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KiRa [710]
3 years ago
5

Consider the equation: 2NO(0) - N.04(). Using ONLY the information given by the equation which of the following

Chemistry
2 answers:
ratelena [41]3 years ago
7 0

Answer:

By increasing the pressure, the molar concentration of  N2O4 will increase

Explanation:

We have the equation 2NO2 ⇔ N2O4

This equation is reversible and exotherm. By <u>decreasing the temperature</u>, the reaction will produce more energy, so the reaction will move to the right.  But a lower temperature also lowers the rate of the process, so, the temperature is set at a compromise value that allows N2O4 to be made at a reasonable rate with an equilibrium concentration that is not too unfavorable

So <u>increasing the temperature</u> will shift the equilibrium to the left. The equilibrium shifts in the direction that consumes energy.

If we d<u>ecrease the concentration of NO2</u>, the equilibrium will shift to the left, resulting in forming more reactants.

To increase the molar concentration of the product N2O4, we have to <u>increase the pressure</u> of the system.

NO2 takes up more space than N2O4, so increasing the pressure would allow the reactant to collide more form more product.

By increasing the pressure, the molar concentration of  N2O4 will increase

ipn [44]3 years ago
5 0

<u>Answer:</u>

<em>5) Increase the pressure</em>

<em></em>

<u>Explanation:</u>

2NO_2 (g)N_2 O_4 (g)   \\\\\Delta H=-58 KJ per mol

In a chemical reaction, equilibrium is the state in which the rate of the forward reaction is equal to the rate of the reverse reaction.  A system will remain in equilibrium unless it is stressed or disturbed.  Le Chatelier’s Principle states that <em>“when a stress is placed on a system at equilibrium, the system will shift to offset the stress applied”. </em>

Equilibrium always shifts away from the increase and towards the decrease.

The equation here shows us that forward reaction is exothermic since ∆H is negative and backward or reverse reaction is endothermic.

Increasing the temperature will shift the equilibrium in favour of the endothermic reaction.

Decreasing the temperature will shift the equilibrium in favour of exothermic reaction.

Increasing the Pressure towards the side with lesser number of gaseous moles

Decreasing the Pressure towards the  side with more number of gaseous moles.

Increasing the concentration of the substance favour the equilibrium shift away from the substance

Decreasing the concentration of the substance favour the  equilibrium shift towards the substance.

2NO_2 (g)N_2 O_4 (g) \Delta H is not given

Since delta H is not given we can rule out options 1 and 3. Decreasing the concentration of NO favours equilibrium shift towards the left side so N_2 O_4 is not produced in greater amount.

So, taking into pressure conditions,

Left side contains 2 moles and right side contains 1 mole.

Increasing the Pressure will shift the equilibrium towards the lesser number of moles that is right side producing more of N_2 O_4.

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unit that contains two or more atoms covalently bonded together but that has an overall charge is called a(n) _____ ion. Many __
OverLord2011 [107]

Answer:

polyatomic, ionic

Explanation:

unit that contains two or more atoms covalently bonded together but that has an overall charge is called a(n) polyatomic ion. Many ionic compounds contain such units.

3 0
2 years ago
What data should be plotted to show that experimental concentration data fits a first-order reaction? A) 1/[reactant] vs. time B
natita [175]

Answer:

C) In[reactant] vs. time

Explanation:

For a first order reaction the integrated rate law equation is:

A = A_{0}e^{-kt}

where A(0) = initial concentration of the reactant

A = concentration after time 't'

k = rate constant

Taking ln on both sides gives:

ln[A] = ln[A]_{0}-kt

Therefore a plot of ln[A] vs t should give a straight line with a slope = -k

Hence, ln[reactant] vs time should be plotted for a first order reaction.

7 0
3 years ago
10 points. Please help.
ratelena [41]

Answer:

-191.7°C

Explanation:

P . V = n . R . T

That's the Ideal Gases Law. It can be useful to solve the question.

We replace data:

2.5 atm . 8 L = 3 mol . 0.082 L.atm/mol.K . T°

(2.5 atm . 8 L) / (3 mol . 0.082 L.atm/mol.K) = T°

T° = 81.3 K

We convert T° from K to C°

81.3K - 273 = -191.7°C

6 0
3 years ago
Read 2 more answers
The solubility of oxygen gas in water at 40 ∘c is 1.0 mmol/l of solution. What is this concentration in units of mole fraction?
juin [17]

The formula for mole fraction is:

mole fraction of solute = \frac{number of moles of solute}{total number of moles of solution}    -(1)

The solubility of oxygen gas = 1.0 mmol/L  (given)

1.0 mmol/L means 1.0 mmol are present in 1 L.

Converting mmol to mol:

1.00 mmol\times \frac{1 mol}{1000 mmol} = 0.001 mol

So, moles of oxygen = 0.001 mol

For moles of water:

1 L of water = 1000 mL of water

Since, the density of water is 1.0 g/mL.

Density = \frac{mass}{volume}

Mass = 1.0 g/ml\times 1000 mL = 1000 g

So, the mass of water is 1000 g.

Molar mass of water = 18 g/mol.

Number of moles of water = \frac{1000 g}{18 g/mol} = 55.55 mol

Substituting the values in formula (1):

mole fraction = \frac{0.001}{55.55+0.001}

mole fraction = 1.8\times 10^{-5}

Hence, the mole fraction is 1.8\times 10^{-5}.

7 0
3 years ago
A solution with a hydrogen ion concentration of 3.25 × 10-2 m is ________ and has a hydroxide concentration of _______
Romashka-Z-Leto [24]

To know the acidity of a solution, we calculate the pH value. The formula for pH is given as:

<span>pH = - log [H+]            where H+ must be in Molar</span>

We are given that H+ = 3.25 × 10-2 M

Therefore the pH is:

pH = - log [3.25 × 10-2] 

pH = 1.488

Since pH is way below 7, therefore the solution is acidic.

 

To find for the OH- concentration, we must remember that the product of H+ and OH- is equivalent to 10^-14. Therefore,

[H+]*[OH-] = 10^-14 <span>
</span>[OH-] = 10^-14 / [H+]

[OH-] = 10^-14 / 3.25 × 10-2

[OH-] = 3.08 × 10-13 M

 

Answers:

Acidic

[OH-] = 3.08 <span>× 10-13 M</span>

6 0
3 years ago
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