Because it looses it's science-street-cred if it can't be replicated.
Essentially.
If you can replicate an experiment you can prove that the results are not just a stroke of luck or happening by chance, but instead that the variables are causing the results and they will always as long as the factors of the experiment remain the same. That is the definition of a <em>scientific</em> experiment.
For all of Carbon's valencies to be satisfied:
H₂C = C = CH₂
Thus, the answer is:
B) Two
Answer:
mass of CO2 = 20.9 g
Explanation:
Given that:
mass of O2= 30.4 g
molar mass O2 = 32
number of moles of O2 = 30.4 / 32
number of moles of O2 = 0.95 moles
The Volume of O2 = 2V
Using ideal gas equation:
PV = nRT
P × (2V) = 0.95 × R × T
PV = 0.475 RT ----- (1)
For CO2;
The volume = V
Using ideal gas equation:
PV = nRT ---- (2)
Equating equation (1) and (2) together, we get:
0.475 RT = nRT
Dividing both sides by RT
(0.475 RT)/RT = (nRT)/RT
0.475 = n
Thus, the number of moles of CO2 = 0.475
Since mass = number of moles × molar mass
mass of CO2 = 0.475 × 44
mass of CO2 = 20.9 g
According to Balance chemical equation,
N₂ + 3 H₂ → 2 NH₃
1 mole of Nitrogen reacts with 3 moles of Hydrogen to produce 2 mole of Ammonia.
It is known that i mole of any gas at standard temperature and pressure occupies 22.4 L of Volume. So, we can also say,
22.4 L (1 × 22.4) of Nitrogen gas (in question it is taken in excess) reacts with 67.2 L (22.4 × 3) of Hydrogen gas to produce 44.8 L (22.4 × 2) of Ammonia.
Result:
44.8 L is the correct answer.
Answer:
See explanation below
Explanation:
You are not putting the mechanism step you want to be explained. I found this question, and it's attached on picture 1.
According to that, we do have a Aryl halide, reacting with cyanide ion, and then, LiAlH4.
The first step is a Sn2 reaction where the cyanide ion displace the Bromide. The second step is the reduction, which is a long step mechanism, and this is shown in pícture 2. At the end of this step, we already has added a CH2 in the molecule, and the water will allow to reduce the N group with the AlH3 to the respective primary amine.
See picture below for explanation of the mechanism