To get the required equation do the following operation,
(3) + (2)/2 - (1)
N2O3 (g) -----------> NO (g) + NO2 (g)
Delta Hrxn = delta H3 + (Delta H2 / 2) - delta H1
= 33.2 + (180.4 / 2) - 83.7
= + 39.7 kJ
Since change in enthalpy of the reaction is positive, it is an example of endothermic reaction.
Calculate Delta H for the reaction N_2 O_3 (g) rightarrow NO(g) + NO_2(g) given the following...
Using the following reactions: N_2(g) + O_2(g) rightarrow 2 NO(g) Delta H = 181 kJ times 2 NO(g) + O_2 rightarrow 2 NO_2(g) Delta H = -113 kJ times 2 N_2O(g) rightarrow 2 N_2(g) + O_2(g) Delta H = -163 kJ times Determine the enthalpy change for the reaction: N_2O(g) + NO_2(g) rightarrow 3 NO(g) Delta H =
For the following equilibrium: N_2(g) + H_2(g) rightarrow NH_3(g) delta H= -386 kJ/mole Predict the direction the equilibrium will shift if: N_2 is added? H_2 is removed? NH_3 is added? NH_3 is removed? the volume of the container is decreased? the pressure is increased by adding Argon gas? the reaction is cooled? equal number of moles of H_2 and NH_3 are added? a catalyst is added The equilibrium constant for the following reaction is 5.0 at 400 degree C. CO_(g)...
Consider the production of dinitrogen pentoxide (N_2O_5) by the reaction O_3(g) + 2NO_2(g) rightarrow N_2O_5(g) + O_2(g) The rate law is given by d[N_2O_5]/dt = k[O_3][NO_2] Which of the following expressions is equivalent to d[NO_2]/dt? k[O_3] [NO_2]^1/2 -2k [O_3][NO_2] K[O_3][NO_2] -(k/2) [O_3][NO_2]
Consider the reaction 2NO_2(g) rightarrow N_2O_4 (g). Using the following data, calculate Delta G degree at 298 K. Delta G degree (NO_2(g)) = 51.84 kJ/mol, Delta G degree (N_2 O_4 (g)) = 98.28 kJ/mol. Calculate Delta G at 298 K if the partial pressures of NO_2 and N_2O_4 are 0.37 atm and 1.62 atm, respectively. Express your answer using one significant figure.
Given the following information fill in the missing values for delta H N_2(g) + O_2(g) 2NO_(g) Delta H= 180.4 kJ 1/2N_2(g) +1/2 O_2(g) rightarrow NO_(g) Delta H= _ 2NO_(g) rightarrow N_2(g) + O_2(g) Delta H= _ 2N_2(g) + 2O_2(g) rightarrow 4NO_(g) Delta H=
Given: 4 NO_2(g) + O_2(g) rightarrow 2 N_2O_5(g) delta H degree = -110.2 kJ find delta H degree for N_2O_5(g) rightarrow 2 NO_2(g) + 1/2 O_2(g) HBr, HCl, HCIO_4, KBr, and NaCl are all classified as Selected Answer: strong electrolytes. Correct Answer: strong electrolytes. What is the empirical formula for ethyl fluoride if the compound contains 49.97% carbon, 10.51% hydrogen, and 39.52% fluorine by mass? Selected Answer: C_4 H_10 F_4 Correct Answer: C_2H_5F Which of the following represent isotopes? A:...
Consider the reaction 2CO(g) + 2NO(g) rightarrow 2CO_2(g) + N_2(g) for which Delta H degree = -746.6 kJ and Delta S degree = -198.0 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.514 moles of CO(g) react under standard conditions at 298.15 K. (2) Is this reaction reactant or product favored under standard conditions? (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If...
For the reaction N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) Delta G degree = -23.6 kJ and Delta S degree = -198.7 J/K at 345 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 345 K. The standard enthalpy change for the reaction of 2.30 moles of N_2(g) at this temperature would be kJ. For the reaction 2 H_2O_2(l) rightarrow 2 H_2O(l) + O_2(g) Delta G degree = -236.9 kJ and Delta H degree =...
Given: 4 NO_2(g) + O_2 (g) rightarrow 2N_2O_5(g) DeltaH degree = - 110.2 kJ find Delta Hdegree for N_2O_5(g) rightarrow 2 NO_2 (g) + 1/2 O_2(g) 55.1 kJ 220.4 kJ -55.1 kJ -220.4 kJ
A proposed mechanism for the reaction of NO_2 and CO is 2 NO_2(g) rightarrow NO(g) + NO_3(g) (Slow, endothermic) NO_3(g) + CO(g) rightarrow NO_2(g) + CO_2(g) (Fast, exothermic) a) Write the overall reaction. b) Identify each of the following as a reactant, product, , or intermediate, NO_2, CO, NO_3, CO_2, NO. c) Draw a reaction coordinate for this reaction. Indicate on this drawing the activation energy for each step and the overall enthalpy change. d) Give a plausible rate law.