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3 years ago

11

In the reaction between bromine and sodium, a bromine atom gains an electron and forms the bromide ion, Br-. What happens to bro

mine?

1 answer:

AlekseyPX3 years ago

6 0

It becomes ionized and attains its stable electronic configuration.

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PLZ HELP I WILL GIVE BRAINLY AND POINTS

max2010maxim [7]

Answer:

1. Define the problem

2. Conduct a literature search

3. Propose a hypothesis

4. Devise an experiment to prove or disprove

5. State conclusions

Explanation: In order to begin an experiment, you must first define a problem or question that you will be answering. Then you must research the problem in order to form a hypothesis, or an educated guess. Then you should devise and execute an experiment to answer your question. The conclusions that you draw will either prove or disprove your hypothesis. Hope this helps!

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2 years ago

What are some examples of supersaturated solutions? Give 10.

Phantasy [73]

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2 years ago

Does the following compound contain a polyatomic ion? Na2SO4<br> Yes<br> No

seropon [69]

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2 years ago

A certain reaction with an activation energy of 185 kJ/mol was run at 505 K and again at 525 K . What is the ratio of f at the h

frosja888 [35]

Answer:

The ratio of f at the higher temperature to f at the lower temperature is 5.356

Explanation:

Given;

activation energy, Ea = 185 kJ/mol = 185,000 J/mol

final temperature, T₂ = 525 K

initial temperature, T₁ = 505 k

Apply Arrhenius equation;

$Log(\frac{f_2}{f_1} ) = \frac{E_a}{2.303 \times R} [\frac{1}{T_1} -\frac{1}{T_2} ]$

Where;

$\frac{f_2}{f_1}$ is the ratio of f at the higher temperature to f at the lower temperature

R is gas constant = 8.314 J/mole.K

$Log(\frac{f_2}{f_1} ) = \frac{E_a}{2.303 \times R} [\frac{1}{T_1} -\frac{1}{T_2} ]\\\\Log(\frac{f_2}{f_1} ) = \frac{185,000}{2.303 \times 8.314} [\frac{1}{505} -\frac{1}{525} ]\\\\Log(\frac{f_2}{f_1} ) = 0.7289\\\\\frac{f_2}{f_1} = 10^{0.7289}\\\\\frac{f_2}{f_1} = 5.356$

Therefore, the ratio of f at the higher temperature to f at the lower temperature is 5.356

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3 years ago