The two pictures shown below represent starting conditions for the following reaction: O3 (g) + NO(g) → O2 (g) + NO2 (g) with a rate law: Rate = k (O3 )(NO) Which flask will react faster than the other? Determine how much faster the fast one reacts compared to the slow one? Explain your answers in terms of molecular collisions.

How do I find the answer to this? My thinking is that box a will react more since there's equal amounts of reactants but box b will react faster since there's so much NO to collide with the O3 molecules. Thanks.

14 days is the half-life of phosphorus-32

give me abc and i will get it for u.

hydrocarbons are organic compounds that contain only hydrogens and carbons. they can be saturated (those which contain only carbon-carbon single bonds) or unsaturated (those which contain carbon-carbon double or triple bonds) in nature. hydrocarbons can undergo several reactions like substitution, elimination etc.  

on substituting one or more hydrogen atoms in hydrocarbon it results in the formation of haloalkane. as the halogen atoms are large compared to the carbon and hydrogen atoms, due to which the molecular weight increases and the bond become polar because of presence electronegative halogen atom and results in the increase in boiling point of the haloalkane.

thus, the correct option is (b) that is the boiling point of the new compound increases on substituting a hydrogen atom with a halogen in a hydrocarbon.