A student carried out a similar experiment to the one in this lab, but used a hydrate of cobalt (II) chloride, CoCl2 n H20, in an attempt to find the value of n. The student used 5.125 grams of the hydrate and after the second and final heating, the anhydrous formed weighed 2.797 grams. What is the % error based on these experimental results? Round the experimental value of n to the nearest whole number and use it as the known value. Assume the known value of n to be an exact number. Enter the number only with the proper number of significant figures. Do not use scientific notation.

A student carried out a similar experiment to the one in this lab, but used a hydrate of cobalt (II) chloride, CoCl2 n H20, in an attempt to find the value of n. The student used 5.125 grams of the hydrate and after the second and final heating, the anhydrous formed weighed 2.797 grams. What is the % error based on these experimental results? Round the experimental value of n to the nearest whole number and use it as the known value. Assume the known value of n to be an exact number. Enter the number only with the proper number of significant figures. Do not use scientific notation.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter3: Mass Relations In Chemistry; Stoichiometry

Section: Chapter Questions

Problem 93QAP: A sample of cocaine, C17H21O4N, is diluted with sugar, C12H22O11. When a 1.00-mg sample of this...

See similar textbooks

Similar questions

A reaction takes place and you expect to yield 250.5 g of product. However, after the experiment, you have weighed out 253.2 g of product. The percent error is 1.08%. What are possible reasons for this?
A student performs this experiment and determines that 1.12 grams of CO2 was lost, but based on their limiting reagent calculations, 1.38 grams of CO2 was expected to be lost. What is the percent error for this student's experiment? Express your answer to the hundredths place.
My Chemistry professor was going over conversions from moles today and put the question up of how many atoms of carbon are in 500mg of C6H8O6.As far as I can tell, my dimensional analysis is correct by converting mg to g, then to mol of C6H8O6 to 6 mol of C then multiplying by Na yet my answer was incorrect by getting 1.7X1021
CoCl2 .x -H2O is the purple sample. Calulacte the value for the x integer. Mass of sample: 1.000 (g) Mass of water lost: 0.454 (g)
How did u get 2.303? I don't understand how you came up with that number and can you plz type the formula used to get t.
The mass of 4.375 x 1016 molecules of compound with the molecular formula C3H9N is ______ g. Report your answer in scientific notation and to 3 s.f. For example, if your answer was 1.076 x 10-10 you would report it as 1.08e-10.
A certain organic compound has the formula C8H12O2. A sample of this compound weighs 1.05 grams. Calculate the number of hydrogen atoms contained in this sample. Round your final result to the nearest tenth.
5. A 2.000 g sample of CoCl2·xH2O is dried in an oven. When the anhydrous salt is removed from the oven, its mass is 1.565 g. What is the value of x?
An unknown sample was found to contain the following:10.62% H42.04% O47.34% CUse this information to determine the subscript x in the formula CxHyOz. Recall that the subscripts represent whole number ratios.
Assume that the ratio of moles of Cl to moles of Cu are 2.7. If we can represent the formula by CuClx, what is the value for x? Round your answer to the nearest whole number. Do NOT include units. So, if you think the formula is CuCl6, you enter the number 6.
Chemistry A suspension was prepared by mixing spherical gum grains with a density of 1.206 gcm-3 and a radius of 0.212 μm and water with a density of 0.999 gcm-3 at 15˚C. Since the number of particles determined microscopically at 5 μm and 35 μm heights from the base is 100 and 47, respectively, in the same time, calculate Avagadro's constant (g= 9.8 m s-2, μm= 10-6 m)
0.848g of Na2B4O7.10H2O into a crucible. After hearing the sample for a short time and allowing the crucible to cool, the two students determine that the sample has a mass of 0.525g. They then do a quick calculation. based on this calculation, what should they do next?