This is because solids have less energy than liquids do, hence it takes more energy to excite a solid into its gaseous phase than it does a liquid.
When opposed to merely reducing their separation, from solid to liquid, the energy needed to totally separate the molecules as they move from liquid to gas is substantially higher. The latent heat of vaporization is therefore bigger than the latent heat of fusion for this reason.
<h3>
What is heat of sublimation?</h3>
The amount of energy required to change one mole of a substance from its solid to its gaseous state under particular conditions—typically the standard ones—is known as the enthalpy of sublimation or heat of sublimation (STP). A solid's worth is based on its cohesive energy.
<h3>
What is heat of vaporization?</h3>
The term "enthalpy of vaporization," which is often referred to as "heat of vaporization" or "heat of evaporation," refers to the amount of energy that must be applied to a liquid substance in order to cause a part of that substance to transform into a gas. Vaporization's enthalpy varies with the pressure at which the transition takes place.
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The correct question is:
Why heat of the sublimation of a substance is greater than the heat of vaporization?
2 HBr + Mg(OH) 2 yields Mg(Br) 2 + 2 H2O
M1V1 = M2V2
(0.245 M)(37.5 mL) = (M2)(18.0 mL)
9.1875 = (M2)(18.0 mL)
9.1875/(18.0 mL) = (M2)(18.0 mL)/(18.0 mL)
0.51041
this is not the complete answer as the mol to mol ratio must be considered!
For every 2 mols of HBr there is 1 mole of <span>Mg(OH)2; ratio = 2:1
</span>0.51041 / 2 = 0.25520
M2 = 0.25520
0.25520 M of<span> Mg(OH)2 solution</span>
Answer:
K = 1.08 X 10¹²
Explanation:
The solved solution is in the attach document
