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kramer
2 years ago
14

Question 8 helpppppp

Chemistry
2 answers:
Strike441 [17]2 years ago
6 0
<h2>Hey There!</h2><h2>_____________________________________</h2><h2>Answer:</h2><h2><u>LE CHATELIER PRINCIPLE</u>:</h2>

Le Chatelier's principle is a principle which predicts the effect of change in condition on a the position of a equilibrium.  

Change could be in Temperature, Moles(Concentration), Pressure.

-------------------------------------------------------------------------------------------------------------

<h2>EFFECTS ON EQUILIBRIUM</h2><h3 /><h3>__________________________________________________</h3><h3>Temperature: </h3>

We could change the temperature by increasing or decreasing it, and there are two types of reactions, endothermic or exothermic, both have different outcomes by changing the condition.

__________________________________________________________

In Endothermic,

When we increase the temperature, It will favor the formation of product thus MORE PRODUCT will be formed - equilibrium will shift towards right i.e. product side.

When we decrease the temperature, It will favor the formation of reactants thus MORE reactant will be formed - equilibrium will shift towards left i.e. reactants side.

__________________________________________________________

In Exothermic,

When we increase the temperature, It will favor the formation of reactants thus MORE REACTANT will be formed - equilibrium will shift towards left i.e. reactants side.

When we decrease the temperature, It will favor the formation of product thus MORE PRODUCT will be formed - equilibrium will shift towards the right i.e. product side

<h2>_____________________________________</h2><h3>Pressure:</h3>

When we increase the pressure, The equilibrium shifts towards the fewer moles of a gas. Wherever there are less moles, it could be any, reactant or product, the increase of Pressure will favor in formation of them.

When we decrease the pressure, The equilibrium shifts towards the more moles of a gas. So whether reactants or product have the higher moles, the decrease in pressure will favor in the formation of them.

<h2>_____________________________________</h2><h3>Concentration of moles:</h3>

When we increase the concentration of moles of any substance, The equilibrium will shift away from that substance. So if we want to make more product and there are more moles of reactant present, then Increase the concentration of reactants.

When we decrease the concentration of any substance, The equilibrium will shift towards that substance. So if we want to make more product, decrease its concentration or add more reactant.

<h2>_____________________________________</h2><h3>Catalyst:</h3>

By the use of the catalyst, There is no effect on the equilibrium. The rate of  both forward and backward reaction are increased with the equal amount.

<h2>_____________________________________</h2><h2>Question:</h2>

By keeping that in mind,

A) Extra NH_{3} will shift the equilibrium towards left i.e. more reactants will be formed.

B) Extra N2 is removed, the equilibrium will shift towards the left i.e. more reactants will be formed.

C) N2 is added, the equilibrium will shift towards right i.e. more PRODUCT will be formed. (I assumed there was a typing error and it meant Addition instead of removal)

D) When we decrease the pressure the equilibrium will shift towards the left i.e. more reactant will be formed.

E) Catalyst has no effect on the system

<h2>_____________________________________</h2><h2>Best Regards</h2><h2>'Borz'</h2><h2 />
solniwko [45]2 years ago
5 0

Answer:

Explanation:

This is lechatlier's principle, which basically talks about how adding or taking away things will disrupt equilibrium and the system will act a certain way to restore equilibrium

1. adding NH3 causes the equilibrium to shift left - produce more reactants

2. removing N2 causes the equilibrium to shift left - produce more reactants

3.  same as number 2

4. decreasing pressure causes equilbrium to shift to the side with more moles so it shifts left and produces more reactants

5. catalyst doesn't change anything about equlibrium, it only affects the reaction's rate

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Katyanochek1 [597]

All atoms are of <u>neutral charge, with an equal amount of protons and electrons.</u>

6 0
3 years ago
Read 2 more answers
Grady is doing an experiment about the solubility of sugar. He puts 100 milliliters of water in each of three beakers. He leaves
olga nikolaevna [1]

Grady is doing an experiment about the solubility of sugar. He puts 100 milliliters of water in each of three beakers. He leaves the first beaker at room temperature, heats the second beaker to 60°C, and heats the third beaker until the water boils at 100°C. The variable Grady change on  purpose in the experiment is the temperature of water in each beaker .

Variables in the experiment is the any factor that can exist in different types or amount. There are three types of variables: independent variable , dependent variable , controlled variable. The independent variable is the variable you changed in the experiment. dependent variable is that changes because of independent variable. the controlled variable is the constant one.

Thus, Grady is doing an experiment about the solubility of sugar. He puts 100 milliliters of water in each of three beakers. He leaves the first beaker at room temperature, heats the second beaker to 60°C, and heats the third beaker until the water boils at 100°C. The variable Grady change on  purpose in the experiment is the temperature of water in each beaker .

To learn more about variables here

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8 0
1 year ago
Force = 2.32 N<br> Acceleration = 0.19 m/s2<br> Mass= ?
Mkey [24]

mass = 12.2 kg

Explanation:

To find the mass we use the following formula (Newton's Second Law of Motion):

force = mass × acceleration

mass = force / acceleration

mass = 2.32 N / 0.19 m/s²

mass = 12.2 kg

Learn more about:

Newton's Second Law of Motion

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3 0
3 years ago
A certain gas is present in a 10.0 LL cylinder at 4.0 atmatm pressure. If the pressure is increased to 8.0 atmatm the volume of
ICE Princess25 [194]

Answer:

The gas obeys Boyle’s law and the value of k_i\&k_f both are equal to 40.0 atm L.

Explanation:

Initial volume of the gas = V_1=10.0 L

Initial pressure of the gas = P_1=4.0 atm

Final volume of the gas = V_2=5.0 L

Final pressure of the gas = P_2=8.0 atm

This law states that pressure is inversely proportional to the volume of the gas at constant temperature.  

PV=k

The equation given by this law is:

P_1V_1=P_2V_2

P_1\propto \frac{1}{V_1}

P_1V_1=k_i

k_i=4.0 atm\times 10.0 L = 40.0 atm L

P_2\propto \frac{1}{V_2}

P_V_2=k_f

k_f=8.0 atm\times 5.0 L = 40.0 atm L

k_i=k_f=40.0 atm L

The gas in the cylinder is obeying Boyle's law.

The gas obeys Boyle’s law and the value of k_i\&k_f both are equal to 40.0 atm L.

6 0
3 years ago
Three mixtures were prepared from three very narrow molar mass distribution polystyrene samples with molar masses of 10,000, 30,
8_murik_8 [283]

Answer:

(a). 46,666.7 g/mol; 78,571.4 g/mol

(b). 86950g/mol; 46,666.7 g/mol.

(c). 86950g/mol; 43,333.33 g/mol

Explanation:

So, we are given the molar masses for the three samples as: 10,000, 30,000 and 100,000 g mol−1.

Thus, the equal number of molecule in each sample = ( 10,000 + 30,000 + 100,000 ) / 3 = 46,666.7 g/mol.

The average molar mass = [ ( 10,000)^2 + (30,000)^2 + 100,000)^2] ÷ 10,000 + 30,000 + 100,000 = 78,571. 4 g/mol.

(b). The equal masses of each sample = 3/[ ( 1/ 10,000) + (1/30,000 ) + (1/100,000) ] = 20930.23 g/mol.

Average molar mass = ( 10,000 + 30,000 + 100,000 ) / 3 = 46,666.7 g/mol.

(c). Equal masses of the two samples = (0.145 × 10,000) + (0.855 × 100,000)/ 0.145 + 0.855 = 86950g/mol.

The weight average molar mass = 1.7 + 10,000 + 100,000/ 1.7 + 1 = 43,333.33 g/mol.

6 0
3 years ago
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