(Must show work for all questions and round the answers to the correct number of significant figures ) 1.Determine the number of atoms in 4.67 mol Zn. 2.Given 7.65 mol AgNO3, determine the number of formula units. 3. Calculate the number of molecules in 11.34 mol H2O. 4. Perform each of the calculations and show your work. How many moles are in each of the following?90.3 g Fe, 300.0 g Zn, 1.00 g Ag . 5. Determine the mass in grams of each of the following: 3.89 mol Fe, 34.7 mol Co, 2.45 mol Rb. 6.How many atoms are in each of the following: 45.6 g Li, 0.230 g Ti, 11.5 g Au. 7. What is the mass in grams of each of the following (This question goes with Picture 1) Please show work for the following below and round your answer to the correct significant figures. How many moles are in each of the following:(This question goes with Picture 2)

Q: a. How many moles of phosphorus trichloride are present in 7.95 × 1022 molecules of this compound?…

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Q: 2. How many moles are there in 7.22 x1024 molecules of H,O? PART II. Instruction: Calculate the…

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Q: Determine the number of molecules of Cr.O. that form when 1.34 x 10 gof oxygen completely reacts…

A: Given: Mass of Oxygen = 1.34 x 103 g Given Reaction is  To determine- Number of molecules of Cr2O3

Q: How many formula units are in 35.4 g of NaCl? Calculate the mass of 2.50 mol of Fe(OH),. What is the…

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Q: 48. How many iron atoms are in 0.32 mol of Fe2O3? A) 3.9 x 1023 iron atoms B) 1.9 x 1023 iron atoms…

A: Answer

Q: Perform each of the following calculations.  You must show your work to receive credit and must must…

A: No of atom/molecules = mole × Avogadro number

Q: Which of the following is included in all the conversion factors we've used in this unit so far? A.…

A: We have to find out which conversion factor is used in the given calculation.

Q: 1. How many moles are present in 24.0 grams of Sb,S,? a. 1.31x10 mol b. 1.56x10 mol c. 5.94x10 mol…

A: (1) Number of moles of Sb2S5 can be determined by using the formula given below as: Moles of…

Q: 19 How many moles are there in 2.00×10 Molecules of C Cly?

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Q: What is the mass (in grams) of Zn(NO3)2 that contains 3.82 x 1023 N atoms? Note: Molar mass of…

A: Given that:The molar mass of Zn(NO3)2 = 189.4 g/molThis implies that the mass of 1 mol of Zn(NO3)2…

Q: 1. How many moles of Na are there in a sample that contains 6.16×1022 sodium atoms? moles 2. How…

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Q: 1. Find the number of moles in 3.7 x 10 ^-5 g of magnesium phosphate.

A: The chemical formula of the given magnesium phosphate compound is Mg3(PO4)2. Given that, the grams…

Q: Calculate the number of moles for each of the questions below. Use the space on the right to show…

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Q: How many molecules are in the sample? 87 g CCl4 Express your answer using two significant figures.

A: Number of moles can be calculated as follows: No. of moles = MassMolar massNo. of moles = 87g153.82…

Q: What would you multiply "atoms of calcium" by to get the units "moles of calcium"? atoms Cax = moles…

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Q: . The formula for ibuprofen is C3H1O2. How many moles of ibuprofen are present in 250.0-mg tablet?

A: Since you have posted multiple questions, we are entitled to answer the first only. Please repost…

Q: 1. How many moles is 8.1 x 10^24 molecules of HCN? SHOW YOUR WORK!

A: Number of molecule given = 8.1 × 10^24molecule

Q: A student synthesizes tin oxide to create a compound with generic formula SnxOy. She does this by…

A: The mass of tin is = 30.80 g The mass of tin oxide is = 39.10 g The mass of oxygen is = 39.10 g -…

Q: An unknown compound comprised of osmium and chlorine is 40.11% osmium by mass. a. If you assume…

A: Hello. Since the question contains more than three sub-parts, the first three sub-parts shall be…

Q: Convert 6.00 moles of calcium to atoms. O 8.50x1024 atoms O 1.56x1023 atoms O 3.61x1024 atoms…

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Q: Writing Empirical Formulas from Chemical Formulas

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Q: Calculate the number of CO, molecules in 2.25x10-2 mole of CO2, Express your answer using three…

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Q: 1. A chemist has a 60g sample of element X and incrementally adds element Y, known to react with…

A: From the given information,The corresponding equation will be:X   +  Y  →   XY Mass of X = 60g Mass…

Q: Find

A: Molar mass of NO2 = ( molar atomic mass of N ) + 2 • ( molar atomic mass of O )  Molar mass of NO2 =…

Q: 2. What is the percent by mass of each element in the following compounds? Compound % By Mass(for…

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Q: 1. A certain compound has a molar mass of 194.19 g/mol. Its percent composition by mass is given…

A: 1.  Given that, a certain compound has a molar mass of 194.19 g/mol. The percent composition ratios…

Q: a. How many moles of carbon tetrachloride are present in 3.10 x 1022 molecules of this compound?…

A: 1 mole = 6.022×1023 (Avogadro's number)  The mass of one mole of molecules of a substance is called…

Q: More commonly, the empirical or simplest formula of a compound is determined by finding the masses…

A: Answer:Number of moles of a substance is always equal to the ratio of its mass and molar mass,…

Q: How many grams of sodium bicarbonate are in 4.5 moles of sodium bicarbonate (84.007 g/mole)? O 189.0…

A: Moles = mass/Molar mass

Q: I. COMPLETE THE TABLE Use the given values in the table to solve the missing values. Mass Number of…

A: As per our guidelines, I can only answer first three sub-parts because you have posted multiple…

Q: How many moles are in 20.0 grams of F2?760. 760. moles 1.05 moles 0.526 moles 19.0 moles 38.0 moles

A: Given data contains, Grams of F2 is 20.0 grams. Molar mass of F2 is 37.99 g/mol.

Q: Complete these statements, supplying the proper quantity. 1. A mole of O atoms contains ----- atoms.…

A: Avogadro’s number is used to determine the number of atoms present in 1 mol of an element.…

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.