CHEMISTRY HIGH SCHOOL

What is the most abundant gas in Earth's present day atmosphere?methane
oxygen
carbon dioxide
nitrogen

Answers

Answer 1
Answer: nitrogen. air consists 78% of nitrogen gas
Answer 2
Answer:

The answer is nitrogen

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Answers

the first one is the correct answer

Answer:

1s2 2s2 2p6 3s2 3p2

Explanation:

you're welcome

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

Answers

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.

Learn more here:

brainly.com/question/10165688

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

How many grams of acetylene react if 1.10 mol of CO2 are produced?

Answers

 Combustion of acetylene :

molar mass acetylene ( C₂H₂ ) = 26.0 g/mol and CO₂ = 44.0 g/mol

2 C₂H₂ + 5 O₂ ---> 4 CO₂ + 2 H₂O

2 moles C₂H₂ --------> 4 moles CO₂
? moles C₂H₂ --------> 1.10 moles CO₂

moles C₂H₂ = 1.10 * 2  / 4

moles C₂H₂ = 0.55 moles of C₂H₂

Mass acetylene:

m = n * mm

m = 0.55 * 26.0

m = 14.3 g

hope this helps!

Which is a molecule?
A. Ne
B. NaCL
C. Trail Mix
D. graphene

Answers

B) NaCl is a molecule.

A soccer balll is travelling at a velcrocity of 50ms the kinetic energy of the ball is 500 what is the mass of the soccer ball

Answers

KE = mv²/2

m=2*KE/v²

v=50 m/s

KE=500J

m=2*KE/v² =2*500/50²=1000/2500= 0.4 kg

Ack please help on this problem

Answers

Answer:

Only the oxygen needs to be balanced. There are equal numbers of hydrogen and carbon

Explanation:

 Given expression:

     C₂H₄ + O₂ → 2H₂O + 2CO₂

The law of conservation of mass suggests that chemical equations be balanced since atoms are neither created nor destroyed in the course of a chemical reaction. In retrospect, bonds are broken and chemical species are change to another form.

 From the given equation, only oxygen is not balanced. This flouts the law of conservation.

 On the reactant side, we have 2 oxygen on the product, we have 6.

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