The chemical equation corresponding to the hydrolysis reaction can be written: R-CI + H20 →R-OH + CI + H* Let's call a the initial concentration in 2-chloro-2-methyl-butane and x the concentration of hydrochloric acid that is formed at time t. Water remains in large excess all over the course of the reaction. Then one can write: R-CI+ H,0 -→R-OH + CI + H* t = 0 0 0 0 a t >0 t = 00 01: Complete the table above with the molar quantities of each compound at times t> 0 and t = 0 with the data of the text.

= ◇ KINETICS AND EQUILIBRIUM Expressing the concentration of an intermediate in terms of the... Consider the following elementary reaction: 2 NO₂(g) → NO₂(g) + NO(g) Suppose we let k₁ stand for the rate constant of this reaction, and k_₁ stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of NO₂ in terms of k₁, k₁, and the equilibrium concentrations of NO and NO. [NO₂] = 0 X 2 8 1/5

Methyl salicylate has the odor of oil of wintergreen. This ester is prepared by the Fisher esterification of salicylic acid with methanol, shown here: HSO, OH * CH,OH OCH, • H,0 +] OH OH Use the dropdowns below to indicate the order of the steps that occur in this reaction mechanism to transform salicylic acid into methyl salicylate. Step 1 [ Choose (Choose Step 2 Protonation of the C-O oxygen atom Step 3 Proton transfer to neutralize the product Reforming of the CHOand loss of the leaving group Step 4 Proton transferts the OH group on the tetrahedral intermediate Attack of the methanol on the carbon of the C-O Step 6 Breaking of the pi bond to push eléctrons onto exygeri nd form the tetrahedial intermedian

Consider a reaction taking place at two different temperatures, T₁= 50 K and T₂- 150 K. What is the mathematical expression showing at which temperature the reaction will be faster?

Initial-rate data at a certain temperature is given in the table for the reaction SO₂Cl₂(g) SO₂(g) + Cl₂(g) [SO₂Cl₂], (M) k= 0.100 0.200 0.300 Initial rate (M/s) 2.00 x 10-6 4.00 x 10-6 6.00 x 10-6 Determine the value and units of the rate constant. units:

Consider a reaction A → B with activation energy 50.7 kJ/mol.   At 19.5 °C, the rate constant, k, for this reaction is 0.095 s−1. Calculate the temperature, T (in °C), at which k = 0.329 s−1. Assume the pre-exponential factor (A) is constant with temperature.   �=0.08206 L⋅atmmol⋅K=8.314 Jmol⋅K   �K=�∘C+273.15   1 kJ = 1000 J   Report your answer to three significant figures without the unit. Example: 20.0. Be sure that your answer is in °C and not Kelvin!