THE ACTUAL WEIGHING OF REACTANTS OFTEN PROVES IMPRACTICAL OR INCONVENIENT. THIS IS ESPECIALLY TRUE IF REACTANTS ARE GASES, LIQUIDS, OR VERY REACTIVE. HOW CAN WE DELIVER KNOWN WEIGHTS OF REACTANTS WITHOUT WEIGHING THEM FIRST? CONSIDER: HNO3 + NaOH = NaNO3 + H2O NEITHER NITRIC ACID, NOR SODIUM HYDROXIDE CAN BE WEIGHED EASILY. WHY? HOWEVER, SOLUTIONS OF KNOWN AMOUNT OF SOLUTE PER UNIT VOLUME CAN BE DELIVERED IN KNOWN VOLUME TO GIVE PRECISELY-KNOWN AMOUNTS OF REACTANTS. WHY? BECAUSE: (MOLES/LITER) X LITERS = MOLES IF YOU KNOW THE NUMBER OF MOLES CONTAINED IN ONE LITER, YOU CAN CALCULATE THE MOLES CONTAINED IN ANY MEASURED VOLUME OF THAT SOLUTION. TYPICALLY, A FLASK CALLED A VOLUMETRIC FLASK IS USED TO PREPARE A SOLUTION OF KNOWN CONCENTRATION, (MOLES SOLUTE/LITERS SOLUTION).
SOLUTE IS WEIGHED AND ADDED TO THE FLASK. THEN THE SOLVENT IS ADDED TO MAKE UP A KNOWN FIXED VOLUME OF SOLUTION. THE AMOUNT OF SOLUTE PER UNIT VOLUME SOLUTION(TYPICALLY MOLES/LITER) IS CALLED THE CONCENTRATION OF THE SOLUTION. IT HAS TO BE DEFINED QUANTITATIVELY. THIS CAN BE DONE IN SEVERAL WAYS. WE WILL USE THE DEFINITION MOST COMMONLY USED IN ANALYSIS, MOLARITY. THE MOLARITY IS GIVEN THE SYMBOL, M. IF A SOLUTION IS 1.000 M, 1.000 LITERS OF SOLUTION CONTAIN EXACTLY 1.000 MOLES OF SOLUTE. THE USEFULNESS OF THE CONCEPT REVOLVES AROUND THE FACT THAT YOU MUST KNOW HOW TO PREPARE DILUTE SOLUTIONS FROM CONCENTRATED ONES. IN MOST LABORATORIES REAGENTS ARE PURCHASED IN CONCENTRATED FORM DUE TO SHIPPING AND PACKAGING COSTS . THEY ARE RARELY USED AS DELIVERED. RATHER THEY ARE DILUTED FOR USE AS NEEDED. IF YOU EVER WORK IN A LABORATORY YOU MUST KNOW HOW TO PREPARE DILUTE SOLUTIONS FROM MORE CONCENTRATED ONES. ACS-CERTIFIED REAGENT-GRADE HCl IS SOLD IN BOTTLES CONTAINING 12.1 M SOLUTION. 8.26 mL OF CONCENTRATED HCl WHEN ADDED TO MAKE ONE LITER OF SOLUTION RESULTS IN A SOLUTION WHICH IS 0.100 M. IT IS A LITTLE EASIER TO MAKE UP SOLUTIONS OF PRECISE MOLARITY VALUES IF THE SOLUTE IS A SOLID AND CAN BE WEIGHED. SILVER NITRATE, AgNO3, IS SUCH A REAGENT. HOW MANY GRAMS OF SILVER NITRATE MUST BE ADDED TO A 100.00 mL FLASK TO PRODUCE A 0.200 M SOLUTION. Ag NO3(S) = Ag+(aq) + NO3-(aq)
The Essay on Solution Preparation And Standardization
Generally, there are two ways in preparing a solution, one is by dissolving a weighed amount of solid in a required solvent and the other is by dilution of a concentrated solution into the desired concentration. In diluting concentrated solution, the concentration of the diluted solution can be determined by standardization. To standardize a solution, we will need to perform titration. In this ...
0.200M 0.200M STRATEGY: FIND THE MOLES AgNO3 NEEDED FOR THE SOLUTION. THEN FIND WHAT THOSE MOLES WEIGH. MOLES AgNO3 = MxV = 0.200 x 0.10000 = 0.0200 0.0200 x 169.8731 = 3.3975 g WITH WHAT PRECISION DO WE NEED TO WEIGH OUT THE SILVER NITRATE? 25. Calculate the mass, in grams, of 1.12 mol CaH2. HOW DO WE FIND THE MASS IF WE KNOW THE NUMBER OF MOLES AND THE MOLECULAR FOLMULA? FROM THE MOLECULAR FORMULA WE CALCULATE THE AVERAGE MASS OF ONE MOLE, THE molar mass IN GRAMS. ONCE WE HAVE THE MOLAR MASS WE MULTIPLY THE MOLAR MASS BY THE NUMBER OF MOLES, 1.12. WE MUST KNOW THE MOLAR MASS TO MAKE THE CALCULATION. molecular mass = mass atoms in the molecule. mass Ca + 2x mass H = 40.077 + 2(1.00794) = 42.093u/molecule or = 42.093 g./mole THAT IS THE MOLAR MASS OF CALCIUM HYDRIDE IS 42.093 GRAMS/MOLE. TO CALCULATE THE MASS IN 1.12 MOLES: = (42.093 GRAMS/MOLE)(1.12 MOLES) = 47.1 g. NOTE THE 3 SIG. FIGS. 27. Calculate the number of moles corresponding to 98.6 g of nitric acid, HNO3. RECOGNIZE: MOLES = GRAMS/(GRAMS/MOLE) AGAIN WE NEED TO KNOW THE MOLAR MASS. THIS TIME WE MUST CALCULATE THE MOLAR MASS OF NITRIC ACID.
MOLAR MASS = mmass N + mmass H + 3x mmass O MOLES = 98.6g / (63.0128 g/mole) = 1.56 moles 29. Calculate the number of molecules in 4.68 mol H2O? YOU HAVE TO RECOGNIZE THAT ONE MOLE CONTAINS 6.02 x 1023 MOLECULES. MOLECULES = 4.68 moles(6.02 x 1023 molecules/mole) = 28.2 x 1023 = 2.82 x 1024 molecules. HOW MANY TOTAL ATOMS ARE IN THE ABOVE MOLECULES? 35. What is the mass per cent oxygen in the compound having the formula, HOOCCH2CH(CH3)COOH? MASS % O = [MASS O per mole/molar mass]x100 THUS, WE NEED TO KNOW THE MASS OF OXYGEN IN ONE MOLE OF MATERIAL AND THE MOLAR MASS OF THE MATERIAL. THIS CAN BE DONE GIVEN THE ATOMIC MASSES AND THE FORMULA. MASS O per mole = 4 x(15.9994) g. = 63.9976 g. Molar mass = 5x(atomic mass C) + 4x(atomic mass O) + 5 x 12.011 + 4 x 15.9994 + 8 x 1.00794 = 132.116 g/mole %O = [(mass O)/(mass/mole)] x 100 =
The Essay on Mixed Problems: Mole/Mole And Mole/Mass
Answer each of the following questions using the equation provided. BE SURE TO BALANCE EACH EQUATION BEFORE SOLVING ANY PROBLEMS. SHOW ALL WORK. 1. ___Cu + ___O2 ___CuO a. If 101 grams of copper is used, how many moles of copper (II) oxide will be formed? b. If 5.25 moles of copper are used, how many moles of oxygen must also be used? c. If 78.2 grams of oxygen react with copper, how many moles ...
=(63.9976/132.116)x100 = 48.4405 % 39. THE EMPIRICAL FORMULA OF PARA-DICHLOROBENZENE IS C3H2Cl. IF THE MOLECULAR MASS IS 147 u, WHAT IS THE FORMULA? RECOGNIZE THAT THE MOLECULAR MASS IS AN INTEGRAL MULTIPLE OF THE EMPIRICAL FORMULA MASS. 3(12.011) + 2(1.00794) + 35.453 = 73.502 u TWO TIMES THE EMPIRICAL FORMULA MASS IS EXACTLY THE MOLECULAR MASS. THIS MEANS THAT THE MOLECULAR FORMULA IS 43. Resorcinol, is composed of 65.44% C, 5.49 % H and 29.06 % O. Its molecular mass is 110 u. Determine the molecular formula. RECOGNIZE THAT YOU HAVE BEEN GIVEN THE INFORMATION NEEDED TO CALCULATE THE EMPIRICAL FORMULA. THE EMPIRICAL FORMULA MASS MULTIPLIED BY A SMALL WHOLE NUMBER WILL GIVE THE MOLECULAR MASS. GIVEN PERCENTAGE COMPOSITION DATA, PROCEED ON THE BASIS OF A 100.000 GRAM SAMPLE. THAT IS, ASSUME YOU HAVE A 100 g SAMPLE AND THAT IT CONTAINS 65.44g C, 5.49 g. H AND 29.06 g. O. FIND THE NUMBER OF MOLES OF EACH ELEMENT IN THE SAMPLE. MOLES C = 65.44 g/ (12.011 g/mole) = 5.448 MOLES H = 5.49 g./ (1.00794 g/mole) = 5.45 MOLES O = 29.06 g./ (15.9994 g./mole) = 1.816 MOLES C/MOLES O = 5.448/1.816 = 3.000 MOLES H/MOLES O = 5.45/ 1.816 = 3.00 3×12.011 + 3×1.00794 + 15.9994 = 55.056 u SINCE THE MOLECULAR MASS IS 110 u, THE [C3H3O]2 = C6H6O2 , OR THE EMPIRICAL FORMULA MULTIPLIED BY TWO.
LATER IN THE COURSE YOU WILL BE GIVEN BETTER DEVICES FOR BALANCING EQUATIONS. AT THIS POINT TRY TO BALANCE THE ELEMENTS OTHER THAN OXYGEN AND HYDROGEN FIRST AND THEN BALANCE THE OXYGEN OR HYDROGEN WITH WHAT EVER MOLECULES YOU HAVE AVAILABLE. Cl2O5 2 HClO3 NOTE BY INSPECTION THAT ADDING ONE WATER TO THE LEFT SIDE WILL PRODUCE BALANCE. ON BOTH SIDES YOU HAVE 2 Cl, 2 H AND 6 O. 2Al Al2O3 NOTE YOU NEED AN EVEN NUMBER OF OXYGENS. 4 Al + 3 O2 = 2 Al2O3 BALANCED. 61. 2 C8H18 + 25 O2 = 16 CO2 + 18 H2O jjj. How many moles of carbon dioxide are produced when 1.8 x 104 moles of octane are burned? THE STOICHIOMETRIC COEFFICIENTS TELL US: MOLES CO2/ MOLES OCTANE = 16/2 = 8/1 = 8 THAT IS, MOLES CARBON DIOXIDE = 8 X MOLES OCTANE. MOLES CARBON DIOXIDE = 8 x 1.8 x 104 = 14.4 x 104 = 1.4 x 105. 67. Kerosene is a mixture of hydrocarbons used in heating and as a jet fuel. Assume that kerosene can be represented by C14H30 and that it has a density of 0.763 g/mL. How many grams of carbon dioxide are produced by the combustion of 3.785 L of kerosene? Strategy: 1. Partially balance the equation for combustion.
The Term Paper on Ecosystem: Carbon Dioxide
Ecosystem is a community of living organisms (plants, animals and microbes) in conjunction with the nonliving components of their environment (things like air, water and mineral soil), interacting as a system. These components are regarded as linked together through nutrient cycles and energy flows. As ecosystems are defined by the network of interactions among organisms, and between organisms and ...
2. Note that you have been given the density and the volume of the kerosene. From d = m/v you can calculate the mass of the kerosene. From the mass you can calculate moles after calculating the molar mass of kerosene. 3. From the balanced equation you determine the ratio of moles carbon dioxide to kerosene. 4. From moles carbon dioxide you calculate grams carbon dioxide. C14H30 + x O2 = y H2O + 14 CO2 Note moles carbon dioxide = 14 x moles kerosene. d x v = (.763 g/mL)(3785mL) = 2.89×103 g. MOLAR MASS KEROSINE = 14x 12.011 + 30 x 1.00794 = 198.392 g/mole MOLES KEROSENE = 2.89 x 103/198.392 = 14.6 MOLES CARBON DIOXIDE = 14.00 X 14.6 = 204 204moles X 44.01g/mole = 8978 g = 8.98 KG. 73. Lithium hydroxide absorbs carbon dioxide to form lithium carbonate and water: If a reaction vessel contains 0.150 mol LiOH and 0.080 mol CO2, which compound is the limiting reagent? How many moles of the carbonate can be produced? 0.150 mol of LiOH will react with 0.075 mol of carbon dioxide. (Moles carbon dioxide)/(moles LiOH) = ?. Thus, the LiOH is the limiting reagent and all the carbon dioxide is not used up. The number of moles of the carbonate will be the same as the number of moles carbon dioxide used, 0.075. 83.a Calculate the molarity of a solution prepared from 6.00 mol HCl in 2.50 L solution. M = moles solute/liters solution = 6.00 moles/2.50 L = 87. How many mL of a 0.215 M solution are required to contain 0.0867 mol NaBr? Note M x VL = moles = 0.0867 = 0.215 x VL VL = 0.0867/.215 = 0.403 liters = 403 mL
The Essay on Carbon dioxide 7
Carbon dioxide is a gas comprising less than 0.04 % of the atmosphere.It is used by plants to make, directly or indirectly, all of the food that we eat.Increases in the concentration of carbon dioxide generally increase the growthrate of plants and decrease their water use. The concentration of carbondioxide in the atmosphere is increasing, mostly as a result of burning of coal,oil, gas and ...
