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Above I have taken a>>x, b>>x because the ratio is very small that means the denominator part will be much larger than numerator part
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. Hydrogen can be extracted from natural gas according to the reaction CHa(g)+CO2 (8)2 2co(g)+2H2le)L Ko...
84. Hydrogen can be extracted from natural gas according to the reaction: CH4(8) + CO2(g) = 2 CO(g) + 2 H2(g) Ky =...
84. Hydrogen can be extracted from natural gas according to the reaction: CH4(8) + CO2(g) = 2 CO(g) + 2 H2(g) Ky = 4.5 x 102 at 825 K An 85.0-L reaction container initially contains 22.3 kg of CH4 and 55.4 kg of CO2 at 825 K. Assuming ideal gas behavior, calcu- late the mass of H, (in g) present in the reaction mixture at equi- librium. What is the percent yield of the reaction under these conditions? CaO(s) :...
Part A Constants Periodic Table Assuming ideal gas behavior, calculate the mass of NH3 (in g)...
Part A Constants Periodic Table Assuming ideal gas behavior, calculate the mass of NH3 (in g) present in the reaction mixture at equilibrium. Express your answer using two significant figures Ammonia can be synthesized according to the following reaction: N2(9) 3 H2(9)2 NH: (9) Kp 5.3 x 10 5 at 725 K A 200.0-L reaction container initially contains 1.27 kg of N2 and 0.310 kg of H2 at 725 K Submt Part B What is the percent yield of the...
uestion 16 of 16 > Bromine monochloride is synthesized using the reaction Br (8) + Cl2(g)...
uestion 16 of 16 > Bromine monochloride is synthesized using the reaction Br (8) + Cl2(g) = 2 BrCl(9) Ko = 1.1 x 10-4 at 150 K A 203.0 L flask initially contains 1.005 kg of Br, and 1.155 kg of Cl. Calculate the mass of BrCI, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of Brci: What is the percent yield of BrCl? percent yield: terms of use contact us help...
Bromine monochloride is synthesized using the reaction Br,(g) + Cl2(8) 2 BrCI(g) K, = 1.1 x...
Bromine monochloride is synthesized using the reaction Br,(g) + Cl2(8) 2 BrCI(g) K, = 1.1 x 10-4 at 150 K A 193.0 L flask initially contains 0.985 kg of Br, and 1.027 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 BrCl: 16.0424 Incorrect What is the percent yield of BrCl? % percent yield: 86.7 Incorrect
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:
Bromine monochloride is synthesized using the reaction Br2(g) + Cl2(g) = 2 BrCl(g) Kp = 1.1...
Bromine monochloride is synthesized using the reaction Br2(g) + Cl2(g) = 2 BrCl(g) Kp = 1.1 x 10-4 at 150 K A 203.0 L flask initially contains 1.070 kg of Br, and 1.115 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 BrCl: g What is the percent yield of BrCl? percent yield: %
Bromine monochloride is synthesized using the reaction Br,(g) + Cl2(g) = 2 BrCI(g) K= 1.1 x...
Bromine monochloride is synthesized using the reaction Br,(g) + Cl2(g) = 2 BrCI(g) K= 1.1 x 10- at 150 K A 194.0 L flask initially contains 0.905 kg of Br, and 1.101 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: 8 What is the percent yield of BrCl? percent yield: %
Bromine monochloride is synthesized using the reaction Br_(g) + Cl2(g) = 2 BrCl(g) K = 1.1...
Bromine monochloride is synthesized using the reaction Br_(g) + Cl2(g) = 2 BrCl(g) K = 1.1 x 10-4 at 150 K A 197.0 L flask initially contains 1.013 kg of Br, and 1.025 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: % about us Careers privacy policy terms of use contact us...
< Problem Set #5 (Ch 15) Exercise 15.83 Ammonia can be synthesized according to the following...
< Problem Set #5 (Ch 15) Exercise 15.83 Ammonia can be synthesized according to the following reaction: N2 (9) + 3 H2 (9) = 2 NH3 (9) Kp = 5.3 x 10-5 at 725 K A 200.0-L reaction container initially contains 1.27 kg of N, and 0.310 kg of H2 at 725 K Part A Assuming ideal gas behavior, calculate the mass of NH3 (in g) present in the reaction mixture at equilibrium. Express your answer using two significant figures....
84. Hydrogen can be extracted from natural gas according to the reaction: CH4(8) + CO2(g) = 2 CO(g) + 2 H2(g) Ky = 4.5 x 102 at 825 K An 85.0-L reaction container initially contains 22.3 kg of CH4 and 55.4 kg of CO2 at 825 K. Assuming ideal gas behavior, calcu- late the mass of H, (in g) present in the reaction mixture at equi- librium. What is the percent yield of the reaction under these conditions? CaO(s) :...
Part A Constants Periodic Table Assuming ideal gas behavior, calculate the mass of NH3 (in g) present in the reaction mixture at equilibrium. Express your answer using two significant figures Ammonia can be synthesized according to the following reaction: N2(9) 3 H2(9)2 NH: (9) Kp 5.3 x 10 5 at 725 K A 200.0-L reaction container initially contains 1.27 kg of N2 and 0.310 kg of H2 at 725 K Submt Part B What is the percent yield of the...
uestion 16 of 16 > Bromine monochloride is synthesized using the reaction Br (8) + Cl2(g) = 2 BrCl(9) Ko = 1.1 x 10-4 at 150 K A 203.0 L flask initially contains 1.005 kg of Br, and 1.155 kg of Cl. Calculate the mass of BrCI, in grams, that is present in the reaction mixture at equilibrium. Assume ideal gas behavior. mass of Brci: What is the percent yield of BrCl? percent yield: terms of use contact us help...
Bromine monochloride is synthesized using the reaction Br,(g) + Cl2(8) 2 BrCI(g) K, = 1.1 x 10-4 at 150 K A 193.0 L flask initially contains 0.985 kg of Br, and 1.027 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 BrCl: 16.0424 Incorrect What is the percent yield of BrCl? % percent yield: 86.7 Incorrect
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:
Bromine monochloride is synthesized using the reaction Br2(g) + Cl2(g) = 2 BrCl(g) Kp = 1.1 x 10-4 at 150 K A 203.0 L flask initially contains 1.070 kg of Br, and 1.115 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 BrCl: g What is the percent yield of BrCl? percent yield: %
Bromine monochloride is synthesized using the reaction Br,(g) + Cl2(g) = 2 BrCI(g) K= 1.1 x 10- at 150 K A 194.0 L flask initially contains 0.905 kg of Br, and 1.101 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: 8 What is the percent yield of BrCl? percent yield: %
Bromine monochloride is synthesized using the reaction Br_(g) + Cl2(g) = 2 BrCl(g) K = 1.1 x 10-4 at 150 K A 197.0 L flask initially contains 1.013 kg of Br, and 1.025 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: % about us Careers privacy policy terms of use contact us...
< Problem Set #5 (Ch 15) Exercise 15.83 Ammonia can be synthesized according to the following reaction: N2 (9) + 3 H2 (9) = 2 NH3 (9) Kp = 5.3 x 10-5 at 725 K A 200.0-L reaction container initially contains 1.27 kg of N, and 0.310 kg of H2 at 725 K Part A Assuming ideal gas behavior, calculate the mass of NH3 (in g) present in the reaction mixture at equilibrium. Express your answer using two significant figures....
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