7) Compounds Q and R are known to react in the gas phase to form Compound X by the following overall balanced chemical equation: 2 Q(g) + R(g) → 2X(g) The reaction kinetics have been studied experimentally and the following elementary step sequence was proposed as the reaction mechanism: Step 1: Q+R-Z (slow step, large Ea) • Step 2: Q+Z+2X (fast step, small Ea) Based upon the proposed mechanism, what would be the best way to write the rate law expression for the reaction 2 Q(g) + R(g) → 2X(g)? A. rate = k[Q]²[R] B. rate = k[Q][R] C. rate = = k[R] D. rate = k[Q] [R][Z] E. rate = k[Q][R]²

Write the FULL reaction rate for the following chemical formula:   5H2C2O4(aq) + 2KMnO4(aq) + 3H2SO4(aq) → 10CO2(g) + 2MnSO4(aq) + K2SO4(aq) + 8H2O(l)

C2H6 (g)  2 CH3 (g)The gas-phase dissociation of ethane (C2H6) occurs with a rate constant of 5.5 x 10-4 sec-1 at 700. oC. The activation energy for the reaction is 384 kJ/mole. Calculate the rate constant at 900. oC.

Identify the molecularity of each elementary reaction in the table below. elementary reaction CH₂ CH₂ SiH, (g) C₂H₂(g) + SiH₂(g) 3 N₂O(g) + 0(g) → N₂ (g) + O₂(g) 2NO(g) + O₂(g) → 2NO₂ (g) molecularity unimolecular bimolecular Cannot be determined. unimolecular bimolecular Cannot be determined. unimolecular bimolecular Cannot be determined. termolecular quadrimolecular termolecular quadrimolecular termolecular quadrimolecular

Suppose the decomposition of dinitrogen monoxide proceeds by the following mechanism: elementary reaction N₂O(g) → N₂(g) + O(g) k₁ 2 N₂O(g) + O(g) → N₂(g) + O₂(g) k₂ Suppose also k₁>>k₂. That is, the first step is much faster than the second. step 1 rate constant.

Classify the following elementary reaction as unimolecular, bimolecular, or termolecular. Select the single best answer. unimolecular bimolecular O termolecular X + S

A compound with the formula, C3H6 undergoes an isomerization reaction in the gas phase to form a new compound with the same molecular formula. The isomerization reaction is first-order with a rate constant of 5.87 x 10-4 sec-1 at 485 degrees Celsius. If a 2.50 liter flask initially contains 722 torr of the starting gaseous compound at 485 degrees Celsius, how long will it take, in minutes, for the partial pressure of the starting compound to drop below 1.00 x 102 torr?

Consider the following two chemical equations that can occur in sequence: 2 Al (s) + 2 KOH (aq) + 6 H2O (l) → 2 KAl(OH)4 (aq) + 3 H2 (g) KAl(OH)4 (aq) + 2 H2SO4 (aq)  → KAl(SO4)2  + 4 H2O (s) a) Identify all intermediates in the reaction sequence. b) What is the net balanced equation for the sequence? c) If 23.0 g of aluminum metal reacts with all other reagents in excess, what mass of KAl(SO4)2 is produced?

Please provide proper explanation of the concept and solution

The kinetics of the reaction: I⁻ + OCl⁻ ⇄ OI⁻ + Cl⁻ was studied in basic aqueous media by Chia and Connick . The initial rate of I⁻ disappearance is given below for mixtures of various initial compositions, at 25°C (None of the solutions initially contained OI⁻ or Cl⁻ ). If the mechanism of the reaction is given below, which constants below play role in the reaction rate law: OCl⁻ + H₂O ⇄ HOCl + OH⁻ (rate constant=k₁, equil.const=K₁)---fast, equilibrium I⁻ + HOCl → HOI + Cl⁻ (rateconstant=k₂)---slow HOI + OH⁻ ⇄ H₂O + OI⁻ (rate constant=k₃, equil.const=K₂)---fast, equilibrium