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meriva
3 years ago
7

How many ions are in 32.45 grams of silver carbonate

Chemistry
1 answer:
GuDViN [60]3 years ago
4 0

Answer:

0.0036265350669622

Explanation:

Report if wrong

-Atlas-

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During the formation of a chemical bond between two hydrogen atoms, which of the following statements is always true?
Wewaii [24]

A) Energy is released during the formation of the bond.

Explanation:

During the formation of a chemical bonds between two hydrogen atoms, energy is always released during the formation of this bond type.

Bond formation process is usually exothermic and energy is released during the formation of the bond.

  • Bond breaking process is an endothermic process in which energy is absorbed from the surrounding.
  • Whenever a bond is broken, the bond energy value is positive but when a bond is formed, the bond energy value is given a negative sign.

For a bond formation process in which hydrogen atoms are bonded covalently, energy is usually released.

Learn more:

Enthalpy changes brainly.com/question/10567109

#learnwithBrainly

5 0
3 years ago
An endergonic reaction with a Δh and Δs can be changed into an exergonic reaction.
zheka24 [161]

Full question:

This question is incomplete, here it is completed:

An endergonic reaction with a ______ ∆H and a ______ ∆S can be changed into an exergonic reaction by decreasing the temperature.

Option A: negative, positive

Option B: negative, negative

Option C: positive, positive

Option D: positive, negative

Answer:

Option B: negative, negative

Explanation:

The change in free energy (ΔG) of a system for a constant-temperature process is

ΔG = ΔH - TΔS

free energy is the energy available to do work. Thus, if a particular reaction is accompanied by a release of usable energy (that is, <u>ΔG is negative</u><u>), it is said to be</u><u> exergonic</u>. On the other hand, if a reaction consumes energy (that is, <u>ΔG is positive</u><u>), it is said to be </u><u>endergonic</u>.

Looking at the equation, we can see that if ΔH is negative and ΔS is negative, then ΔG will be negative only when TΔS  is smaller in magnitude than ΔH. This condition is met when T is small.

ΔG = ΔH - TΔS

           -        -

This means that the reaction proceeds spontaneously at low temperatures. At high temperatures, the reverse reaction becomes spontaneous. An example of that would be the following reaction:

NH₃(g) + HCl(g) → NH₄Cl(s)

4 0
3 years ago
"would you expect to find sodium chloride in underground rock deposits as a solid, liquid, or gas? explain."
Sophie [7]

A sodium chloride is like most of the ionic compounds existing here on earth in which they are composed of having a high melting point and by this, if found in underground rock deposits, they are usually in a form of solid.

3 0
3 years ago
At what temperatures is a reaction that has a positive change in entropy
Setler [38]

Answer:

the answer is A

I made a chart for AP chem if you want to refer to it.

3 0
3 years ago
Circle the atom with the largest atomic radius in each group
Dominik [7]

Answer:

The atomic radius increases down the group because more shell are added

Explanation:

Al >B

Na>Al

S>O

O>F

Br>Cl

Mg>Ca

4 0
3 years ago
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