Answer:
6.5x10⁻³M = [OH⁻]
Explanation:
The Kb of a Weak base as ethylamine is expressed as follows:
Kb = [OH⁻] [C₂H₅NH₃⁺] / [C₂H₅NH₂]
As the equilibrium of ethylenamine is:
C₂H₅NH₂(aq) + H₂O(l) ⇄ C₂H₅NH₃⁺(aq) + OH(aq)
The concentration of C₂H₅NH₃⁺(aq) + OH(aq) is the same because both ions comes from the same equilibrium. Thus, we can write:
Kb = [OH⁻] [C₂H₅NH₃⁺] / [C₂H₅NH₂]
6.4x10⁻⁴ = [X] [X] / [C₂H₅NH₂]
Also, we can assume the concentration of ethylamine doesn't decrease. Replacing:
6.4x10⁻⁴ = [X] [X] / [0.066M]
4.224x10⁻⁵ = X²
6.5x10⁻³M = X
<h3>6.5x10⁻³M = [OH⁻]</h3>
Answer:
The answer would be tundra.
A rain forest has a lot of humidity because it rains a lot otherwise it wouldn't be called a rain forest.
Grassland has a somewhat high temperature and average humidity enough to keep it green and grassy hence grasslands.
A wetland has a lot of water but low temperatures. Still, humidity is water so wetlands aren't it.
Explanation:
Hope this helped.
A brainliest is always appreciated.
Im pretty sure that the current will increase so the answer is A . Hope that helps
Answer:
The change in entropy of gas is 
Explanation:
n= Number of moles of gas
Change in entropy of gas = 
From the given,
Let "T" be the initial temperature.
Therefore, The change in entropy of gas is
Answer : The amount of heat required is, 
Solution :
The process involved in this problem are :
The expression used will be:
![\Delta H=[m\times c_{p,s}\times (T_{final}-T_{initial})]+m\times \Delta H_{fusion}+[m\times c_{p,l}\times (T_{final}-T_{initial})]+m\times \Delta H_{vap}+[m\times c_{p,g}\times (T_{final}-T_{initial})]](https://tex.z-dn.net/?f=%5CDelta%20H%3D%5Bm%5Ctimes%20c_%7Bp%2Cs%7D%5Ctimes%20%28T_%7Bfinal%7D-T_%7Binitial%7D%29%5D%2Bm%5Ctimes%20%5CDelta%20H_%7Bfusion%7D%2B%5Bm%5Ctimes%20c_%7Bp%2Cl%7D%5Ctimes%20%28T_%7Bfinal%7D-T_%7Binitial%7D%29%5D%2Bm%5Ctimes%20%5CDelta%20H_%7Bvap%7D%2B%5Bm%5Ctimes%20c_%7Bp%2Cg%7D%5Ctimes%20%28T_%7Bfinal%7D-T_%7Binitial%7D%29%5D)
where,
= heat required for the reaction
m = mass of ice = 10.0 g
= specific heat of solid water or ice = 
= specific heat of liquid water = 
= specific heat of gaseous water = 
= enthalpy change for fusion = 
= enthalpy change for vaporization = 
Now put all the given values in the above expression, we get:
![\Delta H=[10.0g\times 2.09J/g^oC\times (0-(-20))^oC]+10.0g\times 333J/g+[10.0g\times 4.18J/g^oC\times (100-0)^oC]+10.0g\times 2260J/g+[10.0g\times 2.03J/g^oC\times (120-100)^oC]](https://tex.z-dn.net/?f=%5CDelta%20H%3D%5B10.0g%5Ctimes%202.09J%2Fg%5EoC%5Ctimes%20%280-%28-20%29%29%5EoC%5D%2B10.0g%5Ctimes%20333J%2Fg%2B%5B10.0g%5Ctimes%204.18J%2Fg%5EoC%5Ctimes%20%28100-0%29%5EoC%5D%2B10.0g%5Ctimes%202260J%2Fg%2B%5B10.0g%5Ctimes%202.03J%2Fg%5EoC%5Ctimes%20%28120-100%29%5EoC%5D)
Therefore, the amount of heat required is,
