For the reaction 2A(g) + B(s) ⇌ C(l) + 2D(g) at 700 °C, Kc = 0.00147....
For the reaction 2A(g) + B(s) ⇌ C(l) + 2D(g) at 700 °C, Kc = 0.00147. Calculate the number of moles of D present at equilibrium if a mixture of 1.77 moles of C and 1.77 moles of D is heated to 700 °C in a 5.52-L container. The answer is 0.0650 mol but not sure how to get it.
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For the reaction 2A(g) + B(s) ⇌ C(l)
+ 2D(g) at 700 °C, Kc = 0.00147....
The equilibrium constant, Kc , for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g)...
The equilibrium constant, Kc , for the following reaction is 5.10×10-6 at 548 K. NH4Cl(s) NH3(g) + HCl(g) If an equilibrium mixture of the three compounds in a 5.41 L container at 548 K contains 1.17 mol of NH4Cl(s) and 0.350 mol of NH3, the number of moles of HCl present is ( ) moles. The equilibrium constant, Kc , for the following reaction is 1.80×10-4 at 298 K. NH4HS(s) NH3(g) + H2S(g) If an equilibrium mixture of the three...
16. Enter your answer in the provided box. For the reaction H2(g) + CO2(g) ⇆ H2O(g)...
16. Enter your answer in the provided box. For the reaction H2(g) + CO2(g) ⇆ H2O(g) + CO(g) at 700°C, Kc = 0.534. Calculate the number of moles of H2 that are present at equilibrium if a mixture of 0.720 mole of CO and 0.720 mole of H2O is heated to 700°C in a 50.0−L container. _______ mol
The equilibrium constant, Kc, for the following reaction is 1.80x104 at 298 K. NH_HS(s) ==NH3(g) +...
The equilibrium constant, Kc, for the following reaction is 1.80x104 at 298 K. NH_HS(s) ==NH3(g) + H2S(g) If an equilibrium mixture of the three compounds in a 5.12 L container at 298 K contains 2.26 mol of NH4HS(s) and 0.282 mol of NH3, the number of moles of H2S present is moles. Submit Answer Retry Entire Group 7 more group attempts remaining
The equilibrium constant, Kc, for the following reaction is 1.80x10+ at 298 K. NH_HS(s) 2NH3(g) +...
The equilibrium constant, Kc, for the following reaction is 1.80x10+ at 298 K. NH_HS(s) 2NH3(g) + H2S(g) If an equilibrium mixture of the three compounds in a 6.94 L container at 298 K contains 2.82 mol of NH_HS(s) and 0.209 mol of NH3, the number of moles of H2S present is moles. Submit Answer Retry Entire Group 6 more group attempts remaining
The square in the reaction equation is an equilibrium sign. Consider the following reaction: 2NOBr(g) 2NO(g)...
The square in the reaction equation is an equilibrium
sign.
Consider the following reaction: 2NOBr(g) 2NO(g) + Br2(g) If 0.485 moles of NOBr(g), 0.623 moles of NO, and 0.470 moles of Br2 are at equilibrium in a 14.9 L container at 494 K, the value of the equilibrium constant, Kc, is The equilibrium constant, K. , for the following reaction is 7.00x10- at 673 K. NHI(s) NH3(g) + HI(g) If an equilibrium mixture of the three compounds in a 4.01...
Chapter 14, Question 37 Parameterization At 412 °C, Kn is 0.502 for the following reaction: 2A(s) B(g)C(s) 2D(g) If B g...
Chapter 14, Question 37 Parameterization At 412 °C, Kn is 0.502 for the following reaction: 2A(s) B(g)C(s) 2D(g) If B gas at 1.02 bar is injected into a container at 412 °C that contains excess A, what are the partial pressures of all gases present at equilibrium? a) Pressure of B bar the tolerance is +/-2% LINK TO TEXT b) Pressure of D bar the tolerance is +/-2% LINK TΟΤΕXΤ
A) The equilibrium constant, Kc, for the following reaction is 10.5 at 350K. 2CH2Cl2(g) <->CH4(g) +...
A) The equilibrium constant, Kc, for the following reaction is 10.5 at 350K. 2CH2Cl2(g) <->CH4(g) + CCl4(g) If an equilibrium mixture of the three gases in a 19.9 L container at 350K contains 0.416 mol of CH2Cl2(g) and 0.202 mol of CH4, the equilibrium concentration of CCl4 is B) 2SO3(g) <->2SO2(g) + O2(g) If 0.184 moles of SO3(g), 0.477 moles of SO2, and 0.234 moles of O2 are at equilibrium in a 15.0 L container at 1.23×103 K, the value...
show work please 3. Consider the following reaction where Kc 1.18 at 150K: 2HI(E)H2(g)+ 12(s) A...
show work please
3. Consider the following reaction where Kc 1.18 at 150K: 2HI(E)H2(g)+ 12(s) A reaction mixture was found to contain 0.0381 moles of HI, 0.0471 moles of H2, and 0.0364 moles of lz in a 1.00 L container. Is the reaction at equilibrium? And if not, what direction must it run in order to reach equiltibriurn? At equilibrium a 1.0-liter container was found to contain 0.20 mol of A, 0.20 mol of B, 0.40 mol of C, and...
3. (8 Pts) At 127°C, Kc = 2.6 x 10- for the reaction: 2 NH3(g) +...
3. (8 Pts) At 127°C, Kc = 2.6 x 10- for the reaction: 2 NH3(g) + N2(g) + 3 H2(g) Calculate Kp at this temperature. 4. (10 Pts) A 1.00-L flask was filled with 2.00 mol gaseous SO2 and 2.00 mol gascous NO, and heated. After equilibrium was reached, it was found that 1.30 mol gaseous NO was present. Assume that the reaction: SO2(g) + NO2(g) =SO3(g) + NO(g) occurs under these conditions. Calculate the value of the equilibrium constant,...
1- At a certain temperature, 0.820 mol of SO3 is placed in a 2.50-L container. 2SO3(g)---->2SO2(g)+O2(g)...
1- At a certain temperature, 0.820 mol of SO3 is placed in a 2.50-L container. 2SO3(g)---->2SO2(g)+O2(g) At equilibrium, 0.120 mol of O2 is present. Calculate Kc. 2- At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2(g)----->2HI(g) At this temperature, 0.300 mol of H2 and 0.300 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium? 3-Carbon disulfide is prepared by heating sulfur and charcoal....
The equilibrium constant, Kc, for the following reaction is 1.80x104 at 298 K. NH_HS(s) ==NH3(g) + H2S(g) If an equilibrium mixture of the three compounds in a 5.12 L container at 298 K contains 2.26 mol of NH4HS(s) and 0.282 mol of NH3, the number of moles of H2S present is moles. Submit Answer Retry Entire Group 7 more group attempts remaining
The equilibrium constant, Kc, for the following reaction is 1.80x10+ at 298 K. NH_HS(s) 2NH3(g) + H2S(g) If an equilibrium mixture of the three compounds in a 6.94 L container at 298 K contains 2.82 mol of NH_HS(s) and 0.209 mol of NH3, the number of moles of H2S present is moles. Submit Answer Retry Entire Group 6 more group attempts remaining
The square in the reaction equation is an equilibrium
sign.
Consider the following reaction: 2NOBr(g) 2NO(g) + Br2(g) If 0.485 moles of NOBr(g), 0.623 moles of NO, and 0.470 moles of Br2 are at equilibrium in a 14.9 L container at 494 K, the value of the equilibrium constant, Kc, is The equilibrium constant, K. , for the following reaction is 7.00x10- at 673 K. NHI(s) NH3(g) + HI(g) If an equilibrium mixture of the three compounds in a 4.01...
Chapter 14, Question 37 Parameterization At 412 °C, Kn is 0.502 for the following reaction: 2A(s) B(g)C(s) 2D(g) If B gas at 1.02 bar is injected into a container at 412 °C that contains excess A, what are the partial pressures of all gases present at equilibrium? a) Pressure of B bar the tolerance is +/-2% LINK TO TEXT b) Pressure of D bar the tolerance is +/-2% LINK TΟΤΕXΤ
show work please
3. Consider the following reaction where Kc 1.18 at 150K: 2HI(E)H2(g)+ 12(s) A reaction mixture was found to contain 0.0381 moles of HI, 0.0471 moles of H2, and 0.0364 moles of lz in a 1.00 L container. Is the reaction at equilibrium? And if not, what direction must it run in order to reach equiltibriurn? At equilibrium a 1.0-liter container was found to contain 0.20 mol of A, 0.20 mol of B, 0.40 mol of C, and...
3. (8 Pts) At 127°C, Kc = 2.6 x 10- for the reaction: 2 NH3(g) + N2(g) + 3 H2(g) Calculate Kp at this temperature. 4. (10 Pts) A 1.00-L flask was filled with 2.00 mol gaseous SO2 and 2.00 mol gascous NO, and heated. After equilibrium was reached, it was found that 1.30 mol gaseous NO was present. Assume that the reaction: SO2(g) + NO2(g) =SO3(g) + NO(g) occurs under these conditions. Calculate the value of the equilibrium constant,...
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