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3 years ago

What are the products when ammonia (NH3) decomposes according to this equation? NH3

1 answer:

7 0

<span>Ammonia (NH3) is the combination of Nitrogen and Hydrogen elements.
=> N2 + 3H2 => 2NH3

Ammonia is basically used as a fertilizer. It is a gas composed of nitrogen and hydrogen. It is colorless with strong odor. Here are some other uses of Ammonia aside from fertilizer:
=> used by manufacturer to produce synthetic fiber
=> Used in metallurgical process
Ammonia can be decomposed easily and it produce hydrogen that is very convenient in welding.
Ammonia’s boiling point is -28.03 F and freezing point is -107.8F.

</span>

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Locate the element zinc (Zn) on the periodic table. How many protons does an atom of zinc contain? How many electrons does an at

Lady bird [3.3K]

<h2>Answer:</h2><h3>Part 1:</h3>

Location the element zinc (Zn) on the periodic table:

Group number : 12
Period number : 4
Block : d block
Element : Transition elements.

Protons in an atom of Zn: 30

Electrons in a Zn atom: 30

Neutron in an atom of Zn: 35

<h3 />

4 0

3 years ago

Read 2 more answers

How many moles of co2 are produced when 5.70 mol of ethane are burned in an excess of oxygen

sweet-ann [11.9K]

I believe the answer is 6

4 0

3 years ago

Ethylenediamine (en) forms an octahedral complex with Ni2+(aq) with the formula [Ni(en)3]2+. Ni2+(aq) + 3 en ⇌ [Ni(en)3]2+(aq) K

yawa3891 [41]

Answer:

$3.125\times 10^{-19} mol/L$ is the concentration of $Ni^{2+}(aq)$ in the solution.

Explanation:

$Ni^{2+}(aq) + 3 en\rightleftharpoons [Ni(en)_3]^{2+}(aq)$

Concentration of nickel ion = $[Ni^{2+}]=x$

Concentration of nickel complex= $[[Ni(en)_3]^{2+}]=\frac{0.16 mol}{2 L}=0.08 mol/L$

Concentration of ethylenediamine = $[en]=\frac{0.80 mol}{2 L}=0.40 mol/L$

The formation constant of the complex = $K_f=4.0\times 10^{18}$

The expression of formation constant is given as:

$K_f=\frac{[[Ni(en)_3]^{2+}]}{[Ni^{2+}][en]^3}$

$4.0\times 10^{18}=\frac{0.08 mol/L}{x\times (0.40 mol/L)^3}$

$x=\frac{0.08 mol/L}{4.0\times 10^{18}\times (0.40 mol/L)^3}$

$x=3.125\times 10^{-19} mol/L$

$3.125\times 10^{-19} mol/L$ is the concentration of $Ni^{2+}(aq)$ in the solution.

6 0

3 years ago

What is the law of multiple proportions?

quester [9]

Answer:

I think

(d) All compounds contain the same elements in the same properties

6 0

3 years ago

When 25.0 g of ch4 reacts completely with excess chlorine yielding 45.0 g of ch3cl, what is the percentage yield, according to c

Ber [7]

Taking into account definition of percent yield, the percent yield for the reaction is 57.08%.

<h3>Reaction stoichiometry</h3>

In first place, the balanced reaction is:

CH₄ + Cl₂ → CH₃Cl + HCl

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

CH₄: 1 mole
Cl₂: 1 mole
CH₃Cl: 1 mole
HCl: 1 mole

The molar mass of the compounds is:

CH₄: 16 g/mole
Cl₂: 70.9 g/mole
CH₃Cl: 50.45 g/mole
HCl: 36.45 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

CH₄: 1 mole ×16 g/mole= 16 grams
Cl₂: 1 mole ×70.9 g/mole= 70.9 grams
CH₃Cl: 1 mole ×50.45 g/mole= 50.45 grams
HCl: 1 mole ×36.45 g/mole= 36.45 grams

Mass of CH₃Cl formed

The following rule of three can be applied: if by reaction stoichiometry 16 grams of CH₄ form 50.45 grams of CH₃Cl, 25 grams of CH₄ form how much mass of CH₃Cl?

$mass of CH_{3} Cl=\frac{25 grams of CH_{4}x 50.45grams of CH₃Cl }{16 grams of CH_{4}}$

<u><em>mass of CH₃Cl= 78.83 grams</em></u>

Then, 78.83 grams of CH₃Cl can be produced from 25 grams of CH₄.

<h3>Percent yield</h3>

The percent yield is the ratio of the actual return to the theoretical return expressed as a percentage.

The percent yield is calculated as the experimental yield divided by the theoretical yield multiplied by 100%:

$percent yield=\frac{actual yield}{theorical yield}x100$

where the theoretical yield is the amount of product acquired through the complete conversion of all reagents in the final product, that is, it is the maximum amount of product that could be formed from the given amounts of reagents.

Percent yield for the reaction in this case

In this case, you know: