Respuesta :
The experimental value has a 0.278 % error when compared to the literature / actual value.
The absolute value of the difference between the measured or the experimental value and the literature or actual value is multiplied by 100 and divided by the actual value to get the percent (%) error calculation.
Serious repercussions might happen if the analysis contains a significant inaccuracy. Analytical chemistry is built on the principles of precision, repeatability, and dependability.
The following actions can help reduce % error: guarantee that observers and measurement takers have received enough training. Use the most precise measuring device for taking the reading. Measurements must be recorded in a controlled environment. Test your measurement equipment on a pilot.
Given:
1 mol of H2 = 2.02g
To find:
% error = ?
Formula:
% error = (experimental value – literature value) / literature value x 100
Calculations:
Recall that, at STP
most gases will occupy 22.4L if they are ideal gases
Therefore,
Density = Mass / Volume
Density = 2.02g / 22.4L = 0.09017g/L
This is the experimental value for density of H2
Literature value = 0.08992g/L
% error = (0.09017 - 0.08992) / 0.08992 x 100 = 0.278% error
Result:
The % error is found to be 0.278%.
Learn more about % error in chemistry here:
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