One of the least abundant nitrogen oxides in the atmosphere is dinitrogen pentoxide. One reason concentrations of this oxide are low is that the molecule is unstable and rapidly decomposes to N2O4 and O2: 2N2O5(g)  →  2N2O4(g)  +  O2(g)    A kinetic study of the decomposition of N2O5 at a particular temperature yielded the data in the following Table. Assume that the decomposition of N2O5 is first order in N2O5. Test the validity of your assumption. Determine the value of the rate constant.

N204(g) = 2 NO2(g) Three experiments were run starting with different initial amounts of N2O4(g) ([N204]o in the table). The systems were allowed to reach equilibrium and the concentrations for each gas were measured (in units of moles/Liter). For each of the boxes below, calculate the ratios indicated by the column heading. This will show the mathematical relationship that exists between the concentrations of NO2 and N204 at equilibrium. Be sure to round to the correct number of significant figures. Exp[N204l0 [NO2][N,04] [NO,] / [N204] 2 [NO,] / [N204] [NO2]? / [N204] 1 3.7 2.92 2.2 2 3.0 2.56 1.7 3 2.3 2.15 1.2 Based on your calculations, indicate whether each statement is True (T) or False (F): v1. Each experiment started with a different initial concentration of N204. v2. The ratio ([NO2] / [N204]) is equal to a constant value. v3. The ratio (2 [NO2] / [N204]) is equal to a constant value. v 4. The ratio ([NO2]? / [N204]) is equal to a constant value. v5. Each experiment reached a…

Write the Qc, Kc, and Kp expressions for eq between H2 and N2 gas to produce NH3 and explain the difference between each. Compare the kinetic energy of the reactants to the products and state which side has greater or less kinetic energy based on the number of gas particles?

The value of KC for the thermal decomposition of hydrogen sulfide, shown below, is 2.2 × 10-4 at 1400 K. A sample of gas in which [H2S] = 5.96 M is heated to 1400 K in a sealed vessel. After chemical equilibrium has been achieved, what is the value of [H2S]? Assume no H2 or S2 was present in the original sample.

Consider the following reaction CO₂ (g) +CCL, (g) -2000L₂ (g) 2COCL Calculate A-G for this reaction at 125 °C under the following conditions Pco, 0.105 bar 0.175 bar Poc, Pcoci,-0.735 bar A.G= 55.28 ΑΣΦ H C Previous Answers Request Answer X Incorrect; Try Again: One attempt remaining ? kJ mol

Phosphine gas (PH3), decomposes by the reaction shown below.  A total pressure of 0.64 atm of pure phosphine gas was placed in a sealed 1.00-L flask at 298 K. After equilibrium was attained, the total pressure inside the flask was found to be 0.93 atm. Calculate the mass of solid phosphorous in the flask. PH3(g)   <-->   P(s)   +   3 H2(g)

The following reaction has a Keq = 195 at 1000 K. + CH4 (g) CO (g) + 3H2(g) → H₂O(g) If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.036 M, [H₂] = 0.045 M, [H₂O] = 0.020 M, and [CH4] = 0.032 M, in which direction will a reaction occur and why? Towards products because Q = 0.38. Towards reactants because Q = 0.24. Towards products because Q = 4.1. Towards products because Q = 61. Neither direction; it is at equilibrium.

Given the following equilibrium constants at 700K, 2 N2O(g) (double arrow) 2 N2 (g) + O2(g) K1 = 8.2 x 1033NO2(g) (double arrow) 1⁄2 N2(g) + O2(g) K2 = 2.44 x 108N2O4(g) (double arrow) 2 NO2(g) K3 = 4.6 x 10-3 determine the values of the equilibrium constants for the following reaction. Show your equation-buildingprocess and your calculations. 2 N2O4(g) (double arrow) 2 N2O(g) + 3 O2(g) K =

When exposed to UV light, phosgene (COCL2) decomposes according to the reaction COCL2(g)->CO(g) + Cl2(g). All the air is removed from a flask. The flask is then filled with phosgene to a pressure of 2.8 atm and then exposed to UV light. If the temperature remains constant during the decomposition, what is the partial pressure of Cl2 (g) in the flask after the decomposition is complete, assuming 100% yield?

*** S 19. Solid ammonium hydrogen sulfide is introduced into a 2.00-L flask, and the flask is şealed. If this solid decomposes according to the equation below DAUS Ca Nothange NH4HS(s) NH3(g) + H₂S(g), Kp = 0.108 at 25°C, what is the minimum mass of ammonium hydrogen sulfide that must be present in the flask initially if equilibrium is to be established at 25°C? A) 0.917 g B) 1.37 g C) 2.74 g D) 0.581 g E) 0.452 g