Answer:
Here's what I get
Explanation:
1. Balanced equation
HQ⁻ + CH₃-Br ⟶ HQ-CH₃ + Br⁻
(I must use HQ because the Brainly Editor thinks the O makes a forbidden word)
2. Mechanism
HQ⁻ + CH₃-Br ⟶[HQ···CH₃···Br]⁻⟶ HQ-CH₃ + Br⁻
A C B
The hydroxide ion attacks the back side of the carbon atom in the bromomethane (A).
At the same time as the Q-H bond starts to form, the C-Br bond starts to break.
At the half-way point, we have a high-energy intermediate (C) with partially formed C-O and C-Br bonds.
As the reaction proceeds further, the Br atom drops off to form the products — methanol and bromide ion (B).
3. Energy diagram
See the diagram below.
Answer: The value of 
for the reaction is, -2512.4 kJ
Explanation:
The chemical equation for the combustion of acetylene follows:
The equation for the enthalpy change of the above reaction is:
![\Delta H^o_{rxn}=[(3\times \Delta H^o_f_{(CO_2(g))})+(4\times \Delta H^o_f_{(H_2O(g))})]-[(1\times \Delta H^o_f_{(C_2H_2(g))})+(5\times \Delta H^o_f_{(O_2(g))})]](https://tex.z-dn.net/?f=%5CDelta%20H%5Eo_%7Brxn%7D%3D%5B%283%5Ctimes%20%5CDelta%20H%5Eo_f_%7B%28CO_2%28g%29%29%7D%29%2B%284%5Ctimes%20%5CDelta%20H%5Eo_f_%7B%28H_2O%28g%29%29%7D%29%5D-%5B%281%5Ctimes%20%5CDelta%20H%5Eo_f_%7B%28C_2H_2%28g%29%29%7D%29%2B%285%5Ctimes%20%5CDelta%20H%5Eo_f_%7B%28O_2%28g%29%29%7D%29%5D)
We are given:
Putting values in above equation, we get:
![\Delta H^o_{rxn}=[(4\times (-393.5))+(2\times (-241.8))]-[(2\times (227.4)+(5\times (0))]\\\\\Delta H^o_{rxn}=-2512.4kJ](https://tex.z-dn.net/?f=%5CDelta%20H%5Eo_%7Brxn%7D%3D%5B%284%5Ctimes%20%28-393.5%29%29%2B%282%5Ctimes%20%28-241.8%29%29%5D-%5B%282%5Ctimes%20%28227.4%29%2B%285%5Ctimes%20%280%29%29%5D%5C%5C%5C%5C%5CDelta%20H%5Eo_%7Brxn%7D%3D-2512.4kJ)
Therefore, the value of for the reaction is, -2512.4 kJ
Explanation:
The given data is as follows.
T = 
= (120 + 273.15)K = 393.15 K,
As it is given that it is an equimolar mixture of n-pentane and isopentane.
So, 
= 0.5 and 
= 0.5
According to the Antoine data, vapor pressure of two components at 393.15 K is as follows.
(393.15 K) = 9.2 bar
(393.15 K) = 10.5 bar
Hence, we will calculate the partial pressure of each component as follows.
= 
= 4.6 bar
and, 
= 
= 5.25 bar
Therefore, the bubble pressure will be as follows.
P = 
= 4.6 bar + 5.25 bar
= 9.85 bar
Now, we will calculate the vapor composition as follows.
= 
= 0.467
and, 
= 
= 0.527
Calculate the dew point as follows.
= 0.5, 
= 0.5
= 0.101966 
P = 9.807
Composition of the liquid phase is 
and its formula is as follows.
= 
= 0.5329
= 
= 0.467
Answer : 
Explanation : When diatomic hydrogen gas and diatomic nitrogen gas reacts spontaneously it forms ammonia gas as the product.
we will have the following reactions; As all the reactants and products are in the gaseous state the subscript (g) is given to the molecules.
But this is not a balanced equation, as on the right side of reactants we have 2 hydrogen atoms and 2 nitrogen atoms which gives the product which has one nitrogen and three hydrogen in the compound state.
So, balancing the equation, we get,
We multiplied 2 with the diatomic hydrogen molecule which resulted in production of 2 moles of ammonia as the product.
So, the complete balanced equation is;
Answer: Lead(II) nitrate but idk the rest
Explanation:
