Answer:
Some of the things, are extremly toxic to life
like nuculear power plants, create nuculear waste
you need to let it sit there for several years
unless if you want to get sued by the Enviromental protection agency
Explanation:
Factors that increases reaction rate such as increase in concentration or pressure will reduce reaction time whereas factors that decrease reaction rate such as inhibitors will increase reaction time.
<h3>What are the factors that affect reaction rate?</h3>
Factors that affect reaction rate are those factors which increase or decrease the rate of chemical reaction.
The factors that affect reaction rate include:
- temperature
- concentration/pressure
- catalysts
- surface area
- nature of substance
Any factor that increases reaction rate such as increase in concentration or pressure will reduce reaction time whereas factors that decrease reaction rate such as inhibitors will increase reaction time.
Learn more about factors affecting reaction rate at: brainly.com/question/14817541
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Carbon's molar mass is 12gm
Oxygen's molar mass is 16gm
So CO2 molar mass is 44gm
Hence 1mol of CO2 contains 44gm
There 1/4mol of CO2 contains 44/4=11gm.
Hope it helps
Answer: The value of 
for the half-cell reaction is 0.222 V.
Explanation:
Equation for solubility equilibrium is as follows.
Its solubility product will be as follows.
![K_{sp} = [Ag^{+}][Cl^{-}]](https://tex.z-dn.net/?f=K_%7Bsp%7D%20%3D%20%5BAg%5E%7B%2B%7D%5D%5BCl%5E%7B-%7D%5D)
Cell reaction for this equation is as follows.
Reduction half-reaction: 
, 
Oxidation half-reaction: 
, 
= ?
Cell reaction: 
So, for this cell reaction the number of moles of electrons transferred are n = 1.
Solubility product,
= 
Therefore, according to the Nernst equation
![E_{cell} = E^{o}_{cell} - \frac{0.0592 V}{n} log \frac{[AgCl]}{[Ag^{+}][Cl^{-}]}](https://tex.z-dn.net/?f=E_%7Bcell%7D%20%3D%20E%5E%7Bo%7D_%7Bcell%7D%20-%20%5Cfrac%7B0.0592%20V%7D%7Bn%7D%20log%20%5Cfrac%7B%5BAgCl%5D%7D%7B%5BAg%5E%7B%2B%7D%5D%5BCl%5E%7B-%7D%5D%7D)
At equilibrium, 
= 0.00 V
Putting the given values into the above formula as follows.
![0.00 = E^{o}_{cell} - \frac{0.0592 V}{1} log \frac{1}{[Ag^{+}][Cl^{-}]}](https://tex.z-dn.net/?f=0.00%20%3D%20E%5E%7Bo%7D_%7Bcell%7D%20-%20%5Cfrac%7B0.0592%20V%7D%7B1%7D%20log%20%5Cfrac%7B1%7D%7B%5BAg%5E%7B%2B%7D%5D%5BCl%5E%7B-%7D%5D%7D)
= 
= 0.577 V
Hence, we will calculate the standard cell potential as follows.
= 0.222 V
Thus, we can conclude that value of for the half-cell reaction is 0.222 V.
The answer is B) fills all the space in its container
