Rutherford !
The so-called Rutherford experience consisted mainly of launch, against a gold plate, with a beam of particles emitted by a radioactive source. These particles whose electric charge is positive are known as alpha particles.
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Answer:
Significant hydrogen bonding is possible in
Explanation:
- Hydrogen bonding takes place between an electronegative atom (O, N and F) and a H atom attached to those electronegative atoms.
- Lewis structure reveals that H atom attached to N in .
- In all other compounds no such H atom is present attached to O or N or F.
- Hence significant hydrogen bonding is possible only in
- Lewis structures are given below.
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:
The answer is compound because they consist of multiple things.
Answer:
Kinetic Rate Laws. The rate of the crystal violet/NaOH reaction is given by the following generalized rate law. Rate = k [OHG] [CV]. (1) x y. 25. 30.
The reaction was carried out by varying the concentrations of [CV] within the range 1.00 × 10-5 M-7.00 × 10-5 M at 298 K and fixed [NaOH]o=1.67 × 10-3 M and μ=0.085 M (KNO3). The reaction is dependent on the [CV] as observed rate constant (kobs) increases with increase in [CV] as shown in Table 1.
Explanation:
to calculate the room temperature rate constant for the reaction. BACKGROUND. Reaction Chemistry. Chemical kinetics is the study of reaction rates.