After gathering rate data, a chemist graphed the data to obtain a linear representation of the data. The graph shown below best depicts a time (s) A) zero order reaction with respect to reactant A B) first order reaction with respect to reactant A C) second order reaction with respect to reactant A D) third order reaction with respect to reactant A (W) []

a) The reaction A(ag) → B(aq) is first-order with respect to A(aq). The concentration of A(aq) after 100.0 s of reaction is 0.555 M. The concentration of A(aq) after a further 400.0 s (500.0 s total) is 0.333 M. What will be the concentration of A(aq) after a further 500.0 s (1000.0 s total)? What is the half-life of the reaction? The temperature is 25.0 °C throughout the reaction. b) The reaction 2 A(aq) → B(aq) is second-order with respect to A(aq). When the concentration of A(ag) is 0.150 M and the temperature is 25.0 °C, the reaction rate is 0.1350 M/s. If we increase the concentration of A(aq) to 0.450 M and lower the temperature to 5.0 °C, the rate of reaction becomes 0.0300 M/s. What is the activation energy for this reaction?

What is the concentration of a reactant after 30 minutes, given the initial concentration is 0.10M. The reaction is a first order reaction with a half-life of 75 minutes. Group of answer choices 0.076 M 0.085 M 0.12 M 0.1 M

Can you explain the concept? How to apply the concept to this problem and other problems? And what if they ask for the answer in different time like in seconds or hours

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..

A particular reaction is found to be zero order. The reactant has an initial concentration of 1.52 M and a rate constant of 0.00740 M/s. Calculate the half life of this reactant in seconds. t1/2 =[A]i/2k

Using an integrated rate law for a first-order reaction At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.141 s¯¹: H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.290M. Calculate the concentration of H₂CO3 in the vessel 4.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś

A reaction that is second-order in reactant A has [A]o = 0.200 M. The half-life is 45.6 sec. What is [A] after 3.00 min? Report the molarity in standard notation with 3 significant figures and do not include units (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