A sample of a substance with the empirical formula XCl3 weighs 0.5183 g. When it is...
A sample of a substance with the empirical formula XC1_2 weighs 0.5785 g. When it is dissolved in water and all its chlorine is converted to insoluble AgCl by addition of an excess of silver nitrate, the mass of the resulting AgCl is found to be 1.2794 g. The chemical reaction is XCI_2 + 2 AgNO_3 rightarrow 2 AgCI + X(NO_3)_2 Calculate the formula mass of XCI_2. Formula mass XCI_2 = g mol^-1 Calculate the atomic mass of X. Atomic...
A sample of a substance with the empirical formula XCl3 weighs 0.4393 g. When it is dissolved in water and all its chlorine is converted to insoluble AgCl by addition of an excess of silver nitrate, the mass of the resulting AgCl is found to be 1.1926 g. The chemical reaction is XCl3 + 3 AgNO33AgCl + X(NO3)3 (a) Calculate the formula mass of XCl3. Formula mass XCl3 = g mol-1 (b) Calculate the atomic mass of X. Atomic mass...
A 0.5711 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated as AgCI by the addition of an excess of silver nitrate. The mass of the resulting AgCl is found to be 1.2913 g. What is the mass percentage of chlorine in the original compound? 9 more group attempts remaining Submit Answer Retry Entire Group
A mixture consisting of only iron(III) chloride (FeCl3) and aluminum chloride (AlCl3) weighs 1.0397 g. When the mixture is dissolved in water and an excess of silver nitrate is added, all the chloride ions associated with the original mixture are precipitated as insoluble silver chloride (AgCl). The mass of the silver chloride is found to be 3.0178 g. Calculate the mass percentages of iron(III) chloride and aluminum chloride in the original mixture. Mass percent FeCl3 = % Mass percent AlCl3...
A 2.018-g sample of a metal bromide. MBr2, is dissolved in water and treated with excess aqueous silver nitrate. The silver bromide (AgBr) that formed weighed 2.721 g. Calculate the atomic mass of Mand identify M. (molar mass of AgBr - 187.80 g/mol)
What is the mass of insoluble silver bromide (187.77 g/mol) produced from 2.96 g of iron(III) bromide (295.55 g/mol) and aqueous silver nitrate? FeBr3(s) + AgNO3(aq) → AgBr(s) + Fe(NO3)3(aq)
Question 3 [20 points 1. Copper sulfide is produced when copper and sulfur are heated together Use the data below, obtained after the heating process, to determine the empirical formula of this compound. Molar masses (e/mol) c S 32.06. 18 points) befor 1 Mass of crucible cover copper (B) 2 Mass of crucible + cover (g) 3 Mass of copper (B) 4 Mass of crucible cover + copper sulfide at constant weight (8)40.23 S Mass of copper sulfide (8) 6...
1. A 0.4187 g sample of a pure soluble chloride compound is dissolved in water, and all of the chloride ion is precipitated as AgCl by the addition of an excess of silver nitrate. The mass of the resulting AgCl is found to be 0.9536 g. What is the mass percentage of chlorine in the original compound? ________% 2. A student determines the calcium content of a solution by first precipitating it as calcium hydroxide, and then decomposing the hydroxide...
1. The empirical formula of an unknown substance is HSO4. If the molecular weight of the substance 194 glmol, what is its molecular formula? 2. How many grams of ammonia are produced when 32g of nitrogen react with excess hydrogen? N2 3H23 2NH, 3. The empirical formula of an unknown substance is determined to be CH2. What is its molecular formula if the molecular weight is 84 gmole? 4. Nicotine has an empirical formula of CsHTN and a molecular weight...
Determine the empirical formula of a compound containing: a. 1. 48.5 gram sample containing 1.75 g carbon & 46.75 g bromine. 2. 30.9 gram sample containing 9.63 g sulfur & 21.3 g chlorine Determine the molecular formula of the following: 3. Empirical formula = CFBro & molar mass = 254.7 g/mol 4. Empirical formula = C2H8N & molar mass = 46 g/mol Determine the molecular formula for the following: 5. 74.1% carbon, 8.6% hydrogen, & 17.3% nitrogen by mass. Its...