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Step2247 [10]
3 years ago
8

Which of the following is an exothermic reaction?

Chemistry
2 answers:
alekssr [168]3 years ago
7 0

Answer:

C.) condensing steam

Explanation:

Exothermic reactions are chemical reaction which energy is released to the environment in the form of heat . The overall energy of the reactant is greater than the energy of the product. The higher in energy of the reactant causes a release of heat to the environment. In exothermic reactions, enthalpy change is  usually negative and is accompanied by the loss of energy in the form of heat or light.

Condensation is the change of water vapor to liquid . The conversion is an exothermic reaction as energy is release to the environment in the form of heat.  The water vapor molecules has higher energy than liquid. The changes of water vapor to liquid causes a loss in energy of the water vapor. As the water vapor loss more energy, heat is been release to the surrounding.

All other reaction are endothermic in which heat is absorb from the environment except for condensation of steam.

PilotLPTM [1.2K]3 years ago
6 0

The event that is an example of an exothermic reaction is condensing steam. The answer is letter C. An exothermic reaction is one in which there is a release of heat during the reaction. Dissolving sugar in water, melting ice and dissolving ammonium nitrate in water are all examples of an endothermic reaction.

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would you expect the N-O bond in HNO2 to be longer, shorter, or the same length as the N-O bonds in NO2^-
prohojiy [21]
Longer, this is because the H in HNO2 is bonded with an oxygen, no longer allowing this structure to have a resonance structure.
NO2 on the other hand has one double bond and one single bond, so it has a resonance structure. And resonance structures are actually one structure so there isn't really a single and double bond, it's actually a 1 and 1/2 bond that calls for a higher bond order.
And I higher bond order will result in a shorter lengths!
I hope this helps out!!! And just out of curiosity, is this off of an AP FRQ packet??
8 0
2 years ago
1. Show that heat flows spontaneously from high temperature to low temperature in any isolated system (hint: use entropy change
Inga [223]

Answer:

1 ) Δs ( entropy change for hot block ) = - Q / th  ( -ve shows heat lost to cold block )

Δs ( entropy change for cold block ) = Q / tc

∴ Total Δs = ΔSc + ΔSh

                 = Q/tc - Q/th

2) ΔSdecomposition = Δh / Temp = ( 181.6 * 10^3 / 773 ) = 234.928 J/k

Explanation:

<u>1) To show that heat flows spontaneously from high temperature to low temperature </u>

example :

Pick two(2) solid metal blocks with varying temperatures ( i.e. one solid block is hot and the other solid block is cold )

Place both blocks for time (t ) in an insulated system to reduce heat loss or gain to or from the environment

Check the temperature of both blocks after time ( t ) it will be observed that both blocks will have same temperature after time t ( first law of thermodynamics )

Δs ( entropy change for hot block ) = - Q / th  ( -ve shows heat lost to cold block )

Δs ( entropy change for cold block ) = Q / tc

∴ Total Δs = ΔSc + ΔSh

                 = Q/tc - Q/th

<u>2) Entropy change for Decomposition of mercuric oxide </u>

2HgO (s) → 2Hg(l) + O₂ (g)

Δs = positive

there is transition from solid to liquid and the melting point of mercury ( the point at which reaction will take place ) = 500⁰C

hence ΔSdecomposition = S⁻ Hg  -  S⁻ HgO =

Δh of reaction = 181.6 KJ

Temp = 500 + 273 = 773 k

hence ΔSdecomposition = Δh / Temp = ( 181.6 * 10^3 / 773 ) = 234.928 J/k

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Answer:

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Answer:

Throughout the explanation section, the reason behind the given statement is described.

Explanation:

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