What are the units of the rate constant for the following
reaction?
N2O4(g) ---> 2 NO2(g) rate = k(N2O4)
Can someone please break this down step by step?
What are the units of the rate constant for the following reaction? N2O4(g) ---> 2 NO2(g)...
The Kc for the reaction at 298 K is given N2O4(g) ⇋ 2 NO2(g) Kc = 5.9 × 10–3 What is the Kc for the following reaction? ½ N2O4(g) ⇋ NO2(g) Kc = ?
please show all steps.
find equiibrium concentration of N2O4 and NO2
Consider the following reaction: N2O4(g) = 2NO2(g), K = 0.36 at 2000°C The reaction mixture initially contains only the reactant, (N204] = 0.0220M , and no NO2.
Consider the reaction 2 NO2(g) N2O4(g) . (a) Using ΔGf N2O4(g) = 97.79 kJ/mol and ΔGf NO2(g) = 51.3 kJ/mol, calculate ΔG° at 298 K. ______ kJ (b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.45 atm and 1.55 atm, respectively. _____ kJ
Consider the following system at equilibrium: 2 NO2(g)⇄ N2O4(g) If 2.00 M NO2 is placed in a flask and allowed to react. At equilibrium, 1.80 M NO2 is present. A. Calculate the equilibrium concentration of N2O4. B. Calculate the equilibrium constant, K
The first order reaction of N2O4 to form two mole of NO2 has a rate constant k = 0.023 min–1. How long will it take the initial concentration of N2O4 to decrease to 10 % of the original value? A. 600s B. 43.5s C. 43.5min D. 435 min E. 100 min show working any please
Which statement concerning the reversible reaction 2 NO2(g) N2O4(g) is true? a. NO2 is the product of the forward reaction. b. The reverse reaction produces N2O4. c. At the start of the reaction, the forward and reverse reaction rates are equal. d. As the forward reaction progresses and more N2O4 is formed, the reverse reaction rate increases.
The equilibrium constant, Kc, for the reaction N2O4(g)⇌2NO2(g) is 5.1×10−3. If the equilibrium mixture contains [NO2] = 0.047 M , what is the molar concentration of N2O4? Express the concentration to two significant figures and include the appropriate units.
The rate constant for the second order reaction 2 NO2 ⟶ N2O4 is 2.79 M-1.min-1 at 48oC. If the initial concentration of NO2 is 1.05 M, what is the half-life?
For the reaction: 2 NO2 (g) à N2O4(g) DS0 = -175.5 J/K, DH0=-57.2 kJ (1) The DG0 is _______ kJ at 325 Celsius. (2) The reaction is ____ at 325 Celsius. A. for Spontaneous B. nonspontaneous (3) Would this reaction be spontaneous at___? A. all temperatures B. low temperature C. high temp D. never (4) Based on your answer of DG0 obtained above, solve for DG if [NO2] = 8.50 atm and [N2O4] = 0.00100 atm. Please have three significant figures...
Consider the reaction 2 NO2(g) →N2O4(g) .(a) Using ΔGfN2O4(g) = 97.79 kJ/mol and ΔGf NO2(g) = 51.3 kJ/mol, calculate ΔG° at 298 K.kJ(b) Calculate ΔG at 298 K if the partial pressures of NO2 and N2O4 are 0.25 atm and 1.30 atm, respectively.kJ