Consider the first order reaction 2 N2O(g) ⟶ 2 N2 (g) + O2(g). What will [N2O]...

Consider the first order reaction 2 N2O(g) ⟶ 2 N2 (g) + O2(g). What will [N2O] be after 3 half lives when 0.25

moles N2O is placed in a 1.00-L reaction vessel?

Expert Solution

queen_honey_blossom answered 2 years ago

Consider the following reaction at 173 K: 2 N2O (g) → 2 N2 (g) + O2...

Consider the following reaction at 173 K: 2 N2O (g) → 2 N2 (g) + O2 (g) In one of your laboratory experiments, you determine the equilibrium constant for this process, at 173 K, is 6.678E+57. You are given a table of data that indicates the standard heat of formation (ΔHoform) of N2O is 82.0 kJ/mol. Based on this information, what is the standard entropy change (ΔSorxn) for this reaction at 173 K? ΔSorxn(J/K)=

The decomposition of N2O to N2 and O2 is a first-order reaction. At 730° C the...

The decomposition of N2O to N2 and O2 is a first-order reaction. At 730° C the half-life of the reaction is 3.58 × 103 min. If the initial pressure of N2O is 5.50 atm at 730° C, calculate the total gas pressure after one half-life. Assume that the volume remains constant. _____atm

The following reaction N2 (g) + O2 (g) ⇔ 2 NO (g) has a KP =...

The following reaction N2 (g) + O2 (g) ⇔ 2 NO (g) has a KP = 0.032 at a particular temperature. At that temperature, a vessel is filled with 0.040 atm of N2 (g), 0.040 atm of O2 (g) and 0.043 atm of NO (g). What is the pressure of NO (g) at equilibrium?

The reaction NO2 (g) + NO (g) ⇌ N2O (g) + O2 (g) reached equilibrium at...

The reaction NO2 (g) + NO (g) ⇌ N2O (g) + O2 (g) reached equilibrium at a certain high temperature. Originally, the reaction vessel contained the following initial concentration: [NO2]i = 0.0560 M, [NO]i = 0.294 M, [N2O] = 0.184 M, and [O2] = 0.377 M. The concentration of the NO2, the only colored gas in the mixture, was monitored by following the intensity of the color. At equilibrium, the NO2 concentration had become 0.118 M. What is the value...

The following equilibrium reaction is investigated. 2 N2O(g) + N2H4(g) ⇆ 3 N2(g) + 2 H2O(g)...

The following equilibrium reaction is investigated. 2 N2O(g) + N2H4(g) ⇆ 3 N2(g) + 2 H2O(g) When 0.10 moles of N2O and 0.25 moles of N2H4 are placed in a 10.0-L container and allowed to come to equilibrium, the equilibrium concentration of N2O is 0.0060 M. What is the equilibrium concentration of all four substances?

What is the overall order of the reaction below 2 NO(g) + O2(g) → 2 NO2(g)...

What is the overall order of the reaction below 2 NO(g) + O2(g) → 2 NO2(g) if it proceeds via the following rate expression? a) zero-order b) first-order c) second-order d) third-order e) fourth-order

For the reaction: N2(g) + 2 O2(g) ↔ 2 NO2(g), Kc = 8.3 × 10-10 at...

For the reaction: N2(g) + 2 O2(g) ↔ 2 NO2(g), Kc = 8.3 × 10-10 at 25°C. What is the concentration of N2 gas at equilibrium when the concentration of NO2 is twice the concentration of O2 gas?

PART A.Identify the proper form of the equilibrium-constant expression for the equation N2(g)+O2(g)⇌2NO(g) 1.K=[NO][N2][O2] 2.K=[NO]2[N2][O2] 3.K=[N2][O2][NO]2...

PART A.Identify the proper form of the equilibrium-constant expression for the equation N2(g)+O2(g)⇌2NO(g) 1.K=[NO][N2][O2] 2.K=[NO]2[N2][O2] 3.K=[N2][O2][NO]2 4.K=2[NO][N2][O2] PART B. The equilibrium-constant of the reaction NO2(g)+NO3(g)⇌N2O5(g) is K=2.1×10−20. What can be said about this reaction? 1.At equilibrium the concentration of products and reactants is about the same. 2.At equilibrium the concentration of products is much greater than the concentration of reactants. 3.At equilibrium the concentration of reactants is much greater than that of products. 4.There are no reactants left over once...

the reaction 2 h2o2(aq) -> 2 h2o(l) + o2(g) is first order in h2o2 and has...

the reaction 2 h2o2(aq) -> 2 h2o(l) + o2(g) is first order in h2o2 and has a rate constant of 0.00785 s- at 24C. a reation vessel contains 190ml of 25% h2o2 by mass solution (density of the solution is 1.09 g/ml). the gaseous oxygen is collected over water at 24Cas it forms. What volume of o2 forms in 146 seconds at a barometric pressure of 747.9 mmHg?

At 3748°C, K = 0.093 for the following reaction. N2(g) + O2(g) equilibrium reaction arrow 2...

At 3748°C, K = 0.093 for the following reaction. N2(g) + O2(g) equilibrium reaction arrow 2 NO(g) Calculate the concentrations of all species at equilibrium for each of the following cases. (a) 1.6 g N2 and 3.0 g O2 are mixed in a 1.3-L flask. (b) 2.0 mol pure NO is placed in a 2.1-L flask.

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