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Pachacha [2.7K]
3 years ago
15

Ammonia gas combines with hydrogen chloride gas, forming solid ammonium chloride.

Chemistry
1 answer:
irina [24]3 years ago
5 0

Answer:

a. The balanced chemical equation for the reaction

NH_3(g)+HCl(g)\rightarrow NH_4Cl(g)

b. HCl is the limiting reagent.

c. 7.3295 grams of ammonium chloride could form from the reaction mixture in part (b).

d. 0.6715 grams of ammonia is left over in the reaction mixture in part b.

Explanation:

a. The balanced chemical equation for the reaction

NH_3(g)+HCl(g)\rightarrow NH_4Cl(g)

b.

Moles of ammonia =\frac{3.0 g}{17 g/mol}=0.1765 mol

Moles of HCl = \frac{5.0 g}{36.5 g/mol}=0.1370 mol

According to reaction, 1 mole of HCl reacts with 1 mole of ammonia . Then 0.1370 moles of HCl will react with :

\frac{1}{1}\times 0.1370 mol=0.1370 mol of ammonia

Hence, HCl is the limiting reagent.

c.

Since, HCl is a limiting reagent amount of ammonium chloride will depend upon moles of HCl.

According to reaction, 1 mole of HCl gives with 1 mole of ammonium chloride . Then 0.1370 moles of HCl will give :

\frac{1}{1}\times 0.1370 mol=0.1370 mol of ammonium chloride

Mass of 0.1370 moles of ammonium chloride :

53.5 g/mol × 0.1370 mol =  7.3295 g

7.3295 grams of ammonium chloride could form from the reaction mixture in part (b).

d.

Moles of ammonia =\frac{3.0 g}{17 g/mol}=0.1765 mol

HCl is a limiting reagent and ammonia is an excessive reagent.

According to reaction, 1 mole of HCl reacts with 1 mole of ammonia . Then 0.1370 moles of HCl will react with :

\frac{1}{1}\times 0.1370 mol=0.1370 mol of ammonia

Moles of Ammonia reacted = 0.1370 mol

Moles of ammonia left unreacted = 0.1765 mol - 0.1370 mol = 0.0395 mol

Mass of 0.0395 moles of ammonia :

0.0395 mol × 17 g/mol = 0.6715 g

0.6715 grams of ammonia is left over in the reaction mixture in part b.

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solution:

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substitute the pH and Pka values in the formula.

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thus, the concentration ratio of the salt and acid should be equal to each other.

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3 years ago
The decomposition of N2O5 in solution in carbon tetrachloride proceeds via the reaction 2 N2O5(soln) → 4 NO2(soln) + O2(soln) Th
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<u>Answer:</u> The amount remained after 151 seconds are 0.041 moles

<u>Explanation:</u>

All the radioactive reactions follows first order kinetics.

Rate law expression for first order kinetics is given by the equation:

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Putting values in above equation, we get:

4.82\times 10^{-3}=\frac{2.303}{151}\log\frac{0.085}{[A]}

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7 0
3 years ago
Oxygen gas can be prepared by heating potassium chlorate according to the following equation:2KClO3(s)Arrow.gif2KCl(s) + 3O2(g)T
Eduardwww [97]

Answer:

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Explanation:

(a)

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Total vapor pressure = 748 mmHg

Vapor pressure of Oxygen gas = Total vapor pressure - Vapor pressure of water = (748 - 17.5) mmHg = 730.5 mmHg

To calculate the amount of Oxygen gas collected, we use the equation given by ideal gas which follows:

PV=nRT

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R = Gas constant = 62.3637\text{ L.mmHg }mol^{-1}K^{-1}

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Putting values in above equation, we get:

730.5mmHg\times 9.49L=n\times 62.3637\text{ L.mmHg }mol^{-1}K^{-1}\times 293K\\\\n=\frac{730.5\times 9.49}{62.3637\times 293}=0.3794mol

According to the reaction shown below as:-

2KClO_3(s)\rightarrow 2KCl(s) +3O_2(g)

3 moles of oxygen gas are produced when 2 moles of potassium chlorate undergoes reaction.

So,

0.3794 mol of oxygen gas are produced when \frac{2}{3}\times 0.3794 moles of potassium chlorate undergoes reaction.

<u>Moles of potassium chlorate reacted = 0.2529 moles</u>

(b)

We are given:

Vapor pressure of water = 17.5 mmHg

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Vapor pressure of Oxygen gas = Total vapor pressure - Vapor pressure of water = (753 - 17.5) mmHg = 735.5 mmHg

To calculate the amount of Oxygen gas collected, we use the equation given by ideal gas which follows:

PV=nRT

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n = number of moles of oxygen gas = ?

Putting values in above equation, we get:

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Putting values in above equation, we get:

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