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koban [17]
3 years ago
10

Why is there a need for increased recycling to preserve phosphorus? (20 points) What technique was used to measure the availabil

ity of phosphorus for plants in sewage sludge? (15 points) What is a disadvantage of using thermally conditioned sewage
Chemistry
1 answer:
erastovalidia [21]3 years ago
3 0

Answer 1) : The phosphorus minerals deposits that are currently available is not enough for the future, and the distribution of the ores are also uneven throughout the globe. The major part of food production are also dependent on the production of phosphorus. Phosphorus is also widely used as fertilizer and most of the population of farmers are dependent on it. This has increased the need to preserve and save the phosphorus.


Answer 2) : To measure the current availability of phosphorus found in plants of thermally conditioned sewage sludge, phosphorus radiotracer technique was used and the present amount of phosphorus was determined. A study of experiment in ryegrass was done in pots whcih were filled with soil that underwent isotopic P-labelling, and no fertilizer was added, thermally conditioned sewage sludge as fertilizer. Then shoot and roots were harvested at definite fixed intervals, and their radioactivity was analyzed to measure phosphorus uptake.


Answer 3) : Although there is no major disadvantage of using thermally conditioned sewage sludge as a fertilizer but they incur a great cost on their maintenance and operation, along with this they produce strong odors which is not possible to get rid off, they also generate large amount of liquor waste; handling and safe disposal of that is quite difficult. Continuous physical conditioning has to be given.

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If the equilibrium constant for the reaction A 2B C 5/2 D has a value of 4.0, what is the value of the equilibrium constant for
nirvana33 [79]

Answer:

K'=\frac{1}{16}

Explanation:

Hello!

In this case, since the given reaction is:

A+ 2B \rightleftharpoons C+ \frac{5}{2} D

Whereas the equilibrium constant is:

K=\frac{[C][D]^{5/2}}{[A][B]^2} =4.0

However, the new target reaction reverses and doubles the initial reaction to obtain:

2C+5D \rightleftharpoons 2A+4B

Whereas the equilibrium constant is:

K'=\frac{[A]^2[B]^4}{[C]^2[D]^5}

Which suggest the following relationship between the equilibrium constants:

K'=\frac{1}{K^2}

So we plug in to obtain:

K'=\frac{1}{4.0^2}\\\\K'=\frac{1}{16}

Best regards!

8 0
3 years ago
The rate of decomposition of N2O5 in CCl4 at 317 K has been studied by monitoring the concentration of N2O5 in the solution. 2 N
pav-90 [236]

Answer:

Average rate of reaction is 0.000565 M/min

Explanation:

Applying law of mass action for the given reaction:

Average rate = -\frac{1}{2}\frac{[N_{2}O_{5}]}{\Delta t}=\frac{1}{4}\frac{\Delta [NO_{2}]}{\Delta t}=\frac{\Delta [O_{2}]}{\Delta t}

Where, -\frac{1}{2}\frac{[N_{2}O_{5}]}{\Delta t} represents average rate of disappearance of N_{2}O_{5}, \frac{1}{4}\frac{[NO_{2}]}{\Delta t} represents average rate of appearance of NO_{2} and \frac{[O_{2}]}{\Delta t} represents average rate of appearance of O_{2}

Here,-\frac{[N_{2}O_{5}]}{\Delta t} = -\frac{(2.16-2.36)}{(177-0)}M/min=0.00113M/min

So average rate of reaction = [tex]-\frac{1}{2}\frac{[N_{2}O_{5}]}{\Delta t}[/tex] = \frac{1}{2}\times (0.00113M/min)=0.000565M/min

7 0
3 years ago
Which type of bond creates a crystalline structure?
Vaselesa [24]
Ionic bond is the bond that creates a crystalline structure
7 0
4 years ago
The gas release during a chemical reaction which causes fizzing known as?
IrinaVladis [17]

Answer:

Hey mate...

Explanation:

This is ur answer....

<h3>Effervescence</h3>

<em>Effervescence is the escape of gas from an aqueous solution and the foaming or fizzing that results from that release.</em>

Hope it helps!

Brainliest pls!

Follow me! ♧

8 0
3 years ago
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What might happen to an organism if its habitat could not meet one of its needs?
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The organism could adapt over time and find another way to satisfy this need, it could move to a new location, or the organism could eventually die off.
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