 3 H2(g) reverse reaction arrow 2 NH3(g)

300°C 4.34 multiplied by 10-3 atm-2
500°C 1.45 multiplied by 10-5 atm-2
600°C 2.25 multiplied by 10-6 atm-2
This is an exothermic reaction, can you explain why it is exothermic and not endothermic?
Chemistry
1 answer:
Alexus [3.1K]3 years ago
6 0

Answer:

Explanation:

The reaction of production of ammonia is as follows

N₂ + 3H₂ ⇄ 2NH₃

From the data given , it is clear that

equilibrium constant decreases as temperature increases . In other words

at higher temperature less and less of ammonia is produced .

According to Le Chatelier's Principle , reaction tends to go in the direction so that the effect of external change is minimized. Since the increase in temperature reduces the forward reaction , that means reaction is exothermic .

So , reduction in reaction , helps reduce the production of heat to reduce the effect of temperature increase.

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What attractive force draws in surrounding electrons for chemical bonds?
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3 years ago
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Calculate the maximum numbers of moles and grams of H₂S that can form when 158 g of aluminum sulfide reacts with 131 g of water:
Phantasy [73]

What is Chemical Reaction?

A chemical reaction is the chemical transformation of one set of chemical components into another.

Main Content

Mass of aluminium sulfide is 158g

Mass of water is 131g

The chemical reaction: Al_{2}S_{3} +H_{2}O  _\to  Al(OH)_{3} + H_{2}S

First, balance the chemical equation

Al_{2}S_{3} + 6H_{2}O  \to 2Al(OH)_{3} + 3H_{2}S

Aluminium sulfide has a molar mass of 150.16 g/mol and water has a molar mass of 18.02 g/mol. As a result, the moles of aluminum sulfide are computed as follows:

n_{Al_{2}S_{3}  } = \frac{Mass}{Molar mass}\\n_{Al_{2} S_{3}  } = \frac{158g}{150.16g/mol}   \\n_{Al_{2}S_{3} }=1.05 mol

From the chemical reaction , the ratio of molar is 3mol H_{2}S/1 mol Al_{2}S_{3}. So, the moles of hydrogen sulfide are:

n_{H_{2} O} =\frac{131g}{18.02g/mol}

       = 7.26mol

From the chemical reaction, the molar ratio is 3 mol H_{2}S/6 mol H_{2}O. So, the moles of hydrogen sulfide are:

Moles of H_{2}S formed = 7.26 mol H_{2}O \times \frac{3 mol H_{2}S }{6 mol H_{2} O} }

Th liming reactant isAl_{2}S_{3} beacuse the mass of Al_{2}S_{3} forms less product than water. Therefore, the maximum number of moles of H_{2}S is 3.15 mol.  We know that molar mass of H_{2}S is 34.10g/mol. So, the maximum mass of H_{2}S formed is,

m_{H_{2}S } = n_{H_{2}S } \times Molar mass of H_{2}S

         = 3.15 mol \times 34.10g/mol

         = 107.4g

Now, multiplying the number of moles of Al_{2}S_{3} by the molar ratio between Al_2S_3 and H_2O which is 6mol H_2O/1mol Al_2S_3 we get the number of moles of H_2O reacted.

Moles of H_2O reacted = 1.05 mol Al_{2}S_3 \times \frac{6 mol H_2O}{1 mol Al_2S_3}

                                     = 6.31 mol H_2O

The mass of H_2O is,

m_{H_{2} O} = 6.31 mol \times 18.02g/ mol

          = 114g

On subtracting, the mass of H_2O reacted from the given mass of H_2O is,

m_{H_2O} = (131-114)g

         = 17g

Hence, the excess remaining reactant is 17g

To learn more about Chemical Reaction

brainly.com/question/11231920

#SPJ4

 

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Answer:

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Answer: Option (c) is the correct answer.

Explanation:

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Thus, we can conclude that out of the given options, wood, a mixture of different substances is a material that does not melt at any temperature.

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