[A], M t, s 2.000 1.429 2 1.111 4 5 1.000 0.833 7 0.667 10 0.500 0.333 15 25 0.286 0.250 0.125 30 35 75

Carbon dating is often used to estimate the age of once living organisms (which contain carbon). The first order reaction involves the change of 14C to 12C (two isotopes of carbon). An object is analysed and found that only 87.9% of the expected 14C is still present. Assume that the half-life of 14C is 5700 years. a) Calculate the rate constant for the reaction of 14C to 12C. b) What is the age of the object? c) What % 14C would be left after 8550 years?

The rate at which a certain drug is eliminated by the body follows first-order kinetics, with a half life of 69 minutes. Suppose in a particular patient the concentration of this drug in the bloodstream immediately after injection is 1.9 µg/mL. What will the concentration be 276 minutes later? Round your answer to 2 significant digits.

Calculate the half life, in minutes, for a second order reaction with an initial concentration of 0.45 M and a rate constant, k, of 0.017 M/s.

Can someone please help with question 3

A reactant decomposes with a half-life of 179 s when its initial concentration is 0.247 M. When the initial concentration is 0.775 M, this same reactant decomposes with the same half-life of 179 s. What is the order of the reaction? 1 2 What is the value and unit of the rate constant for this reaction? k =

39. The decomposition of a certain pesticide was found to follow first-order kinetics. A student finds that after 3.0 months a sample of pesticide was 87.5% decomposed (only 12.5% of the pesticide remained). What is the half-life (112) for the decomposition reaction? a. 1.0 months b. 2.0 months 3.0 months d. The half-life can not be determined with the information provided.

The reaction rate coefficient for a pollutant following first order reaction is 0.3 per day. If the initial concentration of the pollutant is 250 mg/L, Calculate the time taken to reduce the concentration to 30 mg/L. Also determine the half life of the reaction.

Give the characteristic of a first order reaction having only one reactant. The rate of the reaction is not proportional to the concentration of the reactant. The rate of the reaction is proportional to the square of the concentration of the reactant. The rate of the reaction is proportional to the square root of the concentration of the reactant. The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. The rate of the reaction is directly proportional to the concentration of the reactant.

It is found that a gas undergoes a zero order decomposition reaction in the presence of a Ni catalyst.  If the rate constant for the reaction is 8.10x10-2M/s and the initial concentration of the gas is 0.100M How long in minutes, will it take for the concentration to decrease to 0.0010M? What would the concentration of the gas be after 65.0 minutes has elapsed? What is the half life for this reaction? What effect would double the concentration of the gas have on the rate of the reaction?