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3 years ago

Using this reversible reaction, answer the following:

Chemistry

2 answers:

spin [16.1K]3 years ago

4 0

<span>-Products formed by the forward
reaction may react with each other to regenerate the reactants.
-When reactants are mixed, they will begin to react at a forward reaction rate particular to that chemical reaction.
- As reactants are depleted and products are formed, however, the rate of the forward reaction begins to slow, and the rate of the reverse reaction begins to increase.</span>

Mamont248 [21]3 years ago

4 0

<h2>Question 1.</h2><h3>Answer:</h3>

The concentration of [N2O4] will decrease.

<h3>Explanation:</h3>

As the reverse reaction which is the formation of N2O4 is an exothermic reaction and the formation of NO2 is an endothermic reaction.
Hence heating will favor the forward reaction and stops the reverse reaction.
N2O4 --> 2NO2
So the concentration of N2O4 decreases.

<h2>Question: 2.</h2><h3>Answer:</h3>

The formation of the products is favored by the addition of heat.

<h3>Explanation:</h3>

As the reverse reaction which is the formation of N2O4 is an exothermic reaction and the formation of NO2 is an endothermic reaction.
So the addition of heat will favor endothermic reaction.
Hence the formation of NO2 will be favored which is a product.

<h2>Question no.4:</h2><h3>Answer:</h3>

The reverse reaction is an exothermic reaction.

N2O4 <-- 2NO2.

<h3>Explanation:</h3>

N2O4 which is a reactant in this reaction is colorless compound.
Its breakdown absorbs energy and its formation release energy in form of heat.
So the reverse reaction which releases energy is an exothermic reaction.

<h2>Question no. 4</h2><h3>Answer:</h3>

The correct option is D which is N2O4 <--> 2NO2, HR = -14 kcal.

<h3>Explanation:</h3>

Enthalpy is the change in energy in reactants and products.
It is actually the difference in energies of products and reactant.
As the enthalpy change from left to right, it means reactants have internal energy 14 kcal high than products and it will be released.
And in option D which is shown as HR = -14 kcal.

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I have no idea pls help ty 11 points

Yanka [14]

Happy Holidays! :)

$\large\boxed{\text{Water.}}$

Looking at the information given in the description, the experiment is testing for the effects of the different salts on the growth of the plants.

This means that the type of salt is the independent variable, or the variable being manipulated and tested.

To ensure fair results, some parts of the experiment would need to be kept the same, which is the control. The only answer choice that makes sense in this instance is A. water.

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3 years ago

Read 2 more answers

The osmotic pressure of a solution containing 2.04 g of an unknown compound dissolved in 175.0 mLof solution at 25 ∘C is 2.13 at

kherson [118]

<u>Answer:</u> The molecular formula of the compound is $C_4H_{10}O_4$

<u>Explanation:</u>

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

$\pi=iMRT$

Or,

$\pi=i\times \frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}\times RT$

where,

$\pi$ = osmotic pressure of the solution = 2.13 atm

i = Van't hoff factor = 1 (for non-electrolytes)

Given mass of compound = 2.04 g

Volume of solution = 175.0 mL

R = Gas constant = $0.0821\text{ L atm }mol^{-1}K^{-1}$

T = temperature of the solution = $25^oC=[273+25]=298K$

Putting values in above equation, we get:

$2.13atm=1\times \frac{2.04\times 1000}{\text{Molar mass of compound}\times 175.0}\times 0.0821\text{ L.atm }mol^{-1}K^{-1}\times 298K\\\\\text{Molar mass of compound}=\frac{1\times 2.04\times 1000\times 0.0821\times 298}{2.13\times 175.0}=133.9g/mol$

<u>Calculating the molecular formula:</u>

The chemical equation for the combustion of compound having carbon, hydrogen and oxygen follows:

$C_xH_yO_z+O_2\rightarrow CO_2+H_2O$

where, 'x', 'y' and 'z' are the subscripts of carbon, hydrogen and oxygen respectively.

We are given:

Mass of $CO_2=36.26g$

Mass of $H_2O=14.85g$

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

<u>For calculating the mass of carbon:</u>

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 36.26 g of carbon dioxide, $\frac{12}{44}\times 36.26=9.89g$ of carbon will be contained.

<u>For calculating the mass of hydrogen:</u>

In 18 g of water, 2 g of hydrogen is contained.

So, in 14.85 g of water, $\frac{2}{18}\times 14.85=1.65g$ of hydrogen will be contained.

Mass of oxygen in the compound = (22.08) - (9.89 + 1.65) = 10.54 g

To formulate the empirical formula, we need to follow some steps:

<u>Step 1:</u> Converting the given masses into moles.

Moles of Carbon = $\frac{\text{Given mass of Carbon}}{\text{Molar mass of Carbon}}=\frac{9.89g}{12g/mole}=0.824moles$

Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{1.65g}{1g/mole}=1.65moles$

Moles of Oxygen = $\frac{\text{Given mass of oxygen}}{\text{Molar mass of oxygen}}=\frac{10.54g}{16g/mole}=0.659moles$

<u>Step 2:</u> Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.659 moles.

For Carbon = $\frac{0.824}{0.659}=1.25\approx 1$

For Hydrogen = $\frac{1.65}{0.659}=2.5$

For Oxygen = $\frac{0.659}{0.659}=1$

Converting the mole fraction into whole number by multiplying the mole fraction by '2'

Mole fraction of carbon = (1 × 2) = 2

Mole fraction of oxygen = (2.5 × 2) = 5

Mole fraction of hydrogen = (1 × 2) = 2

<u>Step 3:</u> Taking the mole ratio as their subscripts.

The ratio of C : H : O = 2 : 5 : 2

The empirical formula for the given compound is $C_2H_5O_2$

For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.

The equation used to calculate the valency is:

$n=\frac{\text{Molecular mass}}{\text{Empirical mass}}$

We are given:

Mass of molecular formula = 133.9 g/mol

Mass of empirical formula = 61 g/mol

Putting values in above equation, we get:

$n=\frac{133.9g/mol}{61g/mol}=2$

Multiplying this valency by the subscript of every element of empirical formula, we get:

$C_{(2\times 2)}H_{(5\times 2)}O_{(2\times 2)}=C_4H_{10}O_4$

Hence, the molecular formula of the compound is $C_4H_{10}O_4$

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3 years ago

Calculate the percent dissociation of benzoic acid C6H5CO2H in a 2.4mM aqueous solution of the stuff. You may find some useful d

Musya8 [376]

Answer:

34%

Explanation:

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3 years ago

What is the source of energy for the Sun?

nikitadnepr [17]

Answer:

Nuclear fusion

Explanation:

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3 years ago

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bulgar [2K]

Answer:

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