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Question 2: Consider the production of bromobenzene from benzene and bromine The reaction mixture contains 45.7...
Consider the combination reaction between aluminum metal and liquid bromine (d = 3.1028 g/mL). Also consider that you h...
Consider the combination reaction between aluminum metal and liquid bromine (d = 3.1028 g/mL). Also consider that you have 38.4 g of aluminum metal and 40.6 g of bromine liquid. For this reaction AHrxn = -526 kJ/mol. If you were able to measure 15.5 kJ of heat being dissipated from this reaction, what would you expect to be the percent yield based on the heat generated? Hint: Find the limiting reagent before calculating the theoretical yield of the reaction.
Calculate the number of moles of acetic anhydride present in the reaction mixture. c. w d....
Calculate the number of moles of acetic anhydride present in the reaction mixture. c. w d. Based on the number of moles of each reactant and the stoichiometry of the reaction, determine the limiting reactant in the preparation. Calculate the theoretical yield of the preparation, based on the number of moles of limiting reactant present. e. Calculate the percent yield of the preparation. f. Preparation of Aspirin Page 86 6. Limiting reactant 3. Following the procedure described in this experiment,...
i need help on question 1 to 4 1. What is the difference between a simple...
i need help on question 1 to 4
1. What is the difference between a simple ion and a complex lon? Give an example (not listed in this experiment) of each. 2. What do we typically call the portion of a synthetic reaction in which we are focused on isolating the pure compound from the reaction mixture? 3. What determines the theoretical yield of any reaction? 4. Consider the following reaction: 2A + B + 3C + D (MM(A) =...
21. [08 pts.] Consider the above reaction for preparation of t-butyl chloride (Mw. 92.57 gmol) fr...
please answer the following question. thankyou
21. [08 pts.] Consider the above reaction for preparation of t-butyl chloride (Mw. 92.57 gmol) from t-butyl alcohol (Mw. = 74.12 gimo) and hydrochloric acid (Mw = 36.46 g/mol) that you did in the lab. 7.0 gt-butyl alcohol reacted with 5.0 g hydrochloric acid to produce experimentally 7.0 gt-butyl chloride What is the limiting reactant? Calculate theoretical yield . Calculate percent yield 22. [03 pts.] A slightly polar organic compound distributes between diethyl ether...
1. Consider the following reaction: 1.00 g 20.0 mL 6.00 M 14.0 g a) Which substance...
1. Consider the following reaction: 1.00 g 20.0 mL 6.00 M 14.0 g a) Which substance is the limiting reactant? b) What is the theoretical yield of the complex formed in the reaction? c) If 10.0 g of the complex was obtained from the reaction, what is the percent yield? 2. Draw the structures for the Al(C204)3 ion and the Cu(C204) ion
13. Consider 28 g O2 mixed with 4.8 g H2 according to this reaction: H2 + ...
13. Consider 28 g O2 mixed with 4.8 g H2 according to this reaction: H2 + O2 = H2O a.) Balance the reaction? b.) Find the limiting reactant? c.) What is the theoretical yield (in grams)? d.) What is the percent yield if 3.4 g H2O are obtained?
Limiting Reactants, Excess Reactant, and % Yield Name H2+Cl2HCI A gaseous mixture containing 7.5 g of H; gas and 9....
Limiting Reactants, Excess Reactant, and % Yield Name H2+Cl2HCI A gaseous mixture containing 7.5 g of H; gas and 9.00 g of Cl2 gas react to form hydrogen chloride gas. а) Which is the limiting reactant? If all the limiting reactant is consumed, how many grams of HCl are produced? How many grams of excess reactant remain un-reacted? b) c) Cl2+3F22CIF Chlorine reacts with fluorine to form gaseous chlorine trifluoride. You start with 50.0g of chlorine and 95.0g of fluorine....
Part 4 Consider the reaction: Cu_2O(s) + C(s) rightarrow 2 Cu (s) + CO(g) When 11.5...
Part 4
Consider the reaction: Cu_2O(s) + C(s) rightarrow 2 Cu (s) + CO(g) When 11.5 g of C are allowed to react with 114.5 g of Cu_2 O, 87.4 g of Cu are obtained. Find the limiting reactant, theoretical yield, and percent yield.
for the first question, simple formula is referring to empircial formula 1. The compound thiophene contains...
for
the first question, simple formula is referring to empircial
formula
1. The compound thiophene contains carbon, hydrogen and sulfur. When a sample weighing 2.450 g is subjected to complete combustion analysis with oxygen, 5.126 g of carbon dioxide and 1.049 g of water are produced. What is the simplest formula of thiophene? 2. When zinc metal reacts with copper(II) nitrate, zinc(II) nitrate and copper metal are the products. How many grams of zinc metal are required to react completely...
Bromine monochloride is synthesized using the reaction Br_(g) + Cl2(g) = 2 BrCl(g) Kp = 1.1...
Bromine monochloride is synthesized using the reaction Br_(g) + Cl2(g) = 2 BrCl(g) Kp = 1.1 x 10-4 at 150 K A 190.0 L flask initially contains 1.078 kg of Br, and 1.068 kg of Cl.. Calculate the mass of BrCl,, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCI: g What is the percent yield of BrCl? percent yield:
Consider the combination reaction between aluminum metal and liquid bromine (d = 3.1028 g/mL). Also consider that you have 38.4 g of aluminum metal and 40.6 g of bromine liquid. For this reaction AHrxn = -526 kJ/mol. If you were able to measure 15.5 kJ of heat being dissipated from this reaction, what would you expect to be the percent yield based on the heat generated? Hint: Find the limiting reagent before calculating the theoretical yield of the reaction.
Calculate the number of moles of acetic anhydride present in the reaction mixture. c. w d. Based on the number of moles of each reactant and the stoichiometry of the reaction, determine the limiting reactant in the preparation. Calculate the theoretical yield of the preparation, based on the number of moles of limiting reactant present. e. Calculate the percent yield of the preparation. f. Preparation of Aspirin Page 86 6. Limiting reactant 3. Following the procedure described in this experiment,...
i need help on question 1 to 4
1. What is the difference between a simple ion and a complex lon? Give an example (not listed in this experiment) of each. 2. What do we typically call the portion of a synthetic reaction in which we are focused on isolating the pure compound from the reaction mixture? 3. What determines the theoretical yield of any reaction? 4. Consider the following reaction: 2A + B + 3C + D (MM(A) =...
please answer the following question. thankyou
21. [08 pts.] Consider the above reaction for preparation of t-butyl chloride (Mw. 92.57 gmol) from t-butyl alcohol (Mw. = 74.12 gimo) and hydrochloric acid (Mw = 36.46 g/mol) that you did in the lab. 7.0 gt-butyl alcohol reacted with 5.0 g hydrochloric acid to produce experimentally 7.0 gt-butyl chloride What is the limiting reactant? Calculate theoretical yield . Calculate percent yield 22. [03 pts.] A slightly polar organic compound distributes between diethyl ether...
1. Consider the following reaction: 1.00 g 20.0 mL 6.00 M 14.0 g a) Which substance is the limiting reactant? b) What is the theoretical yield of the complex formed in the reaction? c) If 10.0 g of the complex was obtained from the reaction, what is the percent yield? 2. Draw the structures for the Al(C204)3 ion and the Cu(C204) ion
Limiting Reactants, Excess Reactant, and % Yield Name H2+Cl2HCI A gaseous mixture containing 7.5 g of H; gas and 9.00 g of Cl2 gas react to form hydrogen chloride gas. а) Which is the limiting reactant? If all the limiting reactant is consumed, how many grams of HCl are produced? How many grams of excess reactant remain un-reacted? b) c) Cl2+3F22CIF Chlorine reacts with fluorine to form gaseous chlorine trifluoride. You start with 50.0g of chlorine and 95.0g of fluorine....
Part 4
Consider the reaction: Cu_2O(s) + C(s) rightarrow 2 Cu (s) + CO(g) When 11.5 g of C are allowed to react with 114.5 g of Cu_2 O, 87.4 g of Cu are obtained. Find the limiting reactant, theoretical yield, and percent yield.
for
the first question, simple formula is referring to empircial
formula
1. The compound thiophene contains carbon, hydrogen and sulfur. When a sample weighing 2.450 g is subjected to complete combustion analysis with oxygen, 5.126 g of carbon dioxide and 1.049 g of water are produced. What is the simplest formula of thiophene? 2. When zinc metal reacts with copper(II) nitrate, zinc(II) nitrate and copper metal are the products. How many grams of zinc metal are required to react completely...
Bromine monochloride is synthesized using the reaction Br_(g) + Cl2(g) = 2 BrCl(g) Kp = 1.1 x 10-4 at 150 K A 190.0 L flask initially contains 1.078 kg of Br, and 1.068 kg of Cl.. Calculate the mass of BrCl,, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of BrCI: g What is the percent yield of BrCl? percent yield:
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