Answer:
In general, the energy needed to remove an electron (the ionization energy) increases as the atomic number increases across a period.
Explanation:
Each additional proton increases the attraction between the nucleus and the electron.
Thus, it takes more energy to remove an electron as you add extra protons.
Answer: The energy of activation for the chirping process is 283.911 kJ/mol
Explanation:
According to the Arrhenius equation,
The expression used with catalyst and without catalyst is,
![\log (\frac{K_2}{K_1})=\frac{Ea}{2.303\times R}[\frac{1}{T_1}-\frac{1}{T_2}]](https://tex.z-dn.net/?f=%5Clog%20%28%5Cfrac%7BK_2%7D%7BK_1%7D%29%3D%5Cfrac%7BEa%7D%7B2.303%5Ctimes%20R%7D%5B%5Cfrac%7B1%7D%7BT_1%7D-%5Cfrac%7B1%7D%7BT_2%7D%5D)
where,
= rate of reaction at 
= 194/min
= rate of reaction at 
= 47.6 /min
= activation energy
R = gas constant = 8.314 J/Kmol
tex]T_1[/tex] = initial temperature = 
tex]T_1[/tex] = final temperature = 
Now put all the given values in this formula, we get
![\frac{194}{47.6}=\frac{E_a}{2.303\times 8.314}[\frac{1}{278}-\frac{1}{301}]](https://tex.z-dn.net/?f=%5Cfrac%7B194%7D%7B47.6%7D%3D%5Cfrac%7BE_a%7D%7B2.303%5Ctimes%208.314%7D%5B%5Cfrac%7B1%7D%7B278%7D-%5Cfrac%7B1%7D%7B301%7D%5D)
Thus the energy of activation for the chirping process is 283.911 kJ/mol
Answer:
709 g
Step-by-step explanation:
a) Balanced equation
Normally, we would need a balanced chemical equation.
However, we can get by with a partial equation, as log as carbon atoms are balanced.
We know we will need an equation with masses and molar masses, so let’s <em>gather all the information</em> in one place.
M_r: 30.07 236.74
C₂H₆ + … ⟶ C₂Cl₆ + …
m/g: 90.0
(i) Calculate the moles of C₂H₆
n = 90.0 g C₂H₆ × (1 mol C₂H₆ /30.07 g C₂H₆)
= 2.993 mol C₂H₆
(ii) Calculate the moles of C₂Cl₆
The molar ratio is (1 mol C₂Cl₆/1 mol C₂H₆)
n = 2.993 mol C₂H₆ × (1 mol C₂Cl₆/1 mol C₂H₆)
= 2.993 mol C₂Cl₆
(iii) Calculate the mass of C₂Cl₆
m = 2.993 mol C₂Cl₆ × (236.74 g C₂Cl₆/1 mol C₂Cl₆)
m = 709 g C₂Cl₆
The reaction produces 709 g C₂Cl₆.
