The picture looks blurry can you tell me what it says?
Answer:
1. NO and Br₂
2. 77
3. 8.8
Explanation:
Let's consider the following reaction.
2 NO(g) + Br₂(g) ⇄ 2 NOBr(g)
The equilibrium constant for this reaction is:
![Kc_{1}=\frac{[NOBr]^{2}}{[NO]^{2}[Br_{2}]} =1.3 \times 10^{-2}](https://tex.z-dn.net/?f=Kc_%7B1%7D%3D%5Cfrac%7B%5BNOBr%5D%5E%7B2%7D%7D%7B%5BNO%5D%5E%7B2%7D%5BBr_%7B2%7D%5D%7D%20%3D1.3%20%5Ctimes%2010%5E%7B-2%7D)
1. At this temperature does the equilibrium favor NO and Br₂, or does it favor NOBr?
Since Kc₁ < 1, the reactants are favored, that is, NO and Br₂.
2. Calculate Kc for 2 NOBr(g) ⇄ 2 NO(g) + Br₂(g)
The equilibrium constant is:
![Kc_{2}=\frac{[NO]^{2}[Br_{2}]}{[NOBr]^{2}} =\frac{1}{Kc_{1}} =77](https://tex.z-dn.net/?f=Kc_%7B2%7D%3D%5Cfrac%7B%5BNO%5D%5E%7B2%7D%5BBr_%7B2%7D%5D%7D%7B%5BNOBr%5D%5E%7B2%7D%7D%20%3D%5Cfrac%7B1%7D%7BKc_%7B1%7D%7D%20%3D77)
3. Calculate Kc for NOBr(g) ⇄ NO(g) + 1/2 Br₂(g)
The equilibrium constant is:
![Kc_{3}=\frac{[NO][Br_{2}]^{1/2} }{[NOBr]} =\sqrt{\frac{[NO]^{2}[Br_{2}]}{[NOBr]^{2}}} =\sqrt{Kc_{2}} =8.8](https://tex.z-dn.net/?f=Kc_%7B3%7D%3D%5Cfrac%7B%5BNO%5D%5BBr_%7B2%7D%5D%5E%7B1%2F2%7D%20%7D%7B%5BNOBr%5D%7D%20%3D%5Csqrt%7B%5Cfrac%7B%5BNO%5D%5E%7B2%7D%5BBr_%7B2%7D%5D%7D%7B%5BNOBr%5D%5E%7B2%7D%7D%7D%20%3D%5Csqrt%7BKc_%7B2%7D%7D%20%3D8.8)
<span>Potassium bromate is a bleaching / elasticity agent which is legally used in breads in the United States. It has been banned in Canada, China, and the EU due to concerns about its potential links to several health issues including: kidney damage, nervous system damage, cancer, thyroid issues and gastrointestinal distress.</span>
Which of the following statements is generally true about change in the workplace ? a ) Most people accept change easily . b) Smart companies can avoid change altogether. c) Change in the workplace fairly infrequently d) Individuals can learn to manage the change in their lives.
Answer:
28 g/mol, N2
Explanation:
Given data:
Volume of gas = 5.0 L
Mass of gas = 6.3 g
Pressure = 1 atm
Temperature = 273 K
Molar mass of gas = ?
Solution:
We will calculate the density first.
d = mass/ volume
d = 6.3 g/ 5.0 L
d = 1.26 g/L
Molar mass:
d = PM/RT
M = dRT/P
M = 1.26 g/L× 0.0821 atm.L/mol.K × 273 K/ 1 atm
M = 28 g/mol
Molar mass of N₂ is 28 g/mol thus given gas is N₂.
