Answer:
Option D. The water in Glass A is cooler than the water in Glass B; therefore, the particles in Glass A move slower.
Explanation:
Solubilities of solutes are enhanced when the temperature is increased.
From the experiment conducted,
It is evident that glass B temperature is higher than glass A temperature, because the solute dissolves faster in glass B than in glass A . This implies that glass A is cooler than glass B, hence the particles in A will move slower than that in B.
The answer is -60.57. With appropriate sig figs it becomes -60.6 KJ.
<span>I think you were on the right track. However you need to multiply H2O by its coefficient from the balanced equation. Then you also need to keep in mind the signs. </span>
<span>Maybe it's easier if I write what I did out: </span>
<span>2H2O > 2H2 +O2...............-H= 2* -285.83 </span>
<span>Ca + O2 + H2 > Ca(OH)2....H= -986.2 </span>
<span>2C + H2 > C2H2.................H= 226.77 </span>
<span>The above H's stand for standard enthalpy of formations. These can be found in textbook appendix. Notice the negative infront of the enthalpy (H) for H2O. This is to remind me/you that the heat lost is gained in the rxn. </span>
<span>So then you add them up. 226.77 - 986.2 + (2*285.83) = -187.77 </span>
<span>Add back the total enthalpy that is given in the question -187.77+127.2 = -60.57 </span>
<span>If signs cross you up find a way to remember that works for you. </span>
When there are lone pairs on the valence shell of the central atom in a molecule, the bond angle is decreased.
The shape of molecules depend on the number of electron pairs on the valence shell of the molecules. These electron pairs could be lone pairs or bond pairs. Lone pairs occupy more space around the central atom since it is attracted to only one nucleus compared to bond pairs which are attracted to two nuclei.
When lone pairs are present on the central atom in a molecule, they tend to "squeeze" the molecule thereby decreasing the bond angle in the molecule. Hence, presence of one or more lone pairs of electrons make the bond angles get smaller.
Learn more: brainly.com/question/10079361
Answer:
Due to hydrogen bond in propylamine.
Explanation:
The boiling point or melting point are property of
a) size
b) the intermolecular force of interactions.
As we know that primary and secondary amines form intermoleclar hydrogen bonds, which increases the force of attractions between molecules increasing the boiling point of amines.
However in case of tertiary amines there is no hydrogen directly attached to electronegative nitrogen atoms, thus no possibility of formation of hydrogen bond hence low boiling points.
The structures are shown in the figure.
For exothermic reaction (that is heat is considered as a product) then
reactants= product + Energy ,
An decrease in temperature favors the forward reaction (more product formed)
pressure depends on number of mole of the product and reactants
a A + b B + c C + d D (Where a b c and d are numerical value and A B C and D are compounds) :
if more A is added to the equilibrium mixture, equilibrium position will shift to the right (more product formed) so as to decrease concentration of A
