CHEMISTRY HIGH SCHOOL

in a second experiment, the total pressure is observed to be 58 atm. what is the partial pressure of the water vapor produced?

Answers

Answer 1

Answer:

The partial pressure exerted by a gas in a mixture, depends on the mole

fraction of the gas and the pressure exerted by the mixture.

The partial pressure of H₂O is 20 atm.

Reasons:

Given parameters are;

Explosion equation is 4C₃H₅N₃O₉ → 12CO₂(g) + O₂(g) + 6N₂(g) + 10H₂O(g)

Amount of nitroglycerine = 227 g

Molar mass of nitroglycerine = 227 g/mol

Required:

Partial pressure of the water vapor

Solution:

Number of moles of nitroglycerine in the reaction = 1 mole

Therefore;

Number of moles of CO₂ = 12/4 = 3 moles

Number of moles of O₂ = 0.25 moles

Number of nitrogen, N = 1.5 moles

Number of moles of H₂O = 2.5 moles

$Mole \ fraction \ of \ H_2O, \ X_(H_2O) = (2.5)/(2.5 + 1.5 + 0.25 + 3) = (10)/(29)$

According to Raoults law, we have;

The partial pressure of H₂O = $X_(H_2O) * P_$

Therefore, partial pressure of H₂O = $(10)/(29) * 58$ = 20 atm.

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Answer 2

Answer:

This is an incomplete question, here is a complete question.

Nitroglycerine (C₃H₅N₃O₉) explodes with tremendous force due to the numerous gaseous products. The equation for the explosion of Nitroglycerine is:

$4C_3H_5N_3O_9(l)\rightarrow 12CO_2(g)+O_2(g)+6N_2(g)+10H_2O(g)$

A scientist conducts an experiment to characterize a bomb containing nitroglycerine. She uses a steel, ridge container for the test.

Volume of rigid steel container: 1.00 L

Molar mass of Nitroglycerine: 227 g/mol

Temperature: 300 K

Amount of Nitroglycerine tested: 227 g

Value for ideal gas constant, R: 0.0821 L.atm/mol.K

In a second experiment, the total pressure is observed to be 58 atm. what is the partial pressure of the water vapor produced?

Answer : The partial pressure of the water vapor is, 20.01 atm

Explanation :

First we have to calculate the moles of $C_3H_5N_3O_9$

$\text{Moles of }C_3H_5N_3O_9=\frac{\text{Given mass }C_3H_5N_3O_9}{\text{Molar mass }C_3H_5N_3O_9}=(227g)/(227g/mol)=1mol$

Now we have to calculate the moles of $CO_2,O_2,N_2\text{ and }H_2O$

The balanced chemical reaction is:

$4C_3H_5N_3O_9(l)\rightarrow 12CO_2(g)+O_2(g)+6N_2(g)+10H_2O(g)$

From the balanced chemical reaction we conclude that,

As, 4 moles of $C_3H_5N_3O_9$ react to give 12 moles of $CO_2$

So, 1 moles of $C_3H_5N_3O_9$ react to give $(12)/(4)=3$ moles of $CO_2$

and,

As, 4 moles of $C_3H_5N_3O_9$ react to give 1 moles of $O_2$

So, 1 moles of $C_3H_5N_3O_9$ react to give $(1)/(4)=0.25$ moles of $O_2$

and,

As, 4 moles of $C_3H_5N_3O_9$ react to give 6 moles of $N_2$

So, 1 moles of $C_3H_5N_3O_9$ react to give $(6)/(4)=1.5$ moles of $N_2$

and,

As, 4 moles of $C_3H_5N_3O_9$ react to give 10 moles of $H_2O$

So, 1 moles of $C_3H_5N_3O_9$ react to give $(10)/(4)=2.5$ moles of $H_2O$

Now we have to calculate the mole fraction of water.

$\text{Mole fraction of }H_2O=\frac{\text{Moles of }H_2O}{\text{Moles of }H_2O+\text{Moles of }CO_2+\text{Moles of }O_2+\text{Moles of }N_2}$

$\text{Mole fraction of }H_2O=(2.5)/(2.5+3+0.25+1.5)=0.345$

Now we have to calculate the partial pressure of the water vapor.

According to the Raoult's law,

$p_(H_2O)=X_(H_2O)* p_T$

where,

$p_(H_2O)$ = partial pressure of water vapor gas = ?

$p_T$ = total pressure of gas = 58 atm

$X_(H_2O)$ = mole fraction of water vapor gas = 0.345

Now put all the given values in the above formula, we get:

$p_(H_2O)=X_(H_2O)* p_T$

$p_(H_2O)=0.345* 58atm=20.01atm$

Therefore, the partial pressure of the water vapor is, 20.01 atm

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The decomposition of ammonia gas (a process that occurs at high temps) is 2KH3(g) --> N2(g) 3H2(g). If a balloon was filled with 3.5L of ammonia gas and all of the gas decomposed, what would be the total volume of gas in the container? Assume the pressure and temp remains constant.

Answers

Ammonia gas is $\text{NH}_3$ .

Since the ammonia gas took up 3.5 L at first, using Avogadro's Law, we know that 2 mols of a gas took up 3.5 L at first, but now there are 4 mols of gas in total after the decomposition. Therefore, we can conclude that now the volume in total is 7 L.

Answer : The total volume of gas in the container will be, 7 liters

Explanation :

The given balanced chemical reaction is,

$2NH_3(g)\rightarrow N_2(g)+3H_2(g)$

From the balanced chemical reaction we conclude that

2 mole of ammonia gas decomposes to give 1 mole of nitrogen gas and 3 moles of hydrogen gas.

According to the Avogadro's Law, the volume of the gas is directly proportional to the number of moles of the gas at constant pressure and temperature.

$V\propto n$

or,

$(V_1)/(V_2)=(n_1)/(n_2)$

where,

$V_1$ = initial volume of ammonia gas = 3.5 L

$V_2$ = total volume of gas in the container = ?

$n_1$ = initial moles of ammonia gas = 2 mole

$n_2$ = final moles of all gas (nitrogen + hydrogen) = (1 + 3) = 4 moles

Now put all the given values in the above formula, we get the total volume of gas in the container.

$(3.5L)/(V_2)=(2mole)/(4mole)$

$V_2=7L$

Therefore, the total volume of gas in the container will be, 7 liters

If the isotope 32S has 16 protons and 16 neutrons, how many protons and how many neutrons will the isotope 35S have? 16pr and 19 ne 19pr and 16ne 18pr and 17ne or cannot be determined

Answers

Answer:

16 protons and 19 neutrons

To make the future development more eco-friendly and decrease soil erosion,choose one of the following recommendations:

Answers

Answer:

build better enclosures to decrease overgrazing by livestock.

Explanation:

In the thermal decomposition of copper carbonate, the black solid left behind weights less than the original copper carbonate . Why?

Answers

CuCO₃ ---T--> CuO↓ + CO₂ ↑

CO₂ escapes to the atmosphere (it's a gas)

It is so bcs of law of conservation of mass

A covalent bond in which electrons are shared unequally isa. polar.
b. a double bond.
c. ionic.
d. polyatomic.

Answers

Covalentbonds = sharing of electrons between two atoms of the same elements or elementsclose to each other on the periodic table. Usually they are metals sometimesnon-metals. In polar bonds electrons areshared unequally. Non polar bonds share electrons equally.

Final answer:

A covalent bond where electrons are shared unequally is known as a polar bond. This unequal sharing occurs due to differences in electronegativity between the two atoms involved in the bond.

Explanation:

A covalent bond in which electrons are shared unequally is defined as a polar bond. This corresponds to option a) polar. This occurs because one atom is more electronegative and pulls the shared electron pair towards its nucleus making the bond polar, having a partial positive and partial negative end. Option b) a double bond, refers to a covalent bond where two pairs of electrons are shared between atoms. Option c) ionic refers to a bond where electrons are completely transferred from one atom to another and option d) polyatomic refers to a molecule that consists of more than two atoms.

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Name the following compound: 2-ethyl-4-methylheptene 3,5-dimethyl-2-octene 2-ethyl-4-methylheptane 3-methyl-5-propyl-2-hexene

Answers

Answer:

3,5-dimethyl-2-octene

Explanation:

The parent chain will be choosen based on the highest value. In this case, if we count from top to bottom, we'll get seven carbon, however if we count from the second carbon, going left and then down, we'll get eight carbon. So the parent chain is octene

The double bond is located at the second carbon and the methyl groups are located on carbon 3 & 5. Since there are two methyl groups, we add di- in front of methyl to indicate two methyl groups present.

Note: The functional group has to be prioritise and it needed to be a part of the parent chain. In this case, the functional group is the double bond. (alkene)

Final answer:

The compounds are named as 2-ethyl-4-methylheptene, 3,5-dimethyl-2-octene, 2-ethyl-4-methylheptane and 3-methyl-5-propyl-2-hexene based on the IUPAC nomenclature rules for organic compounds.

Explanation:

The compounds presented in your question are named based on the rules of the International Union of Pure and Applied Chemistry (IUPAC), which are used for organic compounds. Here are their names:

2-ethyl-4-methylheptene - This is a heptene with methyl and ethyl groups on the 2nd and 4th carbon atoms.
3,5-dimethyl-2-octene - This is an octene with two methyl groups on the 3rd and 5th carbon atoms.
2-ethyl-4-methylheptane - This is a heptane with ethyl and methyl groups on the 2nd and 4th carbon atoms.
3-methyl-5-propyl-2-hexene - This is a hexene with a methyl group on the 3rd carbon atom and a propyl group on the 5th carbon atom.

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