Just breaking stuff so yea that’s it
75.7 grams.
Convert moles to grams using this:
Moles • grams/1 mole = grams
(Grams is over 1 mole)
Answer:
C
Explanation:
The train has significantly more momentum by the car, hence there is little change in the train's momentum after collision..
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Answer:
C2H3O3
Explanation:
Empirical formula is the simplest whole number ratio of moles of atoms that you can find in a molecule.
In combustion analysis all Carbon reacts producing CO2 and all hydrogen reacts producing H2O. With the differences in masses we can find the mass of oxygen and their moles:
<em>Moles CO2 = Moles C:</em>
14.08g * (1mol/44.01g) = 0.3199 moles C * (12.01g/mol) = 3.8423g C
<em>Moles H2O:</em>
4.32g H2O * (1mol/18.01g) = 0.2399 moles H2O * (2mol H / 1molH2O) = 0.4797moles H = 0.4797g H
<em>Mass O:</em>
12.01g = Mass O + 3.8423g C + 0.4797g H
Mass O = 7.688g O
<em>Moles O:</em>
7.688g O * (1mol/16g) = 0.48 moles O
The ratio of atoms (Dividing in the moles of C that are the lower number of moles):
O: 0.48moles O / 0.3199 moles C = 1.50
C: 0.3199 moles C / 0.3199 moles C = 1
H: 0.4797 moles H / 0.3199 moles C = 1.50
As empirical formula requires whole numbers:
O: 1.50* 2 = 3
C: 1*2 = 2
H: 1.50*2 = 3
The empirical formula is:
<h3>C2H3O3</h3>
Answer:
Rate law: ![k[C_4H_6]^2](https://tex.z-dn.net/?f=k%5BC_4H_6%5D%5E2)
Integrated Rate Law: ![\frac{1}{[C_4H_6]}=\frac{1}{[C_4H_6]_0}+kt](https://tex.z-dn.net/?f=%5Cfrac%7B1%7D%7B%5BC_4H_6%5D%7D%3D%5Cfrac%7B1%7D%7B%5BC_4H_6%5D_0%7D%2Bkt)

Explanation:
We can see that the graph of time is linear compared to
and the reaction is second order hence we get the rate law from
.
The integrated rate law for second order is
where A is
.
The slope of the graph
w.r.t time is equal to k. The slope of the graph from the table is 0.014 which is equal to k.