According to Joule’s law, when evaporation occurs, cooling
occurs.
(i.e. latent heat is released). We have two containers with pure
water, both at the same
room temperature. While using our IR camera, we add NaCl to one of
the and observe
that the salty container gradually looks colder. If we know that
salty
water is less prone to evaporation, hence less cooling [i.e. due to
lowering the vapor
pressure - the same reason we add salt on icy roads] then, can you
think what really
causes the cooling when NaCl is added?
The ice and water remain at equilibrium in the absence of salt.The state of matter changes when we add or remove heat from the ice.The freezing point of water gets further reduced when we add salt.Hence breaking the equilibrium as a result melting of ice starts.Heat is required to melt ice which is generally provided from outside in the form of latent heat of fusion which reduces temperature.Cooling occurs when we add salt to the ice.Reduction in temperature of salt takes place. Ice and water attain equilibrium which generally is attained below zero degree celcius.Adding more salt results in melting more ice and further temperature decreases.Due to redistribution of heat taking place among the latent heat of fusion of ice and specific heat of water cooling takes place.
According to Joule’s law, when evaporation occurs, cooling occurs. (i.e. latent heat is released). We have...
i
uploaded everything that was given. Where would I find the
experiemental values?
Complete the calculation summary below. READ THE EXPERIMENTAL DISCUSSION FIRST! REPORT ALL ANSWERS TO THE CORRECT SIGNIFICANT FIGURES. SHOW CALCULATION SET-UP on the next page. PART B: Molarity Determination via Solution Stoichiometry 7.625 g Mass of Empty 50 mL Beaker 7.976 g Mass of Beaker and NaCl (final heating) Mass of NaCl Produced (Experimental Yield of NaCl) moles Moles of Na,CO, Consumed 0.00500 Liter Volume of Na,CO,...