The first order decomposition reaction of N2O5 is given as follows; N,O5 (in CCL4) –→ N;O4 (in CCL4) + ½ O2(g) Find the rate constant (k) corresponding to a 2.00 h half- life at 25°C. Calculate the half-life of the given decomposition reaction at 32°C, if the activation energy is 106 kJ/mol? (R:8.314 J/mol.K) ww w

Solve correctly please need all parts.

The equilibrium constant, Ke, for the following reaction is 1.80×10-² at 698 K. 2HI(g) H2(g) + I,(g) Calculate the equilibrium concentrations of reactant and products when 0.294 moles of HI are introduced into a 1.00 L vessel at 698 K. [HI] M [H2] M [IL] M

Nitromethane, CH3NO2 , can be used as a fuel. When the liquid is burned, the (unbalanced) reaction is mainlyCH3NO2(l) + O2(g) → CO2(g) + N2(g) + H2O(g)a. The standard enthalpy change of reaction (ΔH°van ) for the balanced reaction (with lowest whole-number coefficients) is −1288.5 kJ. Calculate ΔHf0 for nitromethane.b. A 15.0-L flask containing a sample of nitromethane is filled with O2 and the flask is heated to 100.°C. At this temperature, and after the reaction is complete, the total pressure of all the gases inside the flask is 950. torr. If the mole fraction of nitrogen (χnitrogen) is 0.134 after the reaction is complete, what mass of nitrogen was produced?

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|For the reaction at 25.0 °C: 2 SO3(g) 2 SO2 (g) + Q, (g) www. K, = 1.4 x 10-25 and G° = 141 kJ/mol At 25.0 °C, the partial pressure of So, = 10.0 atm, that of SO, is 0.00120 atm, and that of 0, is 0.00180 atm. Calculate G (in kJ) for this process. G= G° + RTINQ

For the following reaction, 0.574 moles of sodium chloride are mixed with 0.504 moles of silver nitrate. sodium chloride(aq) + silver nitrate(aq) → silver chloride(s) + sodium nitrate(aq) What is the formula for the limiting reagent? What is the maximum amount of silver chloride that can be produced? moles

Consider the following reaction: 4PC13(g) P4(g) + 6C12(g) If the initial concentration of PC13(g) is 1.5 mol/L, and "x" is the equilibrium concentration of Pa(g), what is the correct equilibrium relation а. Кс-бх7 O b. Kc=6x7/(1.0-4x)4 O c. Kc=(x)(6x)6/(1.0-4x)4 O d. Kc=(x)(6x)°/(1.5-4x)4 O e. Kc=x'/(1.0-x)4

The Naganohara Fireworks company hired you, as a new chemical engineer in town, to operate one of their reactors used in th, eir fireworks manufacturing. This batch reactor is a constant-volume reactor operated at 0oC. One of the operators then gave you the data for the decomposition of the pure gas Yoimiya-X (YX) into the product they call Amber (A). The stoichiometry of the decomposition is YX -> 2.5A. Your major task as the chemical engineer is to find a rate equation (in moles, liter, and minutes) which satisfactorily represents this decomposition.   The following data are obtained:   time, min 0 2 4 6 8 10 12 14 ∞ Partial pressure of YX, mm Hg 76 60 47.5 39 32 27.5 24 21.5 15

I need help finding the rate constant