What is the rate constant of a first-order reaction that takes 490 seconds for the reactant concentration to drop to half of its initial value? Express your answer with the appropriate units. • View Available Hint(s) Templates Symbols undo redo Peset keyboard shortcuts help Value Units

Consider the coagulation of a protein at 100°C. The first-order reaction has an activation energy of 69 kJ/mol. If the protein takes 5.4 minutes to coagulate in boiling water at 100°C, then how long will it take to coagulate the protein at an altitude where water boils at 83°C? Time = _________________  min

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The reaction A-B is first order with a half life of 0.903 seconds. What is the rate constant of this reaction ins 1? Do not report units in your answer. Report your answer with 3 places past the decimal point. Type your answer..

Determine the activation energy. E, for the reaction. Express your answer in kilojoules per mole to four significant figures. Templates Symtols undo redo feset keyboard shortcuts Help En = kJ- mol

Q5 - Half-life Homework • Unanswered lodine atoms combine to form molecular iodine in the gas phase. This second order reaction has a rate constant of 7.0 x 109 1/(M*s). Calculate the time required for the iodine concentration to decrease from 0.60 M (t=0) to 0.30 M. Note: this specific time is known as the half-life of the reaction. |(g) + I(g) → I2(g) -> |2{8) Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a 2.4 x 10-10 s b 9.9 x 10-11 s 4.3 x 10-11 s

A first-order reaction has a rate constant of 0.33 min-1. It takes ________ min for the reactant concentration to decrease from 0.45 M to 0.09 M.

The reaction A→ Products is a first-order reaction with a rate constant of 1.91 x 10-3 min-1. The reaction started with an initial concentration of A equal to 0.0881 M, what is the concentration of A after 131.1 minutes? Do not write unit in answer. Report your answer with four places past the decimal point. Type your answer... Submit