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UkoKoshka [18]
2 years ago
13

Item 4

Chemistry
1 answer:
Furkat [3]2 years ago
6 0

The statement that best describes a mixture is -

  • two or more substances that are mixed but can be separated back to their original form, maintaining their original properties.

Explanation:

A mixture is that form of matter in which two or more substances are simply mixed in any proportion and it can be separated back to their original form.

  • There are two types of Mixtures -
  1. Homogeneous Mixtures
  2. Heterogeneous Mixtures

<h2>___________________</h2>

In Homogeneous Mixtures, the composition is uniform throughout such as sugar in water , salt in water , sulphur in carbon disulphide , water and alcohol , whereas Heterogeneous Mixtures has non Uniform composition such as sand and salt , sugar and salt , wood , blood , water in soil etc.

  • Pure substance is a Homogeneous material which consists of a single type of particles atoms or molecules with definite set of properties.
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<span>Because as you add energy levels, the electrons are drawn to the nucleus of the atoms giving them a lesser charge. Thus its atomic size also increases. </span>

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... in neutralization reactions, for example:

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A solid reactant is placed into a beaker of a warm water. The liquid vigorously bubbles as the solid dissolves into the solution
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Fewer bubbles will be produced because of fewer collisions of reactant molecules

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As the solid dissolves into the solution after the liquid has been vigorously bubbled, if the temperature of the liquid is reduced a little, what will happen is that fewer bubbles will be produced as a result of lesser amount of collisions occurring between the reactant molecules

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3 years ago
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A student has a 2.19 L bottle that contains a mixture of O 2 , N 2 , and CO 2 with a total pressure of 5.57 bar at 298 K . She k
Sergeeva-Olga [200]

<u>Answer:</u> The partial pressure of oxygen gas is 2.76 bar

<u>Explanation:</u>

To calculate the number of moles, we use the equation given by ideal gas which follows:

PV=nRT

where,

P = pressure of the gas = 5.57 bar

V = Volume of the gas = 2.19 L

T = Temperature of the gas = 298 K

R = Gas constant = 0.0831\text{ L bar }mol^{-1}K^{-1}

n = Total number of moles = ?

Putting values in above equation, we get:

5.57bar\times 2.19L=n\times 0.0831\text{ L. bar }mol^{-1}K^{-1}\times 298K\\\\n=\frac{5.57\times 2.19}{0.0831\times 298}=0.493mol

To calculate the mole fraction of carbon dioxide, we use the equation given by Raoult's law, which is:

p_{A}=p_T\times \chi_{A}         ........(1)

where,

p_A = partial pressure of carbon dioxide = 0.318 bar

p_T = total pressure = 5.57 bar

\chi_A = mole fraction of carbon dioxide = ?

Putting values in above equation, we get:

0.318bar=5.57bar\times \chi_{CO_2}\\\\\chi_{CO_2}=\frac{0.381}{5.57}=0.0571

  • Mole fraction of a substance is given by:

\chi_A=\frac{n_A}{n_A+n_B}

We are given:

Moles of nitrogen gas = 0.221 moles

Mole fraction of nitrogen gas, \chi_{N_2}=\frac{0.221}{0.493}=0.448

Calculating the partial pressure of oxygen gas by using equation 1, we get:

Mole fraction of oxygen gas = (1 - 0.0571 - 0.448) = 0.4949

Total pressure of the system = 5.57 bar

Putting values in equation 1, we get:

p_{O_2}=5.57bar\times 0.4949\\\\p_{O_2}=2.76bar

Hence, the partial pressure of oxygen gas is 2.76 bar

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4 years ago
Explain why the first ionization energy K is less than that of Ca
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Answer:

The first ionization energy for K is less than Ca because Ca has a larger effective nuclear charge.

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