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?

Expert Solution

initially,
[N2O] = number of mol / volume
= 0.10 mol / 10 L
=0.01 M

[N2H4] = number of mol / volume
= 0.25 mol / 10 L
=0.025 M

2 N2O(g) + N2H4(g) <-----> 3 N2(g) + 2 H2O(g)
0.01 0.025 0 0 (initial)
0.01-2x 0.025-x 3x 2x (at equilibrium)

given at equilibrium,
[N2O] = 0.01-2x = 0.0060
x = 0.002 M

equilibrium concentration will be:
[N2O] = 0.0060 M
[N2H4] = 0.025 - x = 0.025 - 0.0020 = 0.023 M
[N2] = 3x = 3*0.002 M = 0.006 M
[H2O] = 2x = 2*0.002 M = 0.004 M

queen_honey_blossom answered 2 years ago

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?

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)=

Consider the following reaction: 2 NO(g) + 2 H2(g)-->N2(g) + 2 H2O(g) (a) The rate law...

Consider the following reaction: 2 NO(g) + 2 H2(g)-->N2(g) + 2 H2O(g) (a) The rate law for this reaction is first order in H2 and second order in NO. Write the rate law. (b) If the rate constant for this reaction at 1000 K is 6.0 * 104 M-2 s-1, what is the reaction rate when 3NO4 = 0.035 M and 3H24 = 0.015 M? (c) What is the reaction rate at 1000 K when the concentration of NO is...

For the reaction N2(g) + 3 H2(g) equilibrium reaction arrow 2 NH3(g) at 25.0°C, the Kc...

For the reaction N2(g) + 3 H2(g) equilibrium reaction arrow 2 NH3(g) at 25.0°C, the Kc of the reaction is 5.4 ✕ 105 and the ΔG° is −32.7 kJ/mol. Use the given concentrations to determine the following. [N2] = 0.0027 M [H2] = 0.0045 M [NH3] = 0.20 M (a) Determine the ΔG of the reaction. (b) Determine which direction the reaction will proceed in order to reach 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...

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.

1) Consider the equilibrium reaction N2(g) + 3 H2(g) ↔ 2 NH3(g) + 91.8 kJ Using...

1) Consider the equilibrium reaction N2(g) + 3 H2(g) ↔ 2 NH3(g) + 91.8 kJ Using Le Chatelier’s Principle, Name two specific ways this equilibrium can be shifted to the right to increase production of NH3. 2) In the reaction below, NH3(g) + H2O(l) ↔ NH2 - + H3O + The equilibrium constant is 1 x 10 -34. Is this reaction likely to take place? Explain your answer.

Consider the reaction, N2(g) + 3 H2(g) → 2 NH3(g). Suppose 56 g of N2(g) reacts...

Consider the reaction, N2(g) + 3 H2(g) → 2 NH3(g). Suppose 56 g of N2(g) reacts with 18 g of H2(g). d. What is the limiting reactant? e. When the reaction is complete, how many grams of NH3(g) are produced? f. When the reaction is complete, how many grams of N2(g) remain? g. When the reaction is complete, how many grams of H2(g) remain? h. If the reaction actually produced 55 g of NH3(g), what is the percent yield?

Consider the following reaction with an equilibrium constant of 5.10 at 527oC. CO(g) + H2O(g) ⇌...

Consider the following reaction with an equilibrium constant of 5.10 at 527oC. CO(g) + H2O(g) ⇌ H2(g) + CO2(g) If [CO] = 0.150 M, [H2O] = 0.250 M, [H2] = 0.420 M, and [CO2] = 0.370 M, calculate Q. ? Consider the following reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g) Which of the following would not result in a shift towards an increase in production of SO3?pick the correct answer? a)Increase in volume b)Decrease in volume c)Increase in the amount of...

A mixture of gases is at equilibrium: 4 NO (g) → 2 N2O (g) + O2...

A mixture of gases is at equilibrium: 4 NO (g) → 2 N2O (g) + O2 (g) ∆H = -199.5 kJ (a) Does the equilibrium shift to the left or to the right when some O2 (g) is removed from the reaction mixture? (b) Does the equilibrium shift to the left or to the right when some NO (g) is added to the reaction mixture? c) In which direction does the equilibrium shift as the temperature is lowered? (d) In...

Question