Lab Report 3 Moles

O STOICHIOMETRY Using the Avogadro Number An aluminum atom has a mass of 4.48 × 10 -23 g and a small airplane has a mass of 5000. kg. Use this information to answer the questions below. Be sure your answers have the correct number of significant digits. What is the mass of 1 mole of aluminum atoms? Round your answer to 3 significant digits. How many moles of aluminum atoms have a mass equal to the mass of a small airplane? Round your answer to 3 significant digits.

How can we find out the formula?

Question 1 options: A. The Mole We will use the analogy of an elephant and its body parts to explore the concept of moles of compounds or elements. The elephant and the carbon tetrachloride, CCl4 molecule are the test cases. One elephant has one trunk and four legs One carbon tetrachloride molecule, CCl4, contains one carbon atom and four chlorine atoms 1 amu = 1.6606 x 10-24 g 1 dozen = 12 items 1 mole = 6.022 x 1023 items = Avogadro's Number   Critical Thinking Questions: (Give your answers in terms of a number such as 17 or 3.25 x 1015 trunks)   How many carbon atoms are found in one dozen carbon tetrachloride (CCl4) molecules?

I added the screenshot of the question that I have been having trouble with, please help.

A compound contains Carbon, Oxygen, and Fluorine. Determine the empirical formula (CXOYFZ) by identifying the smallest whole number set of X, Y, and Z using the data below. A sample of the compound contains 8.25 x 1024 Carbon atoms, 5.48 moles of O, and 8.22 moles of E. • Subscript X for C would be [Select] • Subscript Y for O would be [ Select ] • Subscript Z for F would be [ Select ] (Atomic Masses: C = 12.01 g/mol, O = 16.00 g/mol, F = 19.00 g/mol) %3D (Avogadro's Number = 6.022 x 1023 particles in one mole of particles) >

Q Search th. References Use the References to access important values if needed for this question. A compound is found to contain 37.23 % carbon, 7.827 % hydrogen, and 54.94 % chlorine by weight. To answer the questions, enter the elements in the order presented aboye. 1. What is the empirical formula for this compound? 2. The molecular weight for this compound is 64.52 g/mol. What is the molecular formula for this compound? Submit Answer nt Composition to Empirical a... : This is group attempt 1 of 5

esc Measurements show that unknown compound X has the following composition: element iron 0 oxygen Write the empirical chemical formula of X. Explanation JAN mass % 69.9% 30.0% Check # X 200 S 888 F4 0/ F5 MacBook Air A F6 F7 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center DII FB F9 A F10

Round 2 decimal places for molar mass Use correct number of sig figs Use leading zeros

Use the References to access important values if needed for this question. A compound is found to contain 26.73 % phosphorus, 12.09 % nitrogen, and 61.18 % chlorine by weight. To answer the questions, enter the elements in the order presented above. 1. What is the empirical formula for this compound? 2. The molecular weight for this compound is 115.9 g/mol. What is the molecular formula for this compound? Submit Answer 5 question attempts remaining

Match the left column correctly with the right column.         Hg2CL2 molecular element Silicon dioxide atomic element Hydrosulfuric acid molar mass HIO4 si O2 NO mole Avogadro's Number H2S Isotopers NO2 Germanium Nitorgen monoxide O2 gas periodic acid   metalloid                                                                 mercury(I) chloride                                                                 Silicon oxide                                                                  percent natural abundance

There are 1.5 x 1023 atoms in 2.5 moles of zinc. TRUE FALSE Check it skip 2 SCRATCHPAD Improve - GET A HINT

A molecule contains 16.623% hydrogen, 2.078% oxygen, and no other element except carbon. What is the empirical formula? C = 12.01 g/mol H = 1.01 g/mol O 16.00 g/mol Make sure that you use the letter O not the number O for oxygen please! The computer system will not recognize zero as 'O! Make sure that your formula has a C first, then a H in the middle, then the oxygen. You will not be able to do subscripts so If the formula was CH₂O, you will need to type CH2O A/

b Learning Goal: To learn how to convert grams to moles and to use the mole to find the number of atoms in a sample. The mole (abbreviated mol) is a counting unit used to simplify calculations that would otherwise involve very large numbers. The mole is equivalent to the number of carbon atoms in exactly 12 g of isotopically pure 12C, or 6.02 x 1023. This number is known as Avogadro's number in honor of Amedeo Avogadro. "ock Avogadro's number can be used as a conversion factor between moles and atoms as shown here: The molar mass of a substance is the mass of one mole of a substance and is written in units of grams per mole. The molar mass of an atom is equivalent to its atomic mass whereas the molar mass of a substance is equivalent to its formula weight. esc ! 6.02x10 atoms 1 mole of atoms 1 Q A N @ 2 W S 3 X 2 Control option command H 80 E D $ 4 C Part A How many moles of atoms are in 5.00 g of 13 C? Express your answer numerically in moles. ▸ View Available Hint(s) a Part B…

An analytical chemist measures the amount of Elements E, and E₂ in four samples of an unknown Substance X: mass mass sample of E₁ of E₂ 1 2 3 4 12.2 g 13.8 g 12.5 g 14.4 g 6.1 g 6.9 g Continue It's known that X contains no elements other than E, and E. 11.7 g 13.3 g Using this information, answer the questions in the table below. Is X a pure substance or a mixture? If you don't have enough information to decide, choose can't decide. If you said X is a pure substance, calculate the mass of Element E, the analytical chemist would find in a new 10.0 g sample of X. Round your answer to 2 significant digits. Opure substance O mixture O (can't decide) U MacBook Air 0 X Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms

Pls help, sorry for the trouble, ignore my handwriting

Help with #6 please.

Show ALL your work.  Remember to follow significant digit rules and show proper format in all answers. NOTE: Record all molar mass values to 2 decimal places. Question: Calculate the number of ions in 7.15 g of RbNO3.

F7 1/2 | - 100% + » c. 132.07 g/mol d. 29.02 g/mol e. 89.07 g/mol (2) How many molecules are in 30.1 g of sulfur dioxide? a. 1.81 x 10²5 b. 2.83 x 1023 c. 6.02 x 1023 d. 1.02 x 1024 e. 5.00 x 10-23 (3) How many moles of hydrogen are there in 6.50g of ammonia (NH³)? a. 0.382 mol b. 1.39 mol F8 c. 0.215 mol d. 1.14 mol e. 2.66 mol (4) What are the stoichiometric coefficients in the following equation when it is balanced? SiCl4(s) + H₂O(1)→ H₂SiO3(s) + HCl (g) a. 1,3,1,3 b. 1,1,3,4 c. 1,4,1,4 d. 1,3,1,4 e. 3,9,1,4 (5) Ammonia is produced by the reaction of nitrogen and hydrogen: N2(g) + H2(g) → NH3(g) Q Search F9 * F10 F11 Bb ☆ LO @ Home End Insert Delete

A sample of 7.55 g of Mg(OH)2 is added to 25.0 mL of 0.195 M HNO3. Part C How many moles of Mg(OH)2 are present after the reaction is complete? Express your answer in moles to three significant figures. moles Mg(OH)2 = mol %3! Submit Request Answer Part D How many moles of HNO3 are present after the reaction is complete? Express your answer in moles to three significant figures. ΑΣΦΦ mol moles HNO3 : Submit Request Answer Part E How many moles of Mg(NO3)2 are present after the reaction is complete? Express your answer in moles to three significant figures. ΑΣφ