Moles, Mass and Number of Particles ActivityPart 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 2significant figures in your calculation, and round your final answer.ContentsBag #Write Chemical FormulaCalculate Molar MassMass (g)# of moles(g/mol)Manganese (IV) oxide1MnO₂86.94g/mol12.08g(1 mol/86.94g)=0.1390 molSulfur2Copper31.70 molSodium BicarbonateCarbon1.89 molZincSodium ChlorideBarium Chloride0.264 molLactoseS45678912.08 g12.10 g16.8 g39.49 g3.400 g110.8 g# of particles(atoms/molecules/ions/formula units as indicated)# oxide ions0.138946mol(6.022 x 10²¹ formulaunits/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)

Dear student , since you have posted multiple parts questions we will allow to solve only first…

Bag # 2 3 5 Contents Write Chemical Formula Calculate Molar Mass (g/mol) Manganese (IV) oxide MnO₂ 86.94g/mol Sulfur Copper Sodium Bicarbonate Carbon Mass (g) 12.08 g 12.10 g 16.8 g # of moles 12.08g(1 mol/86.94g) =0.1390 mol 1.70 mol # of particles (atoms/molecules/ions/formula units as indicated) # oxide ions 0.138946mol(6.022 x 10²0 formula units/1 mol)(2 oxide ions/formula unit) = 1.673 x 10¹ oxide ions # atoms (total) # atoms # sodium atoms #atoms

Bag # 2 3 5 Contents Write Chemical Formula Calculate Molar Mass (g/mol) Manganese (IV) oxide MnO₂ 86.94g/mol Sulfur Copper Sodium Bicarbonate Carbon Mass (g) 12.08 g 12.10 g 16.8 g # of moles 12.08g(1 mol/86.94g) =0.1390 mol 1.70 mol # of particles (atoms/molecules/ions/formula units as indicated) # oxide ions 0.138946mol(6.022 x 10²0 formula units/1 mol)(2 oxide ions/formula unit) = 1.673 x 10¹ oxide ions # atoms (total) # atoms # sodium atoms #atoms

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

How many formula units are present in 500.0 g of Substance A. (molar mass 278.2g/mol) O 1.082 x 1024 formula units 8.371 x 1028 formula units O 2.310 x10-19 formula units
Balance the following chemical equation. NaN, - Na + N2 Products Reactants Na = Na = N = N = Calculate the Molar Mass for the Following Compounds. Use the Periodic Table ! Periodic Table:https://ptable.com/#Properties Compound / Chemical Formula Molar Mass Example : 0, 32.00 grams = 1 mole NaN, Na N2
What is the maximum mass of S, that can be produced by combining 85.0 g of each reactant? 8, 8 SO, + 16 H,S 3 Sg + 16 H,0 mass of Sg: g F TOOLS x10
Consider the reaction. Pb(SO4)2+2Zn⟶2ZnSO4+PbPb(SO4)2+2Zn⟶2ZnSO4+Pb If 0.451 mol0.451 mol of zinc reacts with excess lead(IV) sulfate, how many grams of zinc sulfate will be produced in the reaction?
4 NH3 + 5 O 2 -----> 4 NO + 6 H2O HOW MANY MOLES OF OXYGEN (O2) ARE NEEDED TO REACT WITH 51.12 GRAMS OF AMMONIA(NH3) BY THIS REACTION ? NH3 MOLAR MASS = 17.04g/mol 2 C4H10+13 O2 --------------> 8 CO2+ 10H2O HOW MANY GRAMS OF WATER (H2O) ARE PRODUCED IF 100.0 MOLES OF C4H10 ARE USED? H2O MOLAR MASS = 18.02 G /MOL
Copper metal reacts with nitric acid according the equation below 3 Cu (s) +8 HNO 3(aq) -...m+3 Cu^ 2+ (aq)+2NO (g) +6 NO 3 (aq)+4 H 2 O 0 What mass of NO (g) will be produced if 8.96 g of copper are reacted wtih excess nitric acid. Be sure to include units.
A compound is composed of the elements, carbon, hydrogen, and chlorine only. Combustion of the compound produces CO2, H2O, and HClC?H?Cl? + O2 ➝ CO2 + H2O + HCl Combustion of a 10.000 g sample of the compound produces the products shown in the table below. Product Mass (grams) CO2 19.549 H2O 5.502 HCl 4.049 Determine the empirical formula for the compound
CuSO4•5H2O what is molar mass g/ml?
According to the following reaction, how many grams of water are produced in the complete reaction of 26.4 grams of nitrogen monoxide? 2NO(g)+2H2(g)---->N2(g)+2H2O(l) ____grams of H2O
O 000 How many grams of HCl can react with 0.750 g of Al(OH)3 according the following balanced equation? Molar masses: Al(OH)3= 78.01 g, AICI3= 133.33 g, HCI= 36.46 g Al(OH)3(s) + 3 HCI (aq) --> AICI3(aq) + 3 H2O 3.85 g 1.05 g 0.0288 g 1.32 g
Consider the following chemical reaction: Al2O3 (s) + 6HCl(aq) ---------->2AlCl3(aq) + 3H2O(l) How moles of AlCl3 are produced if 1.20 g of hydrochloric acid reacts with aluminum oxide? HCl =36.45 g/mole
Lithium reacts with nitrogen to form lithium nitride. 6 Li(s) + N2(g) → 2 Li3N(s) In one experiment 3.0 mole of Li is combined with 1.0 mole of N2. How much N2 is present after the complete reaction? 0.33 mol 0.67 mol 0.5 mol