the equilibrium constant for the reaction below
decreases from 20570.0 at 440.0 C to 23.0 at 900.0 c
4NO + 3O2 .....2N2O5
from this data...calculate the value of change of heat for the
reaction
The relation between the equilibrium constant and heat for
the reaction is given by Van't Hoff equation
ln(K2/K1) = H/R[1/T1-1/T2] or
log(K2/K1) = (H/(2.303*R)*(1/T1-1/T2)
K2 = 23 T2 = 1173 K
K1 = 20570 T1 = 713 K
H = value of change of heat for the reaction
log(23/20570) = (H/(2.303*8.314)*(1/713-1/1173)
The value of change of heat for the reaction, Hrxn = -102.748 KJ
the equilibrium constant for the reaction below decreases from 20570.0 at 440.0 C to 23.0 at...
The equilibrium constant for the reaction below decreases from 15830.0 at 480 0degreeC to 13.0 at 920.0degreeC. From these data, calculate the value of deltaH^0 for the reaction. 4 NO(g) + 3 O_2(g) 2 N_2 O_5 (g) Collect and Organize Given that K_1 = 15830.0 at 480.0degreeC and K_2 = 13.0 at 920.0degreeC. we are to calculate the standard enthalpy of the reaction between NO and O_2 to produce N_2O_5. Analyze We can use the following equation to solve this...
The equilibrium constant for the reaction NO(g) + O2(g) <=> 2NO2(g) decreases from 1.5 x 105 at 430ºC to 23 at 1000ºC. From these data, calculate the value of ΔHº for the reaction. ΔHº = _________ kJ/mol.
Thermodynamics Free energy and chemical equilibrium Quiz: Te equilibrium constant for the reaction N20 + 029 + 2 NO 200) Decreases from 1.5x 105 at 430 °C to 23 at 1000°C. From these data: a - calculate enthalpy change of this reaction; b- equilibrium constant at 1500 °C.
Thermodynamics Free energy and chemical equilibrium Quiz: Te equilibrium constant for the reaction N29) + O22) + 2 NO 262) Decreases from 1.5 * 109 at 430 °C to 23 at 1000°C. From these data: a-calculate enthalpy change of this reaction; b- equilibrium constant at 1500 °C.
Thermodynamics Free energy and chemical equilibrium Quiz: Te equilibrium constant for the reaction Na + O2 + 2 NO 200 Decreases from 1.5-10 at 430 °C to 23 at 1000°C. From these data: a - calculate enthalpy change of this reaction; b-equilibrium constant at 1500 °C
Thermodynamics Free energy and chemical equilibrium Quiz: Te equilibrium constant for the reaction N20 +020) + 2 NO 262 Decreases from 1.5 x 103 at 430 °C to 23 at 1000°C. From these data: a-calculate enthalpy change of this reaction; b-equilibrium constant at 1500 °C.
3. If the equilibrium constant for a chemical reaction decreases as the temperature is increases from room temperature to 100 degrees C, would the reaction be exothermic of endothermic? Why?
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
Hello, please help thank you Thermodynamics Free energy and chemical equilibrium Te equilibrium constant for the reaction N2 + O2 2 NO 20 Decreases from 1.5x 103 at 430 °C to 23 at 1000°C. From these data: a - calculate enthalpy change of this reaction; b- equilibrium constant at 1500 °C.
Using data from Appendix C in the textbook, write the equilibrium-constant expression and calculate the value of the equilibrium constant and the free-energy change for these reactions at 298 K . A) NaHCO3(s) ⇌ NaOH(s)+CO2(g) What is the free-energy change for this reaction at 298 K? Express the free energy in kilojoules to one decimal place. B) 2HBr(g)+Cl2(g) ⇌ 2HCl(g)+Br2(g) Which is the equilibrium-constant expression for this reaction? K=P2HClPBr2P2HBrPCl2 K=P2HBrPCl2 K=P2HBrPCl2P2HClPBr2 K=PHClPBr2PHBrPCl2 C) 2SO2(g)+O2(g) ⇌ 2SO3(g) Which is the equilibrium-constant...