Consider the reaction 2N2O(g) + 3O2 (g) ⇌ 4NO2 (g). Exactly 0.0560 mol of O2 and...

Consider the reaction 2N2O(g) + 3O2 (g) ⇌ 4NO2 (g). Exactly 0.0560 mol of O2 and 0.020 mol of N2O were placed into a 500 mL flask. The equilibrium concentration of NO2 was 0.020 M. What is the value of Kc for this reaction? Report your answer to the correct number of significant figures.

Expert Solution

queen_honey_blossom answered 2 years ago

consider the reaction 4NO2(g) + O2(g) ---> 2N2O5(g) At a particular time during the reaction, nitrogen...

consider the reaction 4NO2(g) + O2(g) ---> 2N2O5(g) At a particular time during the reaction, nitrogen dioxide is being consumed at the rate of 0.0013 M/s. At what rate is molecular oxygen being consumed?

For the reaction 3O2(g) + 4NO(g)-->2N2O5(g) the rate of change in concentration of O2, delta[O2]/deltat =...

For the reaction 3O2(g) + 4NO(g)-->2N2O5(g) the rate of change in concentration of O2, delta[O2]/deltat = 0.057 mol/L.sec. What is the rate of change of NO and what is the rate of change of N2O5? Show your calculations.

Consider this reaction: 2O3(g)<--->3O2(g) ΔHrxn=-285.4 kj/mol. In which direction will the reaction shift when the following...

Consider this reaction: 2O3(g)<--->3O2(g) ΔHrxn=-285.4 kj/mol. In which direction will the reaction shift when the following stresses are combined? a.Remove ozone from the system b.Add Ar c.Decrease temperature d.Add catalyst

Consider the reaction between reactants S and O2: 2S(s)+3O2(g)→2SO3(g) 1. If a reaction vessel initially contains...

Consider the reaction between reactants S and O2: 2S(s)+3O2(g)→2SO3(g) 1. If a reaction vessel initially contains 5 molS and 9 molO2, how many moles of S will be in the reaction vessel once the reactants have reacted as much as possible? (Assume 100% actual yield.) Express your answer using two significant figures. 2. How many moles of O2 will be in the reaction vessel once the reactants have reacted as much as possible? (Assume 100% actual yield.) Express your answer...

Consider this reaction: 2CH3OH(l) + 3O2(g)2O(l) + 2CO2(g) H = –1452.8 kJ/mol a.Is this reaction endothermic...

Consider this reaction: 2CH3OH(l) + 3O2(g)2O(l) + 2CO2(g) H = –1452.8 kJ/mol a.Is this reaction endothermic or exothermic? b.H if the equation is multiplied throughout by 2? c.H if the direction of the reaction is reversed so that the products become the reactants and vice versa? What is the value of ∆H if water vapor instead of liquid water is formed as the product?

For 2N2O5(g) = 4NO2(g) + O2(g) 1. Determine, by making the appropriate graphs, whether this decomposition reaction...

For 2N2O5(g) = 4NO2(g) + O2(g) 1. Determine, by making the appropriate graphs, whether this decomposition reaction is zero, first, or second order with respect to N2O5 I found by makin the graph in excel that it was a first order reaction Now here are my questions 2. The stoichiometric coefficient for N205 in the reaction equation is 2. Depending on your answer to Problem 1, explain why the reaction order you obtained in Problem 1 is also 2, or explain...

At 800K, 2 mol of NO are mixed with 1 mol of O2. The reaction 2NO(g)...

At 800K, 2 mol of NO are mixed with 1 mol of O2. The reaction 2NO(g) + O2(g) <---> 2NO2(g) comes to equilibrium under a total pressure of 1 atm. Analysis of the system shows that 0.71 mol of oxygen are present at equilibrium. Calculate the equilibrium constant for the reaction. answers 0.64

Consider the following reaction at equilibrium. 2H2O (g) + 2SO2 (g) <--> 2H2S (g) + 3O2...

Consider the following reaction at equilibrium. 2H2O (g) + 2SO2 (g) <--> 2H2S (g) + 3O2 (g) What effect will adding more H2S have on the system? A) The reaction will shift in the direction of reactants B) The equilibrium constant will increase C) The reaction will shift in the direction of products D) The equilibrium constant will decrease E) No change will be observed Can you explain why the one that is the right answer correct and along with...

. The reaction of 2O3(g) → 3O2(g) has the experimental rate: rate = k[O3]2 [O2]—1. The...

. The reaction of 2O3(g) → 3O2(g) has the experimental rate: rate = k[O3]2 [O2]—1. The following mechanism has been proposed: 1. O3 O2 + O fast, equilibrium 2. O + O3 → 2 O2 slow (A) Identify any intermediates. (B) What is the rate law predicted by this mechanism? (C) Is the rate law predicted by the mechanism consistent with the experimental rate law? (D) How would adding a catalyst effect this reaction?

The decomposition of N2O5 is described by the following equation. 2N2O5(g) → 4NO2(g) + O2(g) If...

The decomposition of N2O5 is described by the following equation. 2N2O5(g) → 4NO2(g) + O2(g) If the rate constant is 4.50 × 10−4 s−1, what is the half-life of this reaction? × 10 s in scientific notation The reaction 2A → B is second order with a rate constant of 51.0/M·min at 24°C. (a) Starting with [A]0 = 9.30 × 10−3 M, how long will it take for [A]t = 2.90 × 10−3 M? min (b) Calculate the half-life of...

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