The rate constant for the first-order decomposition of N2O5 in the reaction 2 N2O5(g) → 4 NO2(g) + O2(g) is kr = 3.38 × 10−5 s−1 at 25 °C. What is the half-life of N2O5? If the initial partial pressure of N2O5 is 500 Torr, what will its partial pressure be (i) 50 s, (ii) 20 min after initiation of the reaction?

Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: elementary reaction step 1 2 NO (g) + 0₂ (g) NO₂ (g) +O(g) 2 NO(g) + O(g) → NO₂ (g) Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Suppose also k₁ « k₂. That is, the first step is much slower than the second. 1 Note: your answer should not contain the concentrations of any intermediates. rate constant rate = k k₁ k₂ X Ś

A reaction is first order in A. If the rate constant of the reaction is 8.33 x10–3 s–1, what is the half-life (t1/2) of the reaction?

Chlorine monoxide accumulates in the stratosphere above Antarctica each winter and plays a key role in the formation of the ozone hole above the South Pole each spring. Eventually, CIO decomposes according to the equation: 2Cio(g) Cl,(g) + 0,(g) The second-order rate constant for the decomposition of ClO is 7.08×10° M-1s=1 at a particular temperature. Determine the half-life of CIO when its initial concentration is 1.11x10-8 M.

The gas phase decomposition of hydrogen peroxide at 400 °C H2O2(g)H20(g) + ½ O2(g) is second order in H2O2. In one experiment, when the initial concentration of H,O2 was 0.242 M, the concentration of H,O, dropped to 4.09×10 M after 23.5 seconds had passed. Based on these data, the rate constant for the reaction is M1s1.

The rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NH,NCO(aq)→(NH2)½CO(aq) is second order in NH,NCO. In one experiment, when the initial concentration of NH,NCco was 0.196 M, the concentration of NHẠNCO dropped to 4.00×102 M after 1.26×103 minutes had passed. Based on these data, the rate constant for the reaction is | M' min-1.

The compound 1,1-difluoroethane decomposes at elevated temperatures to give fluoroethylene and hydrogen fluoride according to the equation:  CH3CHF2(g) -> CH2CHF(g) + HF(g) At 460 K, the rate constant for this reaction is k = 5.8 ×× 10–6 s–1 and the activation energy is Ea = 265 kJ/mol. What is the frequency factor for this reaction?   At what temperature would the reaction proceed with a rate four times faster than at 460 K? ____K

In the presence of excess thiocyanate ion, SCN-, the following reaction is first order in iron(III) ion, Fe3+; the rate constant is (1.37x10^0)/s. Fe3+(aq) + SCN-(aq)  → Fe(SCN)2+(aq). What is the half-life, in seconds, of the reaction? Express your answer to three significant figures.

You determine through experimentation that the reaction A⟶P is first order with respect to A. If the rate constant of the reaction is determined to be 5.58 x 108 s−1, what is the half-life when [A]= 0.352 M at 25 ∘C. τ1/2 in seconds

Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) +03 (g) → NO3 (g) + O₂(g) 2 NO3 (g) + NO₂ (g) → N₂O5 (g) Suppose also k₁ « k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. rate = k rate constant k₁ k₂ ロ→ロ X Ś