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Debora [2.8K]
3 years ago
13

PLEASE HELP ASAP!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!

Chemistry
2 answers:
iogann1982 [59]3 years ago
8 0

2. is point source

3. is non point source

storchak [24]3 years ago
4 0
QUESTION 2: POINT SOURCE
QUESTION 3:NONE POINT SOURCE
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Consider the following reaction at a high temperature. Br2(g) ⇆ 2Br(g) When 1.35 moles of Br2 are put in a 0.780−L flask, 3.60 p
UNO [17]

Answer : The equilibrium constant K_c for the reaction is, 0.1133

Explanation :

First we have to calculate the concentration of Br_2.

\text{Concentration of }Br_2=\frac{\text{Moles of }Br_2}{\text{Volume of solution}}

\text{Concentration of }Br_2=\frac{1.35moles}{0.780L}=1.731M

Now we have to calculate the dissociated concentration of Br_2.

The balanced equilibrium reaction is,

                              Br_2(g)\rightleftharpoons 2Br(aq)

Initial conc.         1.731 M      0

At eqm. conc.      (1.731-x)    (2x) M

As we are given,

The percent of dissociation of Br_2 = \alpha = 1.2 %

So, the dissociate concentration of Br_2 = C\alpha=1.731M\times \frac{1.2}{100}=0.2077M

The value of x = 0.2077 M

Now we have to calculate the concentration of Br_2\text{ and }Br at equilibrium.

Concentration of Br_2 = 1.731 - x  = 1.731 - 0.2077 = 1.5233 M

Concentration of Br = 2x = 2 × 0.2077 = 0.4154 M

Now we have to calculate the equilibrium constant for the reaction.

The expression of equilibrium constant for the reaction will be :

K_c=\frac{[Br]^2}{[Br_2]}

Now put all the values in this expression, we get :

K_c=\frac{(0.4154)^2}{1.5233}=0.1133

Therefore, the equilibrium constant K_c for the reaction is, 0.1133

7 0
3 years ago
What will determine the number of moles in a sample
julsineya [31]

Answer:

weigh it and divide the weight by the molecular weight. :) good luck!!

Explanation:

3 0
3 years ago
Read 2 more answers
A mixture of gases at a total pressure of 95 kPa contains N₂, CO₂, and O₂. The partial pressure of the CO₂ is 24 kPa and the par
Zinaida [17]

Answer:

23 kPa = Partial pressure O₂

Explanation:

In a mixture of gases, the sum of partial pressure of each gas that contains the mixture = Total pressure

Total pressure = Partial pressure N₂ + Partial pressure CO₂ + Partial pressure O₂

95 kPa = 48 kPa + 24 kPa + Partial pressure O₂

95 kPa - 48 kPa - 24 kPa = Partial pressure O₂

23 kPa = Partial pressure O₂

7 0
3 years ago
Consider the substances hydrogen (H2), fluorine (F2), and hydrogen fluoride (HF). Based on their molecular structures, how does
katovenus [111]

Answer:

The boiling point of HF is <u><em>higher than</em></u> the boiling point of H2, and it is <u><em>higher than</em></u> the boiling point of F2.

Explanation:

In HF, inter- molecule forces will be present between the hydrogen and fluorine atoms. There will be hydrogen bonding present among the hydrogen and fluorine atoms. Hydrogen bonds are strong bonds and hence the boiling point for HF would be high as much energy will be required to break these bonds.

H2 and F2 will only have intra-molecular attractions and there will be no hydrogen bonds present in them. As a result, their boiling point will be lower.

3 0
3 years ago
The atomic mass is equal to what?​
dsp73

Answer:

The mass number

Explanation:

I hope this helps.

4 0
3 years ago
Read 2 more answers
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