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charle [14.2K]
3 years ago
10

For the equilibrium 2 NOBr(g) D 2 NO(g) + Br2(g), Kc = 1.56 ´ 10-3 at 300 K. Suppose 0.400 M NOBr is placed in a reaction vessel

at 300 K. At a given point, the concentration of Br2 is 0.0134 M. Which of the following statements is true? The value of K will decrease until it is equal to Q. Q < K so the reaction will continue to make more products. Q > K so the reaction will consume products to make more reactants. The value of K will increase until it is equal to Q. Q = K so the system is at equilibrium.
Chemistry
1 answer:
kicyunya [14]3 years ago
5 0

Explanation:

2 NOBr(g) ⇄ 2 NO(g) + Br2(g)

Kc = 1.56 ´ 10-3

Which of the following statements is true?

The reaction quotient (Q) measures the relative amounts of products and reactants present during a reaction at a particular point in time. The Q value can be compared to the Equilibrium Constant, K, to determine the direction of the reaction that is taking place.

- The value of K will decrease until it is equal to Q: This statement is wrong.

Equilibrium constants are not changed if you change the concentrations of things present in the equilibrium. The only thing that changes an equilibrium constant is a change of temperature.

- Q < K so the reaction will continue to make more products.

If Q<K, then the reaction favors the products. the system shifts to the RIGHT to make more products. This statement is true.

- Q > K so the reaction will consume products to make more reactants.

If Q>K, then the reaction favors the reactants. the system shifts to the LEFT to make more reactants. This statement is true.

- The value of K will increase until it is equal to Q: This statement is wrong.

Equilibrium constants are not changed if you change the concentrations of things present in the equilibrium. The only thing that changes an equilibrium constant is a change of temperature.

- Q = K so the system is at equilibrium: This statement is true.

If Q=K, then the reaction is already at equilibrium. There is no tendency to form more reactants or more products at this point. No side is favored and no shift occurs.

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Answer:

A

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3 years ago
A 200.0mL closed flask contains 2.000mol of carbon monoxide gas and 2.000mol of oxygen gas at the temperature of 300.0K. How man
max2010maxim [7]

Answer:

There will react 0.400 moles of oxygen.

Explanation:

<u>Step 1:</u> Data given

Volume of the closed flask = 200.00 mL = 0.2 L

Number of moles of CO = 2.000 mol

Number of moles of O2 = 2.000 mol

Temperature = 300.0 K

Pressure decreases with 10%

<u>Step 2</u>: The balanced equation

2CO(g)+O2(g)⟶2CO2(g)

<u>Step 3</u>: Calculate the initial pressure of the flask before the reaction

P = nRT/V

⇒ with n = the number of moles (2.000 moles CO + 2.000 moles O2 = 4.000 moles)

⇒ R is gas constant (0.08206 atm*L/mol*K)

⇒T = the  temperature = 300.0K

⇒ V = the volume = 200.0 mL = 0.2 L

P = (4 * 0.08206*300)/0.2

P = 492.36 atm

<u>Step 4:</u> When the pressure is 10 % decreased:

The final pressure = 492.36 - 49.236 = 443.124 atm

<u>Step 5:</u> Calculate the number of moles

n = PV/RT

⇒ with n = the number of moles

⇒ with P = the pressure = 443.124 atm

⇒ V = the volume = 200.0 mL = 0.2 L

⇒ R is gas constant (0.08206 atm*L/mol*K)

⇒T = the  temperature = 300.0K

n =(443.124*0.2)/(0.08206*300)

n = 3.6 moles = total number of moles

<u>Step 6:</u> Calculate number of moles

For the reaction :2CO(g) + O₂(g) ⟶ 2CO₂(g)

For each mole of O2 we have 2 moles of CO, to produce 2 moles of CO2

Moles CO = (2 -2X) moles

Moles O2 = (2-X) moles

Moles CO2 = 2X

The total number of moles (4 -X)= 3.6 moles

Where X are moles that react

X = 0.400 moles

There will react 0.400 moles of oxygen.

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3 years ago
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sukhopar [10]
Gay-Lussac's law gives the relationship between pressure and temperature of a gas.
it states that for a fixed amount of gas of constant volume pressure is directly proportional to temperature. 
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temperature should be in the kelvin scale,
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substituting the values in the equation 
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Hoi!! 

its true
 
hope this help!!
:) np


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