How Much Ammonium Sulfate From 75kL Ammonia?

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Ammonia reacts with sulfuric acid to produce ammonium sulfate, a key fertilizer. To determine the mass of ammonium sulfate from 75.0 kL of ammonia at 10°C and 110 kPa, the balanced chemical equation is essential. The reaction involves stoichiometric calculations based on the volume of ammonia and its conditions. Understanding the molar relationships in the balanced equation is crucial for solving the problem. Accurate calculations will yield the mass of ammonium sulfate produced.
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ammonia reacts with sulfuric acid to form the important fertilizer, ammonium sulfate. what mass of ammonium sulfate can be produced from 75.0kL of ammonia at 10°C and 110 kPa?

k so i actually have no idea of what to do, honestly we've never covered this in my class before and we have a test o it in like 5 days, PLEASE HELP ME. IM LIKE DYING HERE.
 
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nic.harv said:
ammonia reacts with sulfuric acid to form the important fertilizer, ammonium sulfate. what mass of ammonium sulfate can be produced from 75.0kL of ammonia at 10°C and 110 kPa?

k so i actually have no idea of what to do, honestly we've never covered this in my class before and we have a test o it in like 5 days, PLEASE HELP ME. IM LIKE DYING HERE.

What is the balanced equation for this reaction?
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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