The density of ethanol was determined experimentally at 25°c in a series of trials to be 0.608 g/ml, 0.705 g/ml, and 0.689 g/ml. the accepted density of ethanol is reported to be 0.789 g/ml. calculate % error for this experiment. use the average experimental density in your calculation and report your answer to o.0.1%.

15.46%

0.667 g/mL (more o less) 0.052 g/mL (standard deviation)

Explanation:

To solve the problem, it is necessary calculate the average:

(0.608 g/mL + 0.705 g/mL + and 0.689 g/mL) / 3= 0.667 g/mL

standard deviation= 0.052

Now, let us calculate the % error:

[(0.789 g/mL - 0.667 g/mL) / 0.789 g/mL] * 100% = 15.46%

the reaction mixture contains some ammonia, plus a lot of unreacted nitrogen and hydrogen. the mixture is cooled and compressed, causing the ammonia gas to condense into a liquid. the liquefied ammonia is separated and removed. the unreacted nitrogen and hydrogen are then recycled back into the reactor .

the correct answer is option d

explanation:

i was wrong its d because they dont use cm when calculating square roots