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UquimulTum ll concentrations are correct following reaction does not proceed...
Home Work Due Next Class Name: For the following reaction in a 5.0 L reaction vessel...
Home Work Due Next Class Name: For the following reaction in a 5.0 L reaction vessel and at some temperature: CO2(g) + H2(g) CO(g) H20(g) 2. Ke-0.20 at this temperature. Complete the following table (use x where appropriate): CO2 1.00 H2 2.00 со 0 H20 0 initial moles change in moles equilibrium moles equilibrium conc equilibrium conc value (no "r") Verify that your equilibrium concentrations are correct! 3. The following reaction does not proceed at room temperature (the equilibrium constant...
The air pollutant NO is produced in automobile engines from the high-temperature reaction N2(g)+O2(g)⇌2NO(g);Kc=1.7×10−3 at 2300...
The air pollutant NO is produced in automobile engines from the high-temperature reaction N2(g)+O2(g)⇌2NO(g);Kc=1.7×10−3 at 2300 K. If the initial concentrations of N2 and O2 at 2300 K are both 1.58 M, what are the concentrations of NO when the reaction mixture reaches equilibrium? Concentrations of NO= UNITS If the initial concentrations of N2 and O2 at 2300 K are both 1.58 M, what are the concentrations of N2 when the reaction mixture reaches equilibrium? Concentrations of O2= If the...
The air pollutant NO is produced in automobile engines from the high-temperature reaction: N2(g)+O2(g)⇌2NO(g)Kc=1.7×10−3. Calculate the...
The air pollutant NO is produced in automobile engines from the high-temperature reaction: N2(g)+O2(g)⇌2NO(g)Kc=1.7×10−3. Calculate the equilibrium concentrations if the initial concentrations are 2.28 M N2 and 0.56 M O2. (This N2/O2concentration ratio is the ratio found in air.) Express your answer using two significant figures. Enter your answers numerically separated by commas.
Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high...
Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N2(g) + O2(g) <--> 2NO(g) The equilibrium constant Kp for the reaction is 0.0025 at 2127°C. If a 2.00 L container is charged with 5.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, (i) what will be the equilibrium partial pressure of nitrogen, PN2, and (ii) how many grams of O2(g) are present at equilibrium?...
Problem 7: Nitric oxide, NO, is a common air pollutant produced by automobile engines and power...
Problem 7: Nitric oxide, NO, is a common air pollutant produced by automobile engines and power plants according to the reaction N2 (g)+02 (g) 2NO (g) A constant-volume reactor of 100 L is initially charged with 4 mol of N2 and 1 mol of O2 and then temperature is increased to 800 K. Estimate the equilibrium extent of the reaction if the pressure is kept constant at 1 bar (Answer: 5.567 x 10-6)
The initial concentrations or pressures of reactants and products are given for each of the following...
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (d) 2SO3 (g) ⇌ 2SO2 (g) + O2 (g) KP = 16.5; initial pressures: SO3 = 1.00 atm, SO2 = 1.00 atm, O2 = 1.00 atm (e) 2NO(g) + Cl2 (g) ⇌ 2NOCl(g) Kc = 4.6 × 104 ; [NO] = 1.00 M, [Cl2] = 1.00...
P26. (Sec. 14.4) A 3.50 L reaction vessel is initially filled with 0.125 moles of N2...
P26. (Sec. 14.4) A 3.50 L reaction vessel is initially filled with 0.125 moles of N2 and 0.115 moles of O2 at 2000 °C. What are the molar concentrations of N2, O2, and NO at equilibrium? Hint: ICE Table] N:(g) +02(g) 2NO(g) Ke 0.109 a) [N2]-0.2121 M, [02]-0.3187 M, and [NO]-0.08421 M b) [N2] -0.03086 M, [O2]-0.02801 M, and [NO] 0.0097 M c [N2]-0.09258 M, [O2]-08403 M, and [NO] 0.0291 M d) [N2] 0.01543 M, [O2]-0.01401 M, and [NO]-0.00485 M...
The initial concentrations or pressures of reactants and products are given for each of the following...
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. 2NH3(g)⇌N2(g)+3H2(g)Kc=17; [NH3] = 0.20 M, [N2] = 1.00 M, [H2] = 1.00 M (b) 2NH3(g)⇌N2(g)+3H2(g)KP=6.8×104; NH3 = 3.0 atm, N2 = 2.0 atm, H2 = 1.0 atm (c) 2SO3(g)⇌2SO2(g)+O2(g)Kc=0.230; [SO3] = 0.00 M, [SO2] = 1.00 M, [O2] = 1.00 M (d) 2SO3(g)⇌2SO2(g)+O2(g)KP=16.5; SO3 = 1.00...
if someone can help answer these questions tion 18 O out of 4 points At the...
if someone can help answer these questions
tion 18 O out of 4 points At the start of a reaction, there are 1.05 moles of NO, 0.955 moles of Bry, and 1.15 moles of NOBr in a 5.5 L reaction vessel at 727 "C. From these initial molar concentrations, decide whether the system is at equilibrium. If not, predict which direction the net reaction will proceed. (Hint: Reaction Quotient) 2NO(g) + Br2(g) + 2NOBr() Ke 0.013 Question 19 O out...
3. Nitrogen and oxygen react to produce nitric oxide according to the following equation: N2 (g)...
3. Nitrogen and oxygen react to produce nitric oxide according to the following equation: N2 (g) + O2(g) → 2 NO (g) The equilibrium constant for this reaction is 1.70 x 10-3. Suppose that 0.180 mol N2 and 0.650 mol O2 are mixed in a 4.00-L reaction vessel. What will be the concentrations of N2, 02, and NO when equilibrium is established? (Hint: assume that the amounts of N2 and O2 that react are small-less than 10% of the starting...
Home Work Due Next Class Name: For the following reaction in a 5.0 L reaction vessel and at some temperature: CO2(g) + H2(g) CO(g) H20(g) 2. Ke-0.20 at this temperature. Complete the following table (use x where appropriate): CO2 1.00 H2 2.00 со 0 H20 0 initial moles change in moles equilibrium moles equilibrium conc equilibrium conc value (no "r") Verify that your equilibrium concentrations are correct! 3. The following reaction does not proceed at room temperature (the equilibrium constant...
Problem 7: Nitric oxide, NO, is a common air pollutant produced by automobile engines and power plants according to the reaction N2 (g)+02 (g) 2NO (g) A constant-volume reactor of 100 L is initially charged with 4 mol of N2 and 1 mol of O2 and then temperature is increased to 800 K. Estimate the equilibrium extent of the reaction if the pressure is kept constant at 1 bar (Answer: 5.567 x 10-6)
P26. (Sec. 14.4) A 3.50 L reaction vessel is initially filled with 0.125 moles of N2 and 0.115 moles of O2 at 2000 °C. What are the molar concentrations of N2, O2, and NO at equilibrium? Hint: ICE Table] N:(g) +02(g) 2NO(g) Ke 0.109 a) [N2]-0.2121 M, [02]-0.3187 M, and [NO]-0.08421 M b) [N2] -0.03086 M, [O2]-0.02801 M, and [NO] 0.0097 M c [N2]-0.09258 M, [O2]-08403 M, and [NO] 0.0291 M d) [N2] 0.01543 M, [O2]-0.01401 M, and [NO]-0.00485 M...
if someone can help answer these questions
tion 18 O out of 4 points At the start of a reaction, there are 1.05 moles of NO, 0.955 moles of Bry, and 1.15 moles of NOBr in a 5.5 L reaction vessel at 727 "C. From these initial molar concentrations, decide whether the system is at equilibrium. If not, predict which direction the net reaction will proceed. (Hint: Reaction Quotient) 2NO(g) + Br2(g) + 2NOBr() Ke 0.013 Question 19 O out...
3. Nitrogen and oxygen react to produce nitric oxide according to the following equation: N2 (g) + O2(g) → 2 NO (g) The equilibrium constant for this reaction is 1.70 x 10-3. Suppose that 0.180 mol N2 and 0.650 mol O2 are mixed in a 4.00-L reaction vessel. What will be the concentrations of N2, 02, and NO when equilibrium is established? (Hint: assume that the amounts of N2 and O2 that react are small-less than 10% of the starting...
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