(6) (1 point) Using the data below, NO(g) + NO2(g) + N203(9) NO(g) + NO2(g) + O2(g) → N205(9) 2 NO2(g) + N20 (9) 2 NO(g...
PIOS 4. Dintrogen pentoxide, N205, decomposes as shown below: 2 N205 (g) ---> 4 NO2(g) + O2(g) The reaction is first order and a plot of the concentration of N2O5 as a function time for an experiment at 55 °C is shown below. What are (i) the half-life: and (ii) the rate constant for reaction at 55 °C? [N205) vs time 0.0200 LE 0.015 (N205 0.010 0.005 O 100 200 300 400 500 600 700 timers 5. A possible mechanism...
QUESTION 23 - For the reaction below at 298 K: 4NO (9) N20 (9) + N203 (9) AH = -192.7 kJ and AS = -308.2 J/K Which of the following statements is TRUE? AG >0 at 298K At higher temperatures, the reaction will be spontaneous At lower temperatures, the reaction will be spontAreous The reaction is spontaneous at all temperatures. None of the above are true. QUESTION 24 What is Asº at 298 K for the following reaction? 2 H2S(g)...
N2O3(g) decomposes to NO2 (g) and O2(g) according to the following balanced equation: N20 (2) $ NO2(g) + O2(g) The decomposition of N2O(g) was found to be first order at 30 °C. The half-life for the reaction was found to be 3000 s. A rigid reactor was initially filled with N2O5 to a pressure of 400 psi at 30°C. What is the total pressure (in psi) in the reactor at 30 °C after 6000 s? ANS: 850 psi
Consider the following data. N2(9) + 2 02(g) → 2 NO2(9) AH = 68.0 kJ N2(9) + 2 02(9) ► N204(9) AH = 10.0 kj Calculate AH for the dimerization of NO as shown below. 2 NO2(9) ► N204(9) k] Need Help? Read It
Given: NO (g) + O2(g) → 2 NO2 (g) AH = -114.2 kJ Calculate AH for this equation: 2 NO2(g) + NO(g) + O2 (g) Note: Your answer should be in kJ
Given: NO (g) + O2(g) +2 NO2 (g) AH = -114.2 kJ Calculate AH for this equation: 2 NO(g) + 2O2(g) →4 NO2 (g) Note: Your answer should be in kJ
Given the following data: () Cu (s) O2 (g)CuO (s) () N2 (g) + 02 (g)NO2 (g) H'--157 kJ AHo+33 kJ calculate AH for the reaction below using Hess' Law. 4 Cu (s) 2 NO2 (g)4 CuO (s) N2 (g)
The decomposition of crystalline N2O5 N2O5 (s) —> 2 NO2 (g) + 1/2 O2 (g) is an example of a reaction that is thermodynamically favored even though it absorbs heat. At 25°C we have the following values for the standard state entrapped and free energy changes of the reaction: ΔH° = +109.6 kJ/mol ΔG° = -30.5 kJ/mol a. Calculate ΔS° at 25°C b. Why is the entropy change so favorable for this reaction? Please answer and explain both questions!
You are given the following data. AH = = -286.0 kJ H2(g) + 1/2O2(g) → H20(1) N2O5(9) + H20(1) → 2 HNO3(aq) 1/2 N2(9) + 3/2 02(9) + 1/2 H2(9) AH = -77.0 kJ HNO3(1) AH = -174.0 kJ Calculate the AH for the reaction given below. 2 N2(g) + 5 O2(g) → 2 N205(9) k] Need Help? Read It Supporting Materials Periodic Table E Constants & Factors Supplemental Data
Arrange the following gases in order of decreasing standard molar entropy: N204(9), NO(g), NO2(g). Select one: O a. N204> NO > NOZ O b. N204 > NO2 > NO O C. NO2 > NO > N20. O d. NO > NO2 > N204 e. NO > N204 > NO2 Which of the following reactions will shift to the left if the volume is decreased? Select one: H2 (8) + Cl2 (8) DIL 2 HCI (8) OD b. 2 SO3 (8)...