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A5.95-g sample of AgNO3 (169.87 g/mol) is reacted with excess BaCl 2 to give a precipitate...
1259 2 0 349H₂ = $.675 mol 10. A 5.95-g sample of AgNO3 is reacted with excess BaCl2 according to the equation 2AgNO3(aq) + BaCl2(aq) + 2AgCl(s) + Ba(NO3)2(aq) to give 4.48 g of AgCl. What is the percent yield of AgCl?
A 0.2150 g sample is dissolved and treated with excess AgNO3. The precipitate is filtered, washed, dried, and weighed. The mass of the product (AgCl) is 0.4587 g. What is the wt% of Cl in the original sample? The molecular weight of AgCl is 143.32 g/mol.
A 5.95-g sample of \(\mathrm{AgNO}_{3}\) is reacted with \(\mathrm{BaCl}_{2}\) according to the equation$$ 2 \mathrm{AgNO}_{3}(\mathrm{aq})+\mathrm{BaCl}_{2}(\mathrm{aq})->2 \mathrm{AgCl}(\mathrm{s})+\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) $$to give \(4.00 \mathrm{~g}\) of \(\mathrm{AgCl}\). What is the percent yield of \(\mathrm{AgCl} ?\)a) \(21.4 \%\)b) \(39.8 \%\)c) \(67.2 \%\)d) \(79.7 \%\)e) \(93.5 \%\)
Silver nitrate is reacted with excess copper (II) chloride, producing solid silver chloride precipitate. If 25.5g of silver nitrate is reacted and there is a 77.0% yield of silver chloride, how much silver was initially present? AgNO3 (s) + CuCl2 (aq) → AgCl (s) + Cu(NO3)2 (aq)
help asap please 6. Soft drink bottles are made of polyethylene terephthalate (PET), a polymer composed of carbon, hydrogen, and oxygen. If 1.9022 g PET is burned in oxygen it produces 0.6585 g H20 and 4,0216 g CO2. What is the empirical formula of PETY 7. A compound consists of only C and F. It contains 17.39% C by mass. What is the empirical formula of the compound? 8. What is the net ionic equation for the reaction of aqueous...
A student reacted 10.2 g of barium chloride with excess silver nitrate, according to the equation BaCl2(aq)+2AgNO3(aq) +2AgCl(s)+Ba(NO3)2(aq). a. What is the theoretical yield for silver chloride? b. If the student recovers 8.48 g of silver chloride, what is the percent yield for this reaction? Potassium and chlorine combine to form potassium chloride. a. How many grams of potassium chloride can be produced from 2.50 g of potassium? 2k + Cl2 → 2kci mmik= 39.10 ginol o KC1 = 74.55g/mol
Consider the reaction of FeCl2 with AgNO3 to form Fe(NO3)2 and AgCl. If 3.11 g AgNO3 is reacted with excess FeCl2 and 1.17 g of Fe(NO3)2 is ultimately isolated, what is the percent yield for the reaction?
1- For the following reaction, Na+(aq) + OH-(aq) + H+(aq) + Cl- (aq) à Na+(aq) + Cl- (aq) + H2O (l) Na+(aq) + Cl- (aq), ions not involved in the reaction, are called _________________ions. 2- For the following reaction, Na+(aq) + OH-(aq) + H+(aq) + Cl- (aq) à Na+(aq) + Cl- (aq) + H2O (l) What type of reaction is taking place? ____________________ 3- What is the mass in grams of 1.73 mol of MgBr2? __________ 4- What is the percentage composition...
1.How many grams of glucose (C6H12O6) are produced if 17.3 mol of H2O are reacted according to this balanced chemical equation? 6CO2 + 6H2O → C6H12O6 + 6O2 2. Nitroglycerin [C3H5(ONO2)3] is made by reacting nitric acid (HNO3) with glycerol [C3H5(OH)3] according to this reaction: C3H5(OH)3 + 3HNO3 → C3H5(ONO2)3 + 3H2O If 87.4 g of HNO3 is reacted with excess glycerol, what mass of nitroglycerin can be made? 3. Precipitation reactions, in which a solid (called a precipitate) is...
A 2.31 g sample of a mixture of AgNO3 and NaNO3 is treated with excess Na2S(aq). The precipitate is filtered off, dried and weighed. The dried precipitate weighs 0.47 g. What is the percentage by mass of NaNO3 in the original mixture? Your answer must be accurate to two significant digits. Keep several extra digits in your calculations and round off only at the end. Do not include the percent sign (%) as part of your answer! Molar masses (in...