A chemist carefully measures the amount of heat needed to raise the temperature of a 894.0g sample of a pure substance from to −
1 answer:
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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.
<u>Answer:</u>
<em>When we finish, the temperature would be 32.5℃</em>
<em></em>
<u>Explanation:</u>
Density of water = mass/volume
So,
Mass of water = Density × Volume
where
= Final T - Initial T
Q is the heat energy in calories
c is the specific heat capacity (for water 1.0 cal/(g℃))
m is the mass of water
plugging in the values
Final T = ∆T + Initial T
= 7.5℃ + 25℃ = 32.5℃ (Answer).