Using Appendix 2 in your textbook, at what temperature (in K) will the reaction, 2CO(g) + O2(g) --> 2CO2(g), change in spontaneity?
Using Appendix 2 in your textbook, at what temperature (in K) will the reaction, 2CO(g) +...
For the reaction 2CO(g)+O2(g)⇌2CO2(g), the value of K at a certain temperature is 1300. Calculate [CO2] at equilibrium when [CO] = 9.0×10−2 mol/L and [O2] = 0.527 mol/L
for the reaction 2CO + O2 = 2CO2 it is found that at a certain temperature the concentration are [CO] = 7.2 x 10^-4 M, [O2] = 8.1 x 10^-3 M, and [CO2] = 2.3 x 10-2 M. write out the equilibrium expression and calculate K for the reaction at this temperature? How would the equilibrium position change if CO2 was added?
Assuming that Ac is independent of temperature, calculate AH1200 for the reaction: 2CO(g) + O2(g) → 2CO2(g) AH co Chemical KkJ mol-?) U moll) -398.029 39.277 CO2(g) o2g) CO(g) n/a 28.34 -111.42 27.247 -577078.56
Using Appendix 2 in your textbook, what is the value for the standard change in Gibbs free energy (in kJ) at 25oC of the reaction: C2H4(g) + H2(g) --> C2H6(g)?
4. Calculate AG°(375 K) for the reaction 2CO(g) + O2(g) → 2CO2(g) from the values of AG°(298 K) and AH°(298 K) (found in tables) and the Gibbs-Helmholtz equation.
a) Complete the table below using data given in the Appendix of your textbook. 2 CH18 (1) + 25 O2 (g) → 16 CO2 (g) +18 H20 (1) O2(g) CO2 (g) H20 (1) C4H8 (1) -208.4 kJ/mol AH® (kJ/mol) sº (J/molK) 463.7 JK 'mol b) Calculate AG° combustion at 25°C for octane, CsH18 (1). Give your answer in kJ/mol of CH18 (1). c) Consider the reaction, 3 Fe203 (s) + 3 C(s) + 4 Fe (s) + 3 CO2 (g)...
Using values from Appendix C of your textbook, calculate the value of Keq at 298 K for each of the following reactions: Using values from Appendix C of your textbook, calculate the value of Keg at 298 K for each of the following reactions: (a) Fe3O4(s) + 4 CO(g) = 3 Fe(s) + 4 CO2(g) Keq = (b) Fe2O3(s) + 6 HCI(g) = 2 FeCl3(s) + 3 H2O(g) Keq = D . (c) 4 NH3(g) + O2(g) = 2 N2H4(9)...
Using values from Appendix C of your textbook, calculate the value of Kea at 298 K for each of the following reactions: (a) 2 SO3(g) 2 SO2(g) O2(g) Кeg (b) 2 NO(g) N2(g)02(g) Кeg (c) 2 NH3(g) N2(g) +3 H2(g) Кeg
Consider the following reaction at equilibrium. 2CO2 (g) 2CO (g) + O2 (g) ΔH° = -514 kJ Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction ________. A.) at low temperature and low pressure B.) at low temperature and high pressure C.) at high temperature and low pressure D.) in the presence of solid carbon E.) at high temperature and high pressure
Using values from Appendix C of your textbook, calculate the value of Keq at 298 K for each of the following reactions: (a) 4 NH3(g) + O2(g) 2 N2H4(g) + 2 H2O(l) Keq = . (b) CH4(g) + 4 Cl2(g) CCl4(l) + 4 HCl(g) Keq = . (c) 6 C(graphite) + 6 H2O(l) C6H12O6(s) Keq = .