at 200 oC Kc = 1.4 x 10-10 for the reaction N2O(g) + NO2(g) <-> 3NO(g)....

at 200 ^oC K_c = 1.4 x 10^-10 for the reaction N₂O(g) + NO₂(g) <-> 3NO(g). If 300 ml of NO measured at 800 torr and 25 ^oC is placed in a 4.00 L container. what will be the N_²O and NO molar concentrations at equilibrium? What will be the total pressure of the mixture (in torr) at equilibrium at 25 ^oC?

14.98 Jespersen 7th Ed.

Expert Solution

Moles of No can be calculated from ideal gas law equation from

PV= nRT, n= PV/RT, P= 800Torr= 800/760 atm =1.052 atm, V= 300ml= 300/1000L=0.3L, T= 25+273= 298K, R= 0.0821 L.atm/mole.K, n= 1.052*0.3/(0.0821*298)=0.0129 moles

Molar concentration of NO= 0.0129/4=0.003225M

The reaction is 3NOßà N2O+ NO2, Kc’= 1/KC= 10¹⁰/1.4= 7.14*10⁹

since there is neither N2O nor NO2, the reaction begins only with the decomposition of NO.

Let x= concentration of N2O at equilibrium.

Hence at equilibrium [N2O]= [NO2]=x and [NO]= 0.003225-3x

Hence KC’ = 7.14*10⁹ = x²/(0.003225-3x)³

When solved using excel, x= 0.0010731855

At Equilibrium [N2O]= [NO2] =0.0010731855 and [NO] =5.4435*10-6 M

Moles at equilibrium

[N2O]= 4*0.0010731855 = [N2O] = 0.00429272

[NO]= 4*5.4435*10^-6 =2.1774*10-5 moles

Total moles= 2*0.00429272+2.1774*10^-5 = 0.00861moles

From gas law, P= nRT/V= 0.00861*0.0821*298/4= 0.053 atm =0.053*760 torr= 40.28 torr

queen_honey_blossom answered 2 years ago

At 300 K, Kc=1.65x10-10 for the reaction: N2O(g) + NO2(g) ⇄ 3NO(g) If 0.400 mol of...

At 300 K, Kc=1.65x10-10 for the reaction: N2O(g) + NO2(g) ⇄ 3NO(g) If 0.400 mol of N2O and 0.600 mol NO2 are added into a 4.00 L container, what will the concentration NO be at equilibrium?

Consider the following reaction occurring at 298 K: N2O(g)+NO2(g)⇌3NO(g) Part A Show that the reaction is...

Consider the following reaction occurring at 298 K: N2O(g)+NO2(g)⇌3NO(g) Part A Show that the reaction is not spontaneous under standard conditions by calculating ΔG∘rxn. Part B If a reaction mixture contains only N2O and NO2 at partial pressures of 1.0 atm each, the reaction will be spontaneous until some NO forms in the mixture. What maximum partial pressure of NO builds up before the reaction ceases to be spontaneous? Part C What temperature is required to make the reaction spontaneous...

Consider the following reaction between oxides of nitrogen: NO2(g)+N2O(g)?3NO(g) 1. Calculate ?G? at 800 K, assuming...

Consider the following reaction between oxides of nitrogen: NO2(g)+N2O(g)?3NO(g) 1. Calculate ?G? at 800 K, assuming that ?H? and ?S? do not change with temperature. Express your answer using two significant figures. 2.Calculate ?G? at 1000 K.

For each reaction, predict the sign and find the value of ∆S°: (a) 3NO(g) → N2O(g)...

For each reaction, predict the sign and find the value of ∆S°: (a) 3NO(g) → N2O(g) + NO2(g) (b) 3H2(g) + Fe2O3(s) → 2Fe(s) + 3H2O(g) (c) C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(g)

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...

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?

At 200°C, Kc = 1.6*10−10 for: N2O(g) + NO2(g) ⇌ 3 NO(g). If 350 mL of...

At 200°C, Kc = 1.6*10−10 for: N2O(g) + NO2(g) ⇌ 3 NO(g). If 350 mL of NO measured at 797 torr and 25.0°C is placed into a 3.00 L container, what will be the molarity of N2O at equilibrium when the reaction is heated to 200°C? what is the total equilibrium pressure, in units of torr at 200°C?

For the reaction SO3(g) + NO(g) NO2(g) + SO2(g) Kc was found to be 0.500 at...

For the reaction SO3(g) + NO(g) NO2(g) + SO2(g) Kc was found to be 0.500 at a certain temperature. A reaction mixture is prepared in which 0.130 mol NO2 and 0.130 mol of SO2 are placed in a 3.00 L vessel. After the system reaches equilibrium what will be the equilibrium concentrations of all four gases?

For the reaction SO2(g) + NO2(g) == NO(g) + SO3(g), Kc = 85.0 at 460

The reaction N2O(g) + O2(g) NO2(g) +NO(g) has ΔHº = -42.9 kJ and ΔSº = -26.1...

The reaction N2O(g) + O2(g) NO2(g) +NO(g) has ΔHº = -42.9 kJ and ΔSº = -26.1 J/K. Suppose 0.400 mol of N2O and 0.400 of O2 are placed in a 8.00 L container at 400 ºC and this equilibrium is established. What percentage of the N2O has reacted? (Note: Assume that ΔH and ΔS are relatively insensitive to temperature, so ΔHº298 and ΔSº298 are about the same as ΔHº673 and ΔSº673 respectively.) Enter your answer with 2 significant digits.

Question