Answer:
Explanation:
Hello,
In this case, by computing the equilibrium constant considering the law of mass action of the undergoing chemical reaction we obtain:
Now, the ICE table turns out:
Now, the change "" due to the reaction is computed via the equilibrium concentration of ammonia as shown below:
Therefore, the initial concentrations result:
Best regards.
Not much.
Ice is only water, when the molecules are submitted to low temeperatures and have formed a crystalline arrangement of low density. In ice, the molecules arange themselves in hexagons with hydrogen bonds binfing each molecule.
When ice melts it turnes into water and the molecules leave the crystalline shape and come back to their normal density. In water, not all molecules are binded forming short and irregular lines.
→ In the image below, you can see the arrangement of ice and water.
Hope it helped,
BioTeacher101
Answer:
See the last entry
Explanation:
Remark
Ammonium Nitrate decomposes as follows.
NH4NO3 → N2O + 2H2O
If this does not agree with the reaction you have, let me know.
Step One
Find the molecular Mass of Ammonium Nitrate.
N = 1 * 14 = 14
H = 1 * 3 = 3
N = 1 * 14 14
O3 = 3<u>*16 = 48</u>
Molar Mass =69
Note: the masses used are approximate. Every periodic table is different. When you answer this question use the masses on your periodic table. My numbers are just guides.
Step Two
Find the number of mols in Ammonium Nitrate.
<u>Formula</u>
mols = given mass / molar mass
<u>Givens</u>
given mass = 3.14
Molar Mass = 69
mols = 3.14 / 69
mols = 0.0455
Step 3
moles of water.
1 mol of Ammonium Nitrate = 2 mols of water
0.0455 mols of Ammonium Nitrate = x mols of water
x = 2* 0.0455 mols of water.
x = 0.091 mols of water
Step 4
Find the molecules of water.
1 mol of water = 6.02*10^23 molecules of water
0.091 mol water= x
x = 0.091 * 6.02*10^23
x = 5.48 * 10^23
The correct answer is A.) dilute