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Deffense [45]
4 years ago
13

The 3 principles of the kinetic theory

Chemistry
1 answer:
jekas [21]4 years ago
5 0

Answer:

There are three main components to kinetic theory: No energy is gained or lost when molecules collide. The molecules in a gas take up a negligible (able to be ignored) amount of space in relation to the container they occupy.

Explanation:

If I helped please mark as brainliest

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In the Haber process, nitrogen (N2) and hydrogen (H2) are directly combined to form ammonia (NH3). Which illustration contains t
Over [174]
The following illustration <span>contains the stoichiometric quantities of the reactants for this reaction.

</span><span>In the Haber process, nitrogen (N2) and hydrogen (H2) are directly combined to form ammonia (NH3). </span><span>The reaction is as follows :

 N</span>N_{2} + 3 H_{2} = 2NH_{3}

Therefore, 1 mole of nitrogen is equivalent to 3 moles of Hydrogen

6 0
4 years ago
Calculate the maximum volume in ml of 0.15M HCl that each of the following antacid formulations would be expected to neutralize.
vlada-n [284]

a. 34 mL; b. 110 mL

a. A tablet containing 150 Mg(OH)₂


Mg(OH)₂ + 2HCl ⟶ MgCl₂ + 2H₂O


<em>Moles of Mg(OH)₂</em> = 150 mg Mg(OH)₂ × [1 mmol Mg(OH)₂/58.32 mg Mg(OH)₂

= 2.572 mmol Mg(OH)₂


<em>Moles of HCl</em> = 2.572 mmol Mg(OH)₂ × [2 mmol HCl/1 mmol Mg(OH)₂]

= 5.144 mmol HCl


Volume of HCl = 5.144 mmol HCl × (1 mmol HCl/0.15 mmol HCl) = 34 mL HCl


b. A tablet containing 850 mg CaCO₃


CaCO₃ + 2HCl ⟶ CaCl₂ + CO₂ + H₂O


<em>Moles of CaCO₃</em> = 850 mg CaCO₃ × [1 mmol CaCO₃/100.09 mg CaCO₃

= 8.492 mmol CaCO₃


<em>Moles of HCl</em> = 8.492 mmol CaCO₃ × [2 mmol HCl/1 mmol CaCO₃]

= 16.98 mmol HCl


Volume of HCl = 16.98 mmol HCl × (1 mL HCl/0.15 mmol HCl) = 110 mL HCl


5 0
3 years ago
A = ε l c. (a) Define the terms in the formula: A = ε l c. (Pick your answers using the letter of the correct definition.)
VladimirAG [237]

Explanation:

Using Beer-Lambert's law :

Formula used :

A=\epsilon \times c\times l

where,

A = absorbance of solution

c = concentration of solution

l = length of the cell

\epsilon = molar absorptivity of this solution

According to question:

A = (C) : absorbance measured by the spectrometer

c = (B) : concentration, in mol/L, of the stock solution from which the sample was made

l = (A): pathlength of light through the cell

ε =  (D) : molar absorptivity, a constant unique to that substance at that wavelength

7 0
3 years ago
Please please help me solve this, I have a test and only 20 mins left T-T<br>​
Ann [662]

Answer: 5.6dm^3[/tex[ of gas is produced when 0.1 moles of magnesium nitrate is decomposed.Explanation:The balanced chemical equation is:&#10;[tex]2NH_4NO_3(s)\rightarrow 2MgO(s)+4NO_2(g)+O_2(g)

According to stoichiometry :

2 moles of NH_4NO_3 produce = 4 moles of NO_2 gas and 1 mole of O_2 gas

2 moles of NH_4NO_3 produce = 5 moles of gas

Thus 0.1 mole of NH_4NO_3 produce =\frac{5}{2}\times 0.1=0.25moles  of gas

Volume of gas produced = moles\times {\text {Molar volume}}=0.25moles\times 22.4dm^3/mol=5.6dm^3

Thus [tex]5.6dm^3[/tex[ of gas is produced when 0.1 moles of magnesium nitrate is decomposed.

7 0
3 years ago
How many protons, neutrons, and electrons are in Potassium, Nitrogen, and oxygen?
pickupchik [31]
<span>The amount of protons is equal to the number of electrons of a chemical element. The atomic number of an element also determines the number of the protons it contains. The number of protons is also the same number of electrons. Protons are positively charged, electrons are negatively charged. To get the number of neutrons, all you need is to deduct the number of  the atomic mass or mass number from the atomic number. Potassium has 19 protons, therefore has 19 electrons as well. The atomic mass of Potassium is 39. So, the number of neutrons Potassium has is 20. </span> Potassium Atomic number: 19 Protons: 19 Electrons: 19 Atomic Mass: 39 Neutron: 20 Nitrogen Atomic number: 7 Protons: 7 Electrons: 7 Atomic Mass: 14.007 Neutrons: 7 Oxygen Atomic Number: 8 Protons: 8 Electrons: 8 Atomic Mass: 15.99 Neutrons: 8



3 0
3 years ago
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