What is the value of ∆Horxn for the reaction shown below?
2 NO(g) + ½ O2(g) → N2O3(g) ∆Horxn = ???
ΔHf°(N2O3(g)) = 91.2 kJ/mol
ΔHf°(NO(g)) = 90.3 kJ/mol
What is the value of ∆Horxn for the reaction shown below? 2 NO(g) + ½ O2(g)...
1.For the reaction at equilibrium 2 SO3↔ 2 SO2 + O2 (∆Horxn= 198 kJ/mol), if we increase the reaction temperature, the equilibrium will (1 point ) * No shift None of the above Question lacks sufficient information Shift to the right 2. For the equilibrium reaction 2 SO2(g) + O2(g) ↔ 2 SO3(g), ∆Horxn = -198 kJ/mol. Which one of these factors would cause the equilibrium constant to increase? (1 point ) * Add a catalyst Decrease the temperature None...
Find the enthalpy change for the reaction CS2(l) + 3 O2(g) → CO2(g) + 2 SO2(g) when: C(s) + O2(g) → CO2(g) ΔHf = -393.5 kJ/mol S(s) + O2(g) → SO2(g) ΔHf = -296.8 kJ/mol C(s) + 2 S(s) → CS2(l) ΔHf = 87.9 kJ/mol
Consider the following reaction:
C2H2 (g)+ 52 O2 (g) ® 2 CO2 (g) +
H2O
(g)
Given ΔHf° of CO2 (g) = -393.5
KJ/mol, ΔHf° H2O (g) = -241.8
KJ/mol, and ΔHf° for
C2H2 (g) = 227.4
KJ/mol, calculate ΔHrxn° for this
reaction.
How many KJ of heat is released when 0.440 kg of carbon dioxide
produced?
Determine the ∆Go for the following reaction if given ∆Horxn= -393.5 kJ and ∆Sorxn = 3.05 J/K at 298 K. Is the reaction spontaneous? Explain. C(s) + O2 (g) ---> CO2 (g)
The combustion reaction of ethane is as follows. C2H6(g) + 7/2 O2(g) → 2 CO2(g) + 3 H2O(l) Using Hess's law and the reaction enthalpies given below, find the change in enthalpy for this reaction. reaction (1): C(s) + O2(g) → CO2(g) ΔH = −393.5 kJ/mol reaction (2): H2(g) + 1/2 O2(g) → H2O(l) ΔH = −285.8 kJ/mol reaction (3): 2 C(s) + 3 H2(g) → C2H6(g) ΔH = −84.0 kJ/mol
The thermochemical equation for the reaction is shown below: 4 Al(s) + 3 O2(g) → 2 Al2O3(s) AH = -3352 kJ How much heat is released when 12.1 g of Al react with O2(g) at 25 °C and 1 atm? 0 - 104 kJ 0 -3.59 x 105 kJ -1.50 x 103 kJ O-376 kJ A 77.0-mL sample of a 0.203 M potassium sulfate solution is mixed with 55.0 mL of a 0.226 M lead(II) nitrate solution and this reaction...
The reaction: 2 Cl2(g) + 2 H2O(g) ➝ O2(g) + 4 HCl(g) has ΔG° = +11.2 kJ/mol and ΔH° = +114.4 kJ/mol at 800 K. a) What is the numerical value of the equilibrium constant for this reaction at 800 K? b) What is the numerical value of ΔG for the reaction in a vessel containing 3.6 bar Cl2, 1.4 bar H2O, 0.20 bar O2, and 0.50 bar HCl at 800 K?
Determine ΔrH° for the following reaction, 2 NH3(g) + 5/2 O2(g) → 2 NO(g) + 3 H2O(g) given the thermochemical equations below. N2(g) + O2(g) → 2 NO(g) ΔrH° = +180.8 kJ/mol-rxn N2(g) + 3 H2(g) → 2 NH3(g) ΔrH° = –91.8 kJ/mol-rxn2 2H2(g) + O2(g) → 2 H2O(g) ΔrH° = –483.6 kJ/mol-rxn a. –1178.2 kJ/mol-rxn b. –452.8 kJ/mol-rxn c. –394.6 kJ/mol-rxn d. –211.0 kJ/mol-rxn e. +1178.2 kJ/mol-rxn
The thermochemical equation for the reaction is shown below: 4 Al(s) + 3 O2(g) → 2 Al2O3(s) ΔH = -3352 kJ How much heat is released when 12.1 g of Al react with O2(g) at 25 oC and 1 atm? Group of answer choices -3.59 × 10^5 kJ -104 kJ -1.50 × 10^3 kJ -376 kJ
Consider the reaction: 2NO(g) + Cl2(g) 2NOCl(g) Given the following table of thermodynamic data, Substance ∆Hfo (kJ/mol) So (J/molK) NO (g) 90.3 210.7 Cl2 (g) 0 223.0 NOCl (g) 51.7 261.6 Calculate ∆Horxn and ∆Sorxn and determine the temperature at which the reaction switches from being spontaneous to being non-spontaneous. Please show all work. Provide equations used. Please use correct significant figures and correct units in answers.