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Chemistry High School

$A mixture of N2, O2 and He have mole fractions of 0.25, 0.65, and 0.10,$

A mixture of N2, O2 and He have mole fractions of 0.25, 0.65, and 0.10, respectively. What is the pressure of N2 if the total pressure of the mixture is 3.9 atm?

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Solution 1

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The pressure of nitrogen in the mixture has been 0.975 atm.

Partial pressure has been defined as the pressure exerted by the gas molecules in the mixture. The partial pressure ( $P_A$ ) has been expressed as:

$P_A=X_A\;\times\;P$

Where, Mole fraction of the element A, $X_{N_2}=0.25\;\rm atm$

The total pressure of the mixture, $P=3.9\;\rm atm$

Substituting the values, the pressure of nitrogen ( $P_{\rm N_2}$ ),

$P_{\rm N_2}=0.25\;\times\;3.9\;\rm atm\\ \textit P_{N_2}=0.975\;atm$

The pressure of nitrogen in the mixture has been 0.975 atm.

For more information about mole fraction, refer to the link:

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Solution 2

Guest #2270213

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Answer:

Partia pressure N₂ → 0.975 atm

Explanation:

Let's analyse the moles fractions:

N₂ → 0.25

O₂ → 0.65

He → 0.1

Partial pressure / Total pressure = Mole fraction

Partial pressure N₂ / 3.9 atm = Mole fraction N₂

Partial pressure N₂ / 3.9 atm = 0.25

Partial pressure N₂ = 3.9 atm . 0.25 → 0.975 atm

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Solution 1

Answer:

The answer is (B) A gamma ray alone

Explanation:

Technetium-99m decays through a process called isomeric transition involving the decay of 99mTc to 99TC via the release of gamma rays and low energy electron

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Many classic experiments have given us indirect evidence of the nature of the atom. Which of the experiments listed below did not give the results described? A. The Rutherford experiment proved the Thomson "plum-pudding" model of the atom to be essentially correct. B. The Rutherford experiment was useful in determining the nuclear charge on the atom. C. Millikan's oil-drop experiment showed that the charge on any particle was a simple multiple of the charge on the electron. D. The electric discharge tube proved that electrons have a negative charge. E. All of the above experiments gave the results described.

Solution 1

Answer:

Option A, The Rutherford experiment proved the Thomson "plum-pudding" model of the atom to be essentially correct.

Explanation:

Thomson's plum pudding model:

Plum pudding model was proposed by J.J Thomson. In Thomson's model, atoms are proposed as sea of positively charge in which electrons are distributed through out.

Result of Rutherford experiment:

As per Rutherford's experiment:

Most of the space inside the atom is empty.

Positively charge of the atom are concentrated in the centre of the atom known as nucleus.

Electrons are present outside the nucleus and revolve around it.

As it is clear that, result of Rutherford experiment did not supported the Thomson model.

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For action potential generation and propagation, are there any other cation channels that could substitute for the voltage-gated sodium channels if the sodium channels were blocked?

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Yes, calcium ions.

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Solution 1

Answer:

In 7.80 g of styrene, we have 3.60×10²³ atoms of H

Explanation:

Empirical formula of styrene is CH

Molecular formula of styrene is C₈H₈

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104.14 g (1 mol of C₈H₈) have 8 moles of H

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Question

Why is pure orange juice a mixture?

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Question

Physical properties such as melting point, boiling point, and solubility are all dependent on the type of interparticle forces a substance experiences. Identify the type of interparticle force that has the greatest influence on the physical properties for each substance. Cl2, NH2OH, PCl3, CH4, CaCl2, KI Two of the substances in Part 1 are ionic. Which factors will result in a stronger ionic bond overall? 1. larger ions2. greater absolute charges3. similarity of ionic sizes4. smaller ions

Solution 1

1) The type of interparticle force that has the greatest influence on the physical properties for each substance is;

CaCl2 and KI; ionic bonding

CaCl2 and KI; ionic bondingPCl3 and CH4; dispersion forces

CaCl2 and KI; ionic bondingPCl3 and CH4; dispersion forcesNH2OH; hydrogen bonding

2) The factor that will result in a stronger ionic bond overall is; Smaller ions

1) We want to Identify the type of interparticle force that has the greatest influence on the physical properties for each substance. Let us look at the options;

For CaCl2 and KI, the elements Calcium and Potassium that form the chloride are metals and as such they form ionic bonds with the halogens Chlorine and Iodine. Thus, ionic bonding has the greatest force here.

For PCl3 and CH4, they possess forces that are dispersive and as such their structural arrangement distribute electrons to any surrounding atoms and molecules. Thus, the forces of dispersion have the greatest force here.

For NH2OH, as a result of the presence of Hydrogen (H) and Oxygen(O) atoms, the bond present in it will be a hydrogen bond. Thus hydrogen bond has the greatest force here.

2) Bond strength, depends largely on the charges present on each ion as well as the distance between each ion. Thus, it means ions that are Small and highly charged will form stronger bonds while ions that are large, minimally charged will form bonds that are weak.

Thus, smaller ions results in stronger ionic bond overall.

Read more at; brainly.com/question/23530058

Solution 2

Answer: CaCl2 and KI- ionic

PCl3 and CH4-dispersion forces

NH2OH- hydrogen bonding

Part B

Smaller ions.

Explanation:

The smaller the ions the easier it is for them to be packed into a well ordered crystal lattice. The strength of ionic interaction always depend on the relative ion sizes. The smaller the ions the stronger the bond. Large ions do not easily pack into crystal lattices.

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Solution 1

Answer:

Mg₃N₂ + 6H₂O → 2NH₃ + 3Mg(OH)₂

Coefficient of water is 6 (option 3)

Explanation:

The reaction is:

Mg₃N₂ + H₂O → NH₃ + Mg(OH)₂

Let's balance the reaction.

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If He gas has an average kinetic energy of 4310 J/mol under certain conditions, what is the root mean square speed of O2 gas molecules under the same conditions? (given that He and O_2 gas are at the same temperature what can you conclude about 0_2's average kinetic energy?) variable equations used to find the solution are greatly appreciated!!!

Solution 1

Answer:

The root mean square speed of O2 gas molecules is

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O2 = 32/1000 = 0.032 Kg/mol

First calculate the temperature at which the K.E of He is 4310J/mol

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Now , Use Vrms to calculate the velocity of O2

$v_{rms}=\sqrt{\frac{3(8.314J/Kmol)(345.60K)}{0.032Kg/mol}}$

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Solution 1

Answer : The diatomic gas is nitrogen gas, N₂.

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First we have to calculate the moles of gas.

Using ideal gas equation:

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V = Volume of gas = 4.4 L

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Answer:

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Thus, the correct answer is option (A).

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