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· The first step in processing these ores involves "roasting" the ore in air to produce the metal Assume that air contains 23 O2 by mass and that the density of air at 25°C is 1.2 g/L. Here is my work 1156.75g O2. Mass of O2 in 1 L of air = 23 of 1.2g = 0.276g. 0.276g of O2 are in 1 litre of air 1156.75g O2 are in (1/0.276) x

· Final mass of lamp an methanol = 84.75g Initial mass of lamp and methanol=85.10g Density of water = 1 g/cm 3 (S.H.C of water = 4.23 g-1K-1) i)Write an equation for the combustion of methanol (ii) Calculate (a) Number of moles of methanol used in this experiment (b) The heat change for this experiment (c) The heat of combustion per mole of methanol

· Archimedes When a body is immersed in a fluid it undergoes a loss in mass equivalent to the mass of fluid displaced . Loss in mass = 75g55.6= 19.4g H2O displaced Density of water = 1g/mL Therefore the object displaced 19.4mL of water = volume of the object . Relative density when kept in water = mass / volume Relative density =55.6 / 19.6mL

· Calculate molality of 2.5 g of ethanoic acid 75g of benzene

Question 1. 100 Geology Students Measure The Mass Of An Ore Sample. The Results Are Normally Distributed With A Mean Of 75g And A Standard Deviation Of 2g. Estimate The Number Of Students Reporting The Following Readings A. More Than 75g B. More Than 73g C. Between 71 And 79g D. Between 69 And 77g

· QUESTION BANK CHEMISTRY CLASS-- XII CHAPTER −−−−1 Q.1 Why is Frenkel defect defect not found in pure alkali metal halides Q.2 Although Si is an insulator then how does it behave as semiconductor upon heating Q.3 In the mineral Spinel having the formula MgAl O2 4 oxide ions are in ccp arrangement (a) What percentage of tetrahedral void is occupied by Mg 2 ions

· A ship floating on water is a great illustration of the difference between mass and density. A ship must have a density of less than 1.0 g/cm 3 (the density of water) or it will sink. Ships have a large mass because they are made of steel but because they

An object s density is represented by a ratio of its mass to volume. The units used for measurements are therefore mass per unit volume. Mass if we look from a physicist s perspective can be defined as a measure of the quantity that is inside a body excluding such factors as the volume of an object or any forces that might be acting on the object.

· Density = mass/volume So Density = 57g/29cm3 = 2.0g/cm3 The number on the calculator is 1. which is rounded to 2.0 because of significant figures.

· Divide weight by volume. 200 g / 200 cm 3 = 1 g/cm 3. Optionally change the unit. 1 g/cm 3 = 1 (1/1000 kg) / (1/) m 3 = 1000 kg/m 3. Or you can use our density calculator to make it a breeze The fastest way to find the density of an object is of course to use our density calculator. To make the calculation you ll need to know a few

· An ore contains Fe3O4 and no other iron. The iron in a 51-gram sample of the ore is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 21.9 g. What was the mass of Fe3O4 in the sample of . Chemistry. 1.630 g of iron ore

While mass is defined by F = ma in situations where density and volume of the object are known mass is also commonly calculated using the following equation as in the calculator provided m = ρ V. In the above equation m is mass ρ is density and V is volume. The SI unit for density is kilogram per cubic meter or kg/m3 while volume

40) Bauxite is an ore that contains the element aluminum. If you obtained 108 grams of aluminum from an ore sample that initially weighed 204 grams what is the mass percent of aluminum in this bauxite ore A) 52.9 B) 15.6 C) 0.53 D) 47.1 E) none of the above

Percent yield represents the ratio between what is experimentally obtained and what is theoretically calculated multiplied by 100 . #" yield" = ("actual yield")/("theoretical yield") 100 # So let s say you want to do an experiment in the lab. You want to measure how much water is produced when 12.0 g of glucose (#C_6H_12O_6#) is burned with enough oxygen.

· Reacting mass calculation Example 6a.5. The production of copper from a copper ore (a) Theoretically how much copper can be obtained from 2000 tonne of pure chalcopyrite ore formula CuFeS 2 Chalcopyrite is a copper-iron sulphide compound and one of the most important and common ores containing copper.

· The units of mass are typically grams. Mass percent is also known as percent by weight or w/w . The molar mass is the sum of the masses of all the atoms in one mole of the compound. The sum of all the mass percentages should add up to 100 . Watch for rounding errors in the last significant figure to make sure all the percentages add up.

· Final mass of lamp an methanol = 84.75g Initial mass of lamp and methanol=85.10g Density of water = 1 g/cm 3 (S.H.C of water = 4.23 g-1K-1) i)Write an equation for the combustion of methanol (ii) Calculate (a) Number of moles of methanol used in this experiment (b) The heat change for this experiment (c) The heat of combustion per mole of methanol

The Ba3(PO4)2 (molar mass = 601.93 g/mol) precipitate that formed from a salt mixture has a mass of 0.667 g. Experimental tests revealed that Na3PO4 • 12H2O (molar mass = 380.12 g/mol) was the limiting reactant in the formation of the precipitate and the BaCl2 •

The formula weight is simply the weight in atomic mass units of all the atoms in a given formula. The atomic weights used on this site come from NIST the National Institute of Standards and Technology. We use the most common isotopes. This is how to calculate molar mass (average molecular weight) which is based on isotropically weighted averages.

When t he mass of the sample is m ore than 75g the de nsity detection accuracy can meet the . requirements. References 1 Wang Xuguang. 2008. Emulsion explosives Metallurgical Industry Press

· 5 Given mass = 50.0 g volume = 22.2 cm3 Plan Place the mass and volume of the osmium metal in the density expression. D = mass = 50.0 g volume 2.22 cm3 calculator = 22.522522 g/cm3 final answer (2) = 22.5 g/cm3 Solution

What is the limiting reagent 2. Calculate the mass of water produced from the reaction of 24.0 g of H2 and 160.0 g of O2. What is the limiting reagent 3. The . Chemistry. Cryolite Na3AlF6(s) an ore used in the production of aluminum can be synthesized using aluminum oxide.

· As noted above weight refers to mass (i.e. measured on a balance). When examining the equation for each of the percent solutions above it is very important to note that in all cases the denominator refers to the solution mass or volume and not just the solvent mass or volume. Thus solution mass is the combined mass of solute and solvent and solution volume is the combined

· Reacting mass calculation Example 6a.5. The production of copper from a copper ore (a) Theoretically how much copper can be obtained from 2000 tonne of pure chalcopyrite ore formula CuFeS 2 Chalcopyrite is a copper-iron sulphide compound and one of the

· "The equation for one of the reactions in the process of turning iron ore into the metal is Fe2O3(s) 3 CO(g) -> 2 Fe(s) 3 CO2(g) If you start with 2.00 kg of each reactant what is the maximum mass of iron you can produce "At 2000g 17 moles of Fe2O3 will require 1428g CO to fully react meaning Fe2O3 should be my limiting reagent.

40) Bauxite is an ore that contains the element aluminum. If you obtained 108 grams of aluminum from an ore sample that initially weighed 204 grams what is the mass percent of aluminum in this bauxite ore A) 52.9 B) 15.6 C) 0.53 D) 47.1 E) none of the above

· 2O dissolving in deionized water to a final mass of 102.234 g. After through mixing 1.022 g of this solution were transferred to a clean dry container and diluted with deionized water to a final mass of 250.654 g. Calculate the final concentration NO 3--N and PO 4 3--P in ppb. Strategy This question involves a series of gravimetric dilutions

Question How Many Milliliters Of 6.50 M Hal(aq) Are Required To React With 6.75g Of An Ore Containing 44.0 Zn(s) By Mass This problem has been solved See the answer. How many milliliters of 6.50 M Hal(aq) are required to react with 6.75g of an ore containing 44.0 Zn(s) by mass

Here is the question "Limestone is an ore of calcium that contains a high proportion of calcium carbonate (CaCO3). Calcium carbonate reacts with hyd

· If the molecular mass of the compound is 268.16 g/ mol calculate the empirical and the molecular formula. C 16 H 16 N 2 O 2 . 7. A compound is 63.55 Ag 8.23 N and 28.24 O calculate the empirical formula. AgNO 3 . 8. A volume of a common gas used for welding has a mass of 0.856 g. An equal volume of H 2 gas has a mass of 0.0658 g.

When calculating molecular weight of a chemical compound it tells us how many grams are in one mole of that substance. The formula weight is simply the weight in atomic mass units of all the atoms in a given formula. If the formula used in calculating molar mass is the molecular formula the formula weight computed is the molecular weight.

· What is the mass percent of Fe 2 O 3 in the impure iron ore sample 86.1 Fe 2 O 3 by mass . An ionic compound MX 3 is prepared according to the following unbalanced chemical equation M X 2 → MX 3 A 0.105g sample of X 2 contains 8.92 x 10 20 molecules. The compound MX 3 consists of 54.47 X by mass.