Experiment 1: Perform the calculations and record the following data in the table. What is the empirical formula of the coppersulfate hydrate? The molar mass of water is 18.015 g/mol and the molar mass of anhydrous copper sulfate is 159.609 g/mol.mass of water in the hydrate sample (g)number of moles of water (mol)mass of anhydrous salt (g)number of moles of anhydrous salt (mol)molar ratio of anhydrous salt to waterempirical formula of the hydrate

Answered: Image /qna-images/answer/13f88c76-033d-4c91-a8d2-ef02d9adfeb1.jpg

Answered: Experiment 1: Perform the calculations…

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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Moles, Mass and Number of Particles Activity Part A: Complete the chart by calculating the missing information. Use your orange Periodic Table and round significant figures accordingly. Pro tip! If you are using a calculated value in a subsequent calculation, keep at least an extra 2 significant figures in your calculation, and round your final answer. Contents Bag # Write Chemical Formula Calculate Molar Mass Mass (g) # of moles (g/mol) Manganese (IV) oxide 1 MnO₂ 86.94g/mol 12.08g(1 mol/86.94g) =0.1390 mol Sulfur 2 Copper 3 1.70 mol Sodium Bicarbonate Carbon 1.89 mol Zinc Sodium Chloride Barium Chloride 0.264 mol Lactose S 4 5 6 7 8 9 12.08 g 12.10 g 16.8 g 39.49 g 3.400 g 110.8 g # of particles (atoms/molecules/ions/formula units as indicated) # oxide ions 0.138946mol(6.022 x 10²¹ formula units/1 mol)(2 oxide ions/formula unit) = 1.673 x 10¹ oxide ions. # atoms (total) #atoms # sodium atoms #atoms #atoms (total) #formula units #chloride ions #atoms (total)
A chemist will use a sample of 30 g of ethanol (CH3CH2OH) in an experiment. In one to two sentences, make and justify a claim about the number of moles of ethanol the chemist will use
Consider this reaction involving an unknown element X. F, + 2 XBr → Br, + 2 XF When 5.800 g of XBr reacts, 3.894 g of Br, is produced. Calculate the molar mass of X, and then identify its element symbol. 40.83 element symbol for X: K molar mass of X: g/mol Incorrect
Answer all parts of each question both 15 and 16 both part a) and b).
a compound is 30.4% N, and 69.6% O (by mass). Calculate the empirical formula for this compound. use: 14.007 g/mol for N and 15.999 g/mol for O
Brasses are alloys in which copper is the primary component and zinc is the second most abundant element. Naval brass, which has a high resistance to salt corrosion is 60.0% Cu, 39.25% Zn, and 0.75% Sn. How many moles of zinc are present in a 72.1 gram sample of naval brass? Report your answer with three significant figures.
calculate the mass of calcium carbonate in the weighing boat using the information below. Mass of weighing boat 2.26 g Mass of calcium carbonate & weighing boat 9.80 g Mass of calcium carbonate _____ g For Part B, calculate the number of moles of calcium carbonate using a molar mass of 100.09 g/mol for calcium carbonate. Label each of your 2 answers when you type your response.
A compound has the following % composition data 49 48% Carbon 5.15% Hydrogen 28.87% Nitrogen 16.49% Oxygen hift The molecular weight is between 180 g/mole and 200 g/mole tab Determine the empirical and molecular formula caps lock Edit Format Table esc 12pt v Paragraph ! 1 Q A 2 N BIU AT²V W #3 E S D $ 4 4 R X C % 5 F M T V MacBook Pro A 6 G Y B 27 & U *00 8 - N ( 9 H J K M ) O- 0 0 < St
Question 3) Consider the reaction, 3CC14+2SBF3>3CCI2F2 + 2S6C13 if 150.0 g of CCI4 (153.8 g/mol) is mixed with 100 g of SbF3 (178.8 g/mol), then the mass in grams of CC12F2 (121.0 g/mol) that can be formed is equal to:
Convert 4.80 x 1021 molecules of H2O2 to moles H2O2. 0.363 moles H2O2 0.00797 moles H2O2 6.022 x 1023 moles H2O2 2.89 x 1045 moles H2O2
Find the empirical and molecular formulas 20.2 % Sodium 37.6 % Sulfur 42.2 % Oxygen Molar Mass: 682.8 g/mol

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