Given the following equation n2o(g) + no2(g) → 3no(g) ∆h =-92 kj/mol
A. Is this reaction exothermic or endothermic?
B. What direction with the equilibrium shift if Nitrogen gas is removed?
C. What direction will the equilibrium shift if the temperature is lowered?
D. What direction will the equilibrium shift if ammonia (NH3) is added?
E. What principle helped you solve B-D?

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.