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myrzilka [38]
3 years ago
5

Consider the following two equilibria and their respective equilibrium constants: (1) NO(g) + ½O2(g) NO2(g) (2) 2NO2(g) 2NO(g) +

O2(g) Which one of the following is the correct relationship between the equilibrium constants K1 and K2?
K2 = 1/(2 K1)

K2 = 2/K1

K2 = 1/(2K1)2

K2 = (1/K1)2

K2 = –K1/2
Chemistry
2 answers:
Brilliant_brown [7]3 years ago
8 0

Answer:

The fourth option is correct K2 = (1/K1)2

Explanation:

Step 1: Data given

(1) NO(g) + ½O2(g) ⇆ NO2(g)  

(2) 2NO2(g) ⇆ 2NO(g) + O2(g)

Step 2: Calculate K1

K1 = [NO2] / [NO][O2]^0.5

Step 3: Calculate K2

K2 = [NO]²[O2]/[NO2]²

Step 4: When we square the first equation

K1² = [NO2]² / [NO]²[O2]

Step 5: Calculate the reverse reaction

1/K1² = [NO]²[O2] / [NO2]² = K2

So K2 = 1/K1²  = 1²/K1²

The fourth option is correct K2 = (1/K1)2

leva [86]3 years ago
8 0

Answer:

The answer is K2 = (1/K1)2

Explanation:

For the first reaction:

NO + 1/2O₂ = NO₂

K_{1} =\frac{[NO_{2}] }{[NO][O_{2}]^{1/2}  }

For the second reaction:

2NO₂ = 2NO + O₂

K_{2} =\frac{[NO]^{2}[O_{2}]  }{[NO_{2}]^{2}  }=\frac{[NO][O_{2}]^{1/2}  }{[NO_{2}]^{2}  } =(\frac{1}{K_{1} } )^{2}

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7 0
1 year ago
An atom has radius of 227 pm and crystallizes in a body-centered cubic unit cell. What is the volume of the unit cell
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V = S^3 = (\frac{4}{\sqrt{3} }*227pm)^3

Solving that we get:

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1) How many bonds can Sr atom form?<br>a) 5<br>c) 3<br>b) 4<br>d) 2​
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5 0
3 years ago
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A container of oxygen with a fixed volume has a pressure of 13.0 atm at a temperature of 20 °C. What will the pressure of the ox
Norma-Jean [14]

Given:

P1 = 13.0 atm

T1 = 20 °C

T2 = 102 °C

Required:

P2 of oxygen

Solution:

At constant volume, we can apply Gay-Lussac’s law of pressure and temperature relationship

P1/T1=P2/T2

(13.0 atm) / (20 °C) = P2 / (102 °C)

P2 = 66.3 atm

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6 0
3 years ago
5. What concentration of acid must be added to change the pH of 1 mM phosphate buffer from 7.4 to 7.3 (pKas of the phosphate buf
mr_godi [17]

Explanation:

According to the Henderson-Hasselbalch equation, the relation between pH and pK_{a} is as follows.

               pH = pK_{a} + log \frac{base}{acid}

where,     pH = 7.4 and pK_{a} = 7.21

As here, we can use the pK_{a} nearest to the desired pH.

So,      7.4 = 7.21 + log \frac{base}{acid}

             0.19 = log \frac{base}{acid}

            \frac{base}{acid} = 1.55

1 mM phosphate buffer means [HPO_{4}] + [H_{2}PO_{4}] = 1 mM

Therefore, the two equations will be as follows.

           \frac{HPO_{4}}{H_{2}PO_{4}} = 1.55 ............. (1)

  [HPO_{4}] + [H_{2}PO_{4}] = 1 mM ........... (2)        

Now, putting the value of [HPO_{4}] from equation (1) into equation (2) as follows.

             1.55[H_{2}PO_{4}] + [tex][H_{2}PO_{4}] = 1 mM

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Putting the value of [H_{2}PO_{4}] in equation (1) we get the following.

                     0.392 mM + [HPO_{4}] = 1 mM

                          [HPO_{4}] = (1 - 0.392) mM

                              [HPO_{4}] = 0.608 mM

Thus, we can conclude that concentration of the acid must be 0.608 mM.

7 0
3 years ago
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