The reaction of nitrogen gas and oxygen gas to form nitrogen monoxide gas is shown below. if the measured concentrations of all three chemicals at some point in time are: [n2] = 0.80 m
[o2] = 0.050 m
[no] = 0.10 m
which statement is true about the reaction at this point in time? n2(g) + o2(g) ⇄ 2 no(g) k = 0.10
the reaction is at equilibrium.
the reverse reaction is occurring at a faster rate than the forward reaction.
the forward reaction is occurring at a faster rate than the reverse reaction.
this set of concentration values is impossible because the concentrations of n2 and o2 must be the same.

This is a characteristic of the elements in the periodic table that shows a pattern. it may increase or decrease across or down the table.

The element that has the greatest electronegativity is

These questions are based on the attached photo. the experiment is about burning magnesium metal with oxygen. 1. write the balanced chemical equation for the reaction you are performing. 2. calculate the mass of magnesium metal used in each trial. o trial 1: o trial 2: 3. calculate the actual yield of magnesium oxide for each trial. o trial 1: o trial 2: 4. magnesium is the limiting reactant in this experiment. calculate the theoretical yield of mgo for each trial. o trial 1: o trial 2: 5. determine the percent yield of mgo for your experiment for each trial. o trial 1: o trial 2: 6. determine the average percent yield of mgo for the two trials. your company currently uses a process with a similar cost of materials that has an average percent yield of 91 percent. if the average percent yield of this process is higher than that, this could save the company money. what is your recommendation to the company? support your recommendation using your data, calculations, and understanding of stoichiometry gathered from this lab.