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Marianna [84]
3 years ago
13

Pls help I will give brainpower to who ever. Helps

Chemistry
2 answers:
Tju [1.3M]3 years ago
7 0

Answer: im pretty sure it is A but i might be wrong

Explanation:

trasher [3.6K]3 years ago
4 0

Answer:

Their identity changes in both Reaction A and Reaction B.

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PlEASE HELP MEEEE ASAP 50 PTS
Over [174]

In the given reaction potassium metal is placed in water and when a reactive metal is placed in water, it reacts with water to form metal hydroxide and hydrogen gas, as a result, potassium hydroxide and hydrogen gas are produced in the reaction. A redox reaction is a reaction in which a substance is oxidized during the reaction whereas some other substance is reduced during the reaction, simultaneously.

The given chemical reaction is:

2K(s) + 2H20(l) arrow 2KOH(aq) + H2(g)

Hope it Helps! Please mark as Brainliest!

8 0
3 years ago
All matter on earth contains energy
Dafna11 [192]
Yes; every object has energy and you cannot create or destroy energy but you can transfer it. 
6 0
3 years ago
What is the approximate total number of atoms in 1.0 mole of lithium?
chubhunter [2.5K]

Answer:

6.0 x 10 to the power of 23

6 0
3 years ago
2. Consider the reaction 2NO(g) + O2(g) → 2NO2(g) Suppose that at a particular moment during the reaction nitric oxide (NO) is r
vredina [299]

Answer :

(a) The rate of NO_2 formed is, 0.066 M/s

(b) The rate of O_2 formed is, 0.033 M/s

Explanation : Given,

\frac{d[NO]}{dt} = 0.066 M/s

The balanced chemical reaction is,

2NO(g)+O_2(g)\rightarrow 2NO_2(g)

The rate of disappearance of NO = -\frac{1}{2}\frac{d[NO]}{dt}

The rate of disappearance of O_2 = -\frac{d[O_2]}{dt}

The rate of formation of NO_2 = \frac{1}{2}\frac{d[NO_2]}{dt}

As we know that,

\frac{d[NO]}{dt} = 0.066 M/s

(a) Now we have to determine the rate of NO_2 formed.

\frac{1}{2}\frac{d[NO_2]}{dt}=\frac{1}{2}\frac{d[NO]}{dt}

\frac{d[NO_2]}{dt}=\frac{d[NO]}{dt}=0.066M/s

The rate of NO_2 formed is, 0.066 M/s

(b) Now we have to determine the rate of molecular oxygen reacting.

-\frac{d[O_2]}{dt}=-\frac{1}{2}\frac{d[NO]}{dt}

\frac{d[O_2]}{dt}=\frac{1}{2}\times 0.066M/s=0.033M/s

The rate of O_2 formed is, 0.033 M/s

6 0
3 years ago
What products are always made when any carbon-based fuel
IRISSAK [1]

Answer:

B) carbon dioxide and water

5 0
3 years ago
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