Find the molecular formular of your unknown Molecular weight of unknown - 143.5 g/mol Emperical formular of unknown - C8H6 Assuming that the molecular formula is correct determine the expected molecular weight of your unknown and determine the percent error in your experimental value

Find the molecular formular of your unknown Molecular weight of unknown - 143.5 g/mol Emperical formular of unknown - C8H6 Assuming that the molecular formula is correct determine the expected molecular weight of your unknown and determine the percent error in your experimental value

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Determine the mass in grams of 1.6 x 10-3 mol glucose, CsH12O6 TARTING AMOUNT ADD FACTOR ANSWER RESET *( ) %3D 6.022 x 1023 12.01 0.29 180.18 0.13 9.6 x 1020 1 1.6 x 10-3 84.18 g C6H12O6 mol CoH12Oe g CeH12O6/mol molecules CH½O6
Part C: Determine percent Oxalic Acid in Unknown Sample Molar mass of oxalic acid 90.03 g/mol Trial 1 Trial 2 Trial 3 Average Precision Mass of unknown oxalic acid (g) 1.0048 0.9995 1.0018 --- Volume (mL) of Standardized KMNO4 used Moles of KMnO4 10.03 9.85 10.45 --- --- --- Moles of oxalic acid (H2C204 • 2H2O) --- --- grams of oxalic acid (H2C204 • 2H2O) (g) percent oxalic acid (%) --- --- Show calculations:
Solve correctly please. Need all a to d parts. (Gpt/ai wrong answer not allowed)
Calculate the percent error for magnesium carbonate with a measured percent magnesium of 29.4%. Group of answer choices 58.0% 1.95% 36.7% 1.99% 98.1%
Please check my work. Analyze the data for the sample to get the Empirical formula of CxHy Given data for sample compound with no oxygen: Mass of sample (g) - 5.99 Mass of carbon dioxide collected (g) - 19.25 Mass of water collected (g) - 6.57
8. Calculate the number of grams in the following in 1.77 moles of nitrogen dioxide, NO2. Must Show work with units and correct number of significant digits. Round atomic weight off periodic table to two decimal places. 9. Calculate the number of grams in the following 0.84 mole of 2-propanol, C3H30, rubbing alcohol. Must Show work with units and correct number of significant digits. Round atomic weight off periodic table to two decimal places. 10. Calculate the number of moles in 4.9 x 10³ grams of vitamin C (C6HgO6). Must Show work with units and correct number of significant digits. Round atomic weight off periodic table to two decimal places. 11. Calculate the number of moles of sodium ions in 6.56 moles of Na,S. Must Show work with units and correct number of significant digits. Round atomic weight off periodic table to two decimal places. 12. Calculate the number of molecules in 8.320 moles of Mg3(PO4)2, Must Show work with units and correct number of significant digits. Round…
Results table. To clean up, zoom out from the balance and drag the sample to the red disposal container. Repeat with ammonium chloride (NH4Cl), located on the Salts shelf. C12H22O11 NH4ClMass (g) 1.0481 g 1.0444g Molar Mass (g/mol)MolesMoles of each elementAtoms of each element Much like the previous calculation, you will use the periodic table to determine the molar massof the compound. The example shown is for sodium chloride, NaCl. The molar mass is the massof 1 sodium (22.98g/mole) and 1 chlorine (35.45g/mole) added together, 58.43g/mole. If theformula shows multiple atoms, as in sugar, you must take that into account. For sugar, it will be12 times the mass of a carbon atom plus 22 time the mass of hydrogen atom, plus 11 times themass of oxygen atoms.The calculation of moles will be similar to that done in the previous…
Could you please help me with this question? It is broken up into 3 parts and I’m having a hard time. I have attached a picture below.
Use the following atomic weights and quantities to calculate the overall % yield of hexaphenylbenzene using the following abstract equation. Assume that all the inorganic reagents are in excess but remember that your yield must be based on the stoichiometry, the limiting reagent, and that grams must be converted to moles. Filling out most of the chart will help. Give only two significant digits in your answer. If after rounding the answer is a whole number, do not include a decimal point. C = 12, H = 1, CI = 35.5, O = 16, P = 31 3 Ph Ph -Ph Fe Ph Ph 0=C: 0 Fe Ph Ph 2 HBr JULY-XH 2 Ph OH Ph Ph H4N 0 -N Ph N₂ Ph -P -Ph C 5 H₂O HC1 H₂ Ph 0 Ph formula formula weight benzaldehyde phenylacetic acid benzyltriphenylphosphonium chloride hexaphenylbenzene milliliters 4.947 22.917 density 1.044 grams moles Answer: 5.513 7.198 % yield ?
Use the following atomic weights and quantities to calculate the overall % yield of hexaphenylbenzene using the following abstract equation. Assume that all the inorganic reagents are in excess but remember that your yield must be based on the stoichiometry, the limiting reagent, and that grams must be converted to moles. Filling out most of the chart will help. Give only two significant digits in your answer. If after rounding the answer is a whole number, do not include a decimal point. C=12, H = 1, CI = 35.5, O= 16, P = 31 3 Ph Ph- Fe Ph Ph. CI B12 2 Ph H4NO N Phi OH Phi Ph Ph =C: 0 Fe Ph Ph 2 HBr N₂ Ph -Ph C 5 H₂O Ph HC1 H₂ formula formula weight benzaldehyde phenylacetic acid benzyltriphenylphosphonium chloride -> hexaphenylbenzene milliliters 3.843 16.754 density 1.044 grams moles Answer: 5.982 5.592 % yield ?
Show work using conversion factors Answer Key:#37a CaCO3 + 2HCl --> CaCl2 + H2O + CO2 #37b 36.46 g/mol HCl #37c 100.09 g/mol CaCO3 #37d 1.250 moles CO2 #37e 4.92 mole HCl #37f 7.1422 moles HCl ( fixed 10/14/2020) #37g 143 g CO2
(URGENT) Help fill in the rest of the empirical formula of an unknown chart. The parts that are filled in are given as context clues, the rest is to solve through a direct estimate.