1-Calculate the equilibrium constant at 17 K for a reaction with ΔHrxno = 10 kJ and ΔSrxno = -100 J/K. (Don't round unil the end. Using the exponent enlarges any round-off error.)
2-Calculate the equilibrium constant at 103 K for the
thermodynamic data in the previous question.
Notice that Keq is larger at the larger temperature for
an endothermic reaction.
1-Calculate the equilibrium constant at 17 K for a reaction with ΔHrxno = 10 kJ and...
Please help with these 1. Calculate ΔG (in kJ) at 298 K for some solid ZnF2, 0.082 M Zn2+ and 0.039 M F-(aq). 2.Calculate the equilibrium constant at 45 K for a reaction with ΔHrxno = 10 kJ and ΔSrxno = -100 J/K. (Don't round unil the end. Using the exponent enlarges any round-off error. Calculate the equilibrium constant at 136 K for the thermodynamic data in the previous question. ( Problem 2)
1) Calculate the equilibrium constant at 138 K for the thermodynamic data in the previous question. Notice that Keq is larger at the larger temperature for an endothermic reaction. 2) Endothermic reaction; increase in entropy Calculate the equilibrium constant at 40 K for a reaction with ΔHrxno = 10 kJ and ΔSrxno = 100 J/K.
Incorrect = 10 kJ and Calculate the equilibrium constant at 36 K for a reaction with AH ASrxn° = 100 J/K. Mark 0.00 out of 1.00 P Flag question Answer: 2.00e-16 Question 25 Not answered Calculate the equilibrium constant at 106 K for the thermodynamic data in the previous question Marked out of 1.00 Notice that Keg is dramatically larger for a larger temperature when there is a substantial positive increase in entropy, P Flag question Answer: Question 28 Assume...
1) Calculate ΔG (in kJ) at 298 K for some solid ZnF2, 0.067 M Zn2+ and 0.070 M F-(aq). Hint given in feedback. 2) Endothermic reaction; decrease in entropy: Calculate the equilibrium constant at 24 K for a reaction with ΔHrxno = 10 kJ and ΔSrxno = -100 J/K. (Don't round unil the end. Using the exponent enlarges any round-off error.)
Given the thermodynamic data below, calculate the value of the equilibrium constant for the reaction shown at 25.0ºC H₂ (g) + I₂ (g) ⇄ 2 HI (g) Given the thermodynamic data below, calculate the value of the equilibrium constant for the reaction shown at 25.0°C H2(g) + 12 (g) = 2 HI(g) AH° = -9.48 kJ AS° = +21.79 J/K K= at 25.0°C Check
e. 2.89 Calculate the thermodynamic equilibrium constant at 25°C for a reaction for which Δσ.-2560 kJ per mol of reaction:R-8.314 J/mol K a. 5.14 ×101 42. 6.12 × 102 3.07 x 104 d) e. 4.32 x 10 -t も
For the reaction 2NO(g) + O2(g) —>2NO2(g) AH° = -114.2 kJ and AS° = -146.5 J/K The equilibrium constant for this reaction at 270.0 K is Assume that AH° and AS are independent of temperature. Submit Answer Try Another Version 3 item attempts remaining elefchces to access important values if needed for this question, Consider the reaction 2CO2(g) + 5H2(g)CH2(g) + 4H2O(g) Using the standard thermodynamic data in the tables linked above, calculate AG for this reaction at 298.15K if...
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...
A reaction has a delta H^0_Txn= -167.5 kJ/mol and delta S^0_Txn = 57.3 J/mo\ K. Calculate the equilibrium constant for the reaction. What is the difference between thermodynamic equilibrium constant and the apparent equilibrium constant?
Given the thermodynamic data below, calculate the value of the equilibrium constant for the reaction shown at 25.0ºC H₂ (g) + I₂ (g) ⇄ 2 HI (g) ΔHº = -9.48 kJ ΔSº = +21.79 J/K K = Answer at 25.0ºC