The equilibrium constant of a reaction is 1.12e+02 at 312 K and 2.02e+03 at 431 K....
The equilibrium constant of a reaction is 1.12e+02 at 312 K and 2.02e+03 at 431 K. Determine the following for this reaction: Ho= 11.37 Incorrect: Your answer is incorrect. kJ/mol So= J/mol-K What is the value of the equilibrium constant at 372 K? K=
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The equilibrium constant of a reaction is 1.12e+02 at 312 K and
2.02e+03 at 431 K....
What is the value of the equilibrium constant, K, for an equilibrium reaction occurring at 58.0...
What is the value of the equilibrium constant, K, for an equilibrium reaction occurring at 58.0 degrees Celsius given that the value of deltaS is 126.98 J/mol and the value of deltaH is 176.93 kJ/mol?
At a certain temperature, the equilibrium constant K for the following reaction is 807.; N2(g) +...
At a certain temperature, the equilibrium constant K for the following reaction is 807.; N2(g) + O2(g) = 2 NO(g) Use this information to complete the following table. There will be very little N2 and 02. Suppose a 7.0 L reaction vessel is filled with 1.7 mol of N2 and 1.7 mol of 02. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little NO. x o ? Neither of...
The equilibrium constant K for a certain reaction was measured as a function of temperature (in...
The equilibrium constant K for a certain reaction was measured as a function of temperature (in Kelvin). A plot of ln(K) versus 1/T for this reaction gives a straight line with a slope of 1.352 times 10^4 K and a y-intercept of -14.51. Determine the value of Delta H degree for this reaction -120.6 kJ/mol -164.7 kJ/mol -112.4 kJ/mol -176.7 kJ/mol none of the above
part 1 Calculate the equilibrium constant at 184 °C for a reaction that has a standard...
part 1 Calculate the equilibrium constant at 184 °C for a reaction that has a standard enthalpy of reaction, ΔH° = 30.2 kJ/mol and an equilibrium constant, K = 0.0603 at 10.6 °C. R = 8.314472 J⋅mol−1⋅K−1. Report your answer to THREE significant figures. part 2 The standard enthalpy of reaction (i.e. ΔH°) for a particular reaction is −31.7 kJ/mol. At 24.9 °C the equilibrium constant for the reaction is 3.96 × 10−2. Calculate the temperature (in °C) at which...
2NO(g)02(g)2NO2(g) AH° =-114.2 kJ and AS° =-146.5 J/K The equilibrium constant for this reaction at 321.0...
2NO(g)02(g)2NO2(g) AH° =-114.2 kJ and AS° =-146.5 J/K The equilibrium constant for this reaction at 321.0 K is Assume that AH° and AS° are independent of temperature
Determine the equilibrium constant for the following reaction at 667 K HCN(g) + 2 H2(g) -...
Determine the equilibrium constant for the following reaction at 667 K HCN(g) + 2 H2(g) - CH3NH2(g) AH° = -132.0 kJ; AS = -250.0 J/K A) B) C) D) E) 6.33E+08 1.90E+08 2.71E-11 -1.00E-11 1.90E-03
Consider the reaction SnO2(s) + 2C(graphite) + 2Cl2(g) SnCl4(l) + 2CO(g) Determine the following at 298...
Consider the reaction SnO2(s) + 2C(graphite) + 2Cl2(g) SnCl4(l) + 2CO(g) Determine the following at 298 K: Ho = -186.13 Correct: Your answer is correct. kJ/mol So = 144.75 Correct: Your answer is correct. J/mol-K Go = 229.04 Incorrect: Your answer is incorrect. kJ/mol What is log K at 298K (log K = ln K/2.3026)? log K = 40.15 Correct: Your answer is correct. (Hint log K = (ln K)/2.3026) Assume that Ho and So are temperature independent to determine...
Calculate the equilibrium constant at 177 °C for a reaction that has a standard enthalpy of...
Calculate the equilibrium constant at 177 °C for a reaction that has a standard enthalpy of reaction, ΔH° = 21.3 kJ/mol and an equilibrium constant, K = 0.0612 at 40.5 °C. R = 8.314472 J⋅mol−1⋅K−1. Report your answer to THREE significant figures.
6) Distrubuting Equilibrium a) The equilibrium constant, K, for the following reaction is 10.5 at...
6) Distrubuting Equilibrium a) The equilibrium constant, K, for the following reaction is 10.5 at 350 K 2CH2Cl2(g)CH4(g + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.32x10-2 M CH2C2, 0.172 M CH4 and 0.172 M CCI4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 9.58x102 mol of CH4(g is added to the flask? CH2Cl2l [CH4 [CCI4] b) The equilibrium constant, K, for the...
The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K. CO(g) + Cl2(g)...
The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K. CO(g) + Cl2(g) COCl2(g) If AH° for this reaction is -108 kJ, what is the value of Kp at 716 K? Ko For the reaction S(s,rhombic) + 2CO(g)- SO2(g) + 2C(s,graphite) AH° = -75.8 kJ and AS° = -167.6 J/K The equilibrium constant for this reaction at 305.0 K is Assume that AHⓇ and AS are independent of temperature.
At a certain temperature, the equilibrium constant K for the following reaction is 807.; N2(g) + O2(g) = 2 NO(g) Use this information to complete the following table. There will be very little N2 and 02. Suppose a 7.0 L reaction vessel is filled with 1.7 mol of N2 and 1.7 mol of 02. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little NO. x o ? Neither of...
The equilibrium constant K for a certain reaction was measured as a function of temperature (in Kelvin). A plot of ln(K) versus 1/T for this reaction gives a straight line with a slope of 1.352 times 10^4 K and a y-intercept of -14.51. Determine the value of Delta H degree for this reaction -120.6 kJ/mol -164.7 kJ/mol -112.4 kJ/mol -176.7 kJ/mol none of the above
2NO(g)02(g)2NO2(g) AH° =-114.2 kJ and AS° =-146.5 J/K The equilibrium constant for this reaction at 321.0 K is Assume that AH° and AS° are independent of temperature
Determine the equilibrium constant for the following reaction at 667 K HCN(g) + 2 H2(g) - CH3NH2(g) AH° = -132.0 kJ; AS = -250.0 J/K A) B) C) D) E) 6.33E+08 1.90E+08 2.71E-11 -1.00E-11 1.90E-03
6) Distrubuting Equilibrium a) The equilibrium constant, K, for the following reaction is 10.5 at 350 K 2CH2Cl2(g)CH4(g + CCl4(g) An equilibrium mixture of the three gases in a 1.00 L flask at 350 K contains 5.32x10-2 M CH2C2, 0.172 M CH4 and 0.172 M CCI4. What will be the concentrations of the three gases once equilibrium has been reestablished, if 9.58x102 mol of CH4(g is added to the flask? CH2Cl2l [CH4 [CCI4] b) The equilibrium constant, K, for the...
The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K. CO(g) + Cl2(g) COCl2(g) If AH° for this reaction is -108 kJ, what is the value of Kp at 716 K? Ko For the reaction S(s,rhombic) + 2CO(g)- SO2(g) + 2C(s,graphite) AH° = -75.8 kJ and AS° = -167.6 J/K The equilibrium constant for this reaction at 305.0 K is Assume that AHⓇ and AS are independent of temperature.
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