please answer all :( 49. How many moles are there in 500 g indigo, C16H10N2O2, a blue dye.a.1.90 molb. 131000 molc. 1.15 X10E24 mold. 7.89 ×10E28 mol50. Calculate the number of molecules of a 2.00 g Valium, C15H13CIN20.a. 4.43 ×1OE21b. 8.19 ×10E25c. 3.28 ×10E26d. 9.03 X10E29

Mole concept: The number of molecules or atoms present in the one mole of the substance is equal to…

Answered: 49. How many moles are there in 500 g…

Chemistry: An Atoms First Approach

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Chapter5: Stoichiometry

Section: Chapter Questions

Problem 16ALQ: Consider the equation 2A + B . A2B. If you mix 1.0 mole of A with 1.0 mole of B, what amount (moles)...

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itamin B12 , cyancobalamin, is essential for human nutrition. Its molecular formula is C63H88CoN14O14P . A lack of this vita min in the diet can lead to anemia. Cyanocohalamin is the form of the vitamin found in vitamin supplements. l type='a'> What is the molar mass of cyanocobalamin to two decimal places? How many moles of cyanocohalamin molecules are present in 250 mg of cyanocobalamin? What is the mass of 0.60 mole of cyanocobalamin? How many atoms of hydrogen are in 1 .0 mole of cyanocobalamin? What is the mass of 1.0107 molecules of cyanocobalamin? What is the mass (in grams) of one molecule of cyanocobalamin?
Consider the equation 2A + B . A2B. If you mix 1.0 mole of A with 1.0 mole of B, what amount (moles) of A2B can be produced?
Consider the following reaction: 4NH3(g)4NO(g)+6H2O(g) If a container were to have 10 molecules of O2 and 10 molecules of NH3 initially, how many total molecules (reactants plus products) would be present in the container after this reaction goes to completion?
. How many atoms of carbon are present in 1 .0 g of CH4O ? How many atoms of carbon are present in 1.0 of CH3CH2OH ? How many atoms of nitrogen are present in 25.0 g of CO( NH2)2 ?
Considering your answer to Exercise 79, which type of formula, empirical or molecular, can be obtained from elemental analysis that gives percent composition?
A weighed sample of iron (Fe) is added to liquid bromine (Br2) and allowed to react completely. The reaction produces a single product, which can be isolated and weighed. The experiment was repeated a number of times with different masses of iron but with the same mass of bromine (see graph below). (a) What mass of Br2 is used when the reaction consumes 2.0 g of Fe? (b) What is the mole ratio of Br2 to Fe in the reaction? (c) What is the empirical formula of the product? (d) Write the balanced chemical equation tor the reaction of iron and bromine. (e) What is the name of the reaction product? (f) Which statement or statements best describe the experiments summarized by the graph? (i) When 1.00 g of Fe is added to the Br2, Fe is the limiting reagent. (ii) When 3.50 g of Fe is added to the Br2, there is an excess of Br2. (iii) When 2.50 g of Fe is added to the Br2, both reactanu are used up compietely. (iv) When 2.00 g of Fe is added to the Br2, 10.8 g of product is formed. The percent yield must therefore be 20.0%.
A 0.755-g sample of hydrated copper(II) sulfate CuSo4xH2O was heated carefully until it had changed completely to anhydrous copper(II) sulfate (CuSO4 ) with a mass of 0.4183 g. Determine the value of x. [This number is called the number of waters of hydration of copper(II) sulfate. It specifies the number of water molecules per formula unit ofCuSO4 in the hydrated crystal.]
Calculate the molarity of solutions prepared by dilution or calculate the quantities needed to carry out a dilution to prepare a solution of a specified concentration.
A dark brown binary compound contains oxygen and ametal. It is 13.38% oxygen by mass. Heating it moderatelydrives off some of the oxygen and gives a red binary compoundthat is 9.334% oxygen by mass. Strong heatingdrives off more oxygen and gives still another binary compound,which is only 7.168% oxygen by mass. (a) Compute the mass of oxygen that is combined with1.000 g of the metal in each of these three oxides. (b) Assume that the empirical formula of the first compoundis MO2 (where M representsthe metal). Givethe empirical formulas of the second and thirdcompounds. (c) Name the metal.

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49. How many moles are there in 500 g indigo, C16H10N202, a blue dye. c. 1.15 X10E24 mol a. 1.90 mol b. 131000 mol d. 7.89 ×10E28 mol 50. Calculate the number of molecules of a 2.00 g Valium, C15H13CIN20. a. 4.43 ×10E21 b. 8.19 ×10E25 C. 3.28 ×10E26 d. 9.03 ×10E29