Agroup of students perform three trials in a lab and determine the density of aluminum to be 2.1, 2.12, and 2.09 g/cm³ if the true density of aluminum is 2.7 g/cm³ what is the percent error of their lab

Percent error = -22%

Explanation:

Given data:

Density of aluminium = 2.1,2.12 and 2.09 g/cm³

Accepted value of density of aluminium = 2.7 g.cm³

Percent error = ?

Solution:

First of all we will calculate the average of data measured by students.

Average value = 2.1 g/cm³ + 2.12 g/cm³+ 2.09 g/cm³ / 3

Average value = 6.31 g/cm³/ 3

Average value = 2.1 g/cm³

Now we will calculate the percent error.

Percent error = [ Measured value - accepted value / accepted value ]× 100

Percent error = [ 2.1 g/cm³  - 2.70 g/cm³ / 2.70 g/cm³ ]× 100

Percent error = [-0.6/2.70 g/cm³ ] × 100

Percent error = -0.22 × 100

Percent error = -22%

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 .