Molecular Formula Proof for C,H,O, a compound with an empirical formula of C,H₂O₂: CALCULATE THE EMPERICAL FORMULA MASS DIVIDE THE MOLAR MASS OF THE UNKNOWN COMPOUND BY THE EMPERICAL FORMULA MASS 4xC-4x12.011- 48.044 3x H-3x 1.008- 3.024 166.132/83.066 = 2 2x0=2 x 15.999 - 31.998 Show the molecular formula proof for any other compound listed in the table provided: Percent Composition ONTBORK HYDROGEN 57.838% 3.6405% 79.887% 20.113% 27.293% 40.002% 83.066 g/mol 6.7142% OXYGEN 38.521% 72.711% 53.284% Empirical Formula C₂H₂O₂ CH₂ CO₂ CH,O Molecular Formula с, н.о. C₂H₂ CO₂ CHO MULTIPLY ALL THE SUBSCRIPTS IN THE EMPIRICAL FORMULA BY THE QUOTIENT C₂H₂O₂ C₂H₂O₂

Molecular Formula Proof for C,H,O, a compound with an empirical formula of C,H₂O₂: CALCULATE THE EMPERICAL FORMULA MASS DIVIDE THE MOLAR MASS OF THE UNKNOWN COMPOUND BY THE EMPERICAL FORMULA MASS 4xC-4x12.011- 48.044 3x H-3x 1.008- 3.024 166.132/83.066 = 2 2x0=2 x 15.999 - 31.998 Show the molecular formula proof for any other compound listed in the table provided: Percent Composition ONTBORK HYDROGEN 57.838% 3.6405% 79.887% 20.113% 27.293% 40.002% 83.066 g/mol 6.7142% OXYGEN 38.521% 72.711% 53.284% Empirical Formula C₂H₂O₂ CH₂ CO₂ CH,O Molecular Formula с, н.о. C₂H₂ CO₂ CHO MULTIPLY ALL THE SUBSCRIPTS IN THE EMPIRICAL FORMULA BY THE QUOTIENT C₂H₂O₂ C₂H₂O₂

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...

See similar textbooks

Similar questions

Can you help me to write the label of the units for the moles, molar mass, molecules, and grams?
A compound is 25.0% carbon, 8.4% hydrogen and 66.6% sulfur by mass. Put symbols in order of CHS. Enter the formula without subscripting the numbers, add no spaces. For example: C4H402. Its empirical formula is
1. A compound is found to contain 63.52 % iron and 36.48% sulfur. Find its empirical formula. 2. A 60.00 g sample of tetraethyllead, a gasoline additive, is found to contain 38.43 g lead, 17.83 g carbon, and 3.74 g hydrogen. Find its empirical formula. 3. Determine the molecular formula of a compound with an empirical formula of NH2 and a formula mass of 32.06 u. 4. A sample of a compound with a formula mass of 34.00 u is found to consist of 0.44 g H and 6.92 g 0. Find its molecular formula (Ctrl)
Please help, I keep getting wrong answers The molar masses and empirical formulas of several compounds containing carbon and nitrogen are as follows. Find the molecular formula of each compound. Part A163.26 g/mol, C11H17NExpress your answer as a chemical formula. Part B186.24 g/mol, C6H7NExpress your answer as a chemical formula. Part C312.29 g/mol, C3H2NExpress your answer as a chemical formula.
Find the Formula Weight of the substance to three significant figures: PBPO3 Pb: 207.2 P: 30.974 O: 15.999
Need help with percent composition calculation and empirical formula
What is the empirical formula of the following compound if a sample contains 55.3% K, 14.6% P and 30.1% O by mass? O K3P203 (all numbers are subscripts) K3PO4 (all numbers are subscripts) O K2(PO3)2 (all numbers are subscripts) KPO (all numbers are subscripts) K2PO2 (all numbers are subscripts) O O
D. Calculate the mass (g) of the following samples. 25) 238 moles of lead 26) 1.54 x 10⁹ moles of Zn 27) 7.70 x 10-⁹ moles of Mg(NO3)2 28) 8.42 x 1027 atoms of tin 29) 6.39 x 10¹8 atoms of sulfur 30) 5.99 x 1030 molecules of SiO₂
20) Write the empirical formulas for the following compound: HH -0- A) C,H¿O2 B) CH,0 C) CH,O 21) Write a sentence that describes how to determine the number of moles of a compound in a known mass of the compound if we know its molecular formula. A) Use the molecular formula to find the molar mass; to obtain the number of moles, divide the molar mass of the compound by the mass of compound. B) Use the molecular formula to find the molar mass; to obtain the number of moles, divide the mass of compound by the molar mass of the compound. C) Use the molecular formula to find the molar mass; to obtain the number of moles, multiply the mass of compound with the molar mass of the compound. 22) Compare 1 mole of H, 1 mole of O, and 1 mole of F2. Which has the largest number of molecules? Which has the greatest mass? A) All three have the same number of molecules, since a mole is defined as a specific number of particles. B) O2 has the largest number of molecules. C) H2 has the largest number…
1. Suppose that you weigh out 6.95 g of CuSO4.5 H₂O at the beginning of the experiment. How many moles of Cu 2+ are present in this sample? Express your answer to 3 significant figures, and do not include units!