Ask question

Ask question

All categories

3 years ago

14

What kind of chemical reaction does the chemical equation sodium + chlorine → sodium chloride represent? A. combustion B. decomp

osition C. single replacement D. synthesis

1 answer:

KatRina [158]3 years ago

8 0

Answer:

d. synthesis

Explanation:

it uses the formula a+b=ab.

You might be interested in

Mass can be created and destroyed.

Musya8 [376]

Answer:

Conservation of Energy and Mass

The law of conservation of mass states that in a chemical reaction mass is neither created nor destroyed. ... Similarly, the law of conservation of energy states that the amount of energy is neither created nor destroyed.

5 0

2 years ago

Helpppp fasttttttttttttttt Choose the best word to complete the sentence.

Lapatulllka [165]

Answer:

equilateral (B)

Explanation:

it is the only word which relates to triangles and their shape - plus, its logical and makes sense.

5 0

3 years ago

SCIENCE - Can someone tell me the ph level of rain water?

amid [387]

Normal rainwater has a pH of 5.6<span> (slightly acidic)</span>

8 0

3 years ago

using the knowledge of the structures of argon and chlorine. Explain why they are both gases at room temperature ?

aleksley [76]

Because at atmospheric pressure the boiling point is below room temperature, just like Oxygen, Nitrogen etc

3 0

3 years ago

A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion solution and another electrode c

Andre45 [30]

<u>Answer:</u> The standard potential of the cell is 0.77 V

<u>Explanation:</u>

We know that:

$E^o_{Ni^{2+}/Ni}=-0.25V\\E^o_{Cu^{+}/Cu}=0.52V$

The substance having highest positive $E^o$ reduction potential will always get reduced and will undergo reduction reaction.

The half reaction follows:

<u>Oxidation half reaction:</u> $Ni(s)\rightarrow Ni^{2+}(aq)+2e^-$

<u>Reduction half reaction:</u> $Cu^{+}(aq)+e^-\rightarrow Cu(s)$ ( × 2)

To calculate the $E^o_{cell}$ of the reaction, we use the equation:

$E^o_{cell}=E^o_{cathode}-E^o_{anode}$

Substance getting oxidized always act as anode and the one getting reduced always act as cathode.

Putting values in above equation follows:

$E^o_{cell}=0.52-(-0.25)=0.77V$

Hence, the standard potential of the cell is 0.77 V

5 0

3 years ago