What happens to the atoms in a scoop of ice cream as it melts?

2 answers:

6 0

The solid water begins to change into liquid water when the ice molecules start to move around. Another way to say that a substance changes from the solid state to the liquid state is to say it melts. Te ice continues to melt as more ice molecules get enough energy to move around.

baherus [9]3 years ago

3 0

You might be interested in

Symbol for protons, neutrons, electrons in chemistry.

CaHeK987 [17]

This is the symbols for protons, neutrons, and electrons

7 0

3 years ago

Read 2 more answers

If your good at science you could help me out so much!

Andrei [34K]

Answer:

Potassium (K) and Lithium (Li) for the fist one i cant see the second

Explanation:

6 0

3 years ago

How many grams of oxygen are required too burn 8.8g of c3h8?

hichkok12 [17]

From the balanced equation:
1mol C3H8 requires 5mol O2 for combustion 
Molar mass C3H8 = 44g/mol 
8.8g C3H8 = 8.8/44 = 0.2mol C3H8 
This will require 5*0.2 = 1.0mol O2 
Molar mass O2 = 32g/mol 
Therefore 32g of O2 required.

4 0

3 years ago

A solution may contain Ag+, Pb2+, and/or Hg22+. A white precipitate forms when 6 M HCl is added. The precipitate is partially so

omeli [17]

Answer:

All three are present

Explanation:

Addition of 6 M HCl would form precipitates of all the three cations, since the chlorides of these cations are insoluble: $AgCl (s), PbCl_2 (s), Hg_2Cl_2 (s)$ .

Firstly, the solid produced is partially soluble in hot water. Remember that out of all the three solids, lead(II) choride is the most soluble. It would easily completely dissolve in hot water. This is how we separate it from the remaining precipitate. Therefore, we know that we have lead(II) cations present, as the two remaining chlorides are insoluble even at high temperatures.
Secondly, addition of liquid ammonia would form a precipitate with silver: $AgCl (s) + 2 NH_3 (aq) + H_2O (l)\rightarrow [Ag(NH_3)_2]OH (s) + HCl (aq)$ ; Silver hydroxide at higher temperatures decomposes into black silver oxide: $2 [Ag(NH_3)_2]OH (s)\rightarrow Ag_2O (s) + H_2O (l) + 4 NH_3 (g)$ .
Thirdly, we also know we have $Hg_2^{2+}$ in the mixture, since addition of potassium chromate produces a yellow precipitate: $Hg_2^{2+} (aq) + CrO_4^{2-} (aq)\rightarrow Hg_2CrO_4 (s)$ . The latter precipitate is yellow.