They try to base their conclusions off of data and measurements of which they should record from conducting experiments
Answer:
There is a mass of 154 Grams of Carbon Dioxide.
Explanation:
One mole is equal to 6.02 × 10^23 particles.
This means we have 1.05 X 10^24 total particles of Ethane.
Each ethane particle contains 2 carbon atoms.
If every particle of ethane is burned, we will end up with 2.10 x 10^24 molecules of Carbon Dioxide (Particles of Methane x 2, since each Methane particle contains 2 carbon atoms)
Carbon Dioxide has a molar mass of 44.01 g/mol
So if we take our amount of Carbon Dioxide molecules and divide it by 1 mole, ((2.10 x 10^24)/(6.02 x 10^23) = 3.49) we find that we have 3.49 moles of Carbon Dioxide.
Now all we need to do is multiply our moles of carbon dioxide(3.49) by it's molar mass(44.01) while accounting for significant digits.
What you should end up with is 154 Grams of Carbon Dioxide.
Hope this helps (And more importantly I hope I didn't make any errors in my math lol)
As a side note this is all assuming that this takes place at STP conditions.
-they are inside the nucleus of an atom
- they have a relative charge of +1
- they have a relative mass of 1
Answer: Option (d) is the correct answer.
Explanation:
Steps involved for the given reaction will be as follows.
Step 1: 
(fast)
Rate expression for step 1 is as follows.
Rate = k ![[NO]^{2}](https://tex.z-dn.net/?f=%5BNO%5D%5E%7B2%7D)
Step 2: 
This step 2 is a slow step. Hence, it is a rate determining step.
Step 3. 
(fast)
Here, 
is intermediate in nature.
All the steps are bimolecular and it is a second order reaction. Also, there is no catalyst present in this reaction.
Thus, we can conclude that the statement step 1 is the rate determining step, concerning this mechanism is not directly supported by the information provided.
