A novice chemist conducted an experiment to study the decomposition of a reactant A. The concentration of A was measured at different time intervals. a) appr Assuming the decomposition of reactant A follows a second-order reaction, elucidate for the novice chemist the methodology for calculating both the half-life of the reaction and the reaction rate. Include any relevant equations and a brief explanation of each term. C Upon measuring the half-lives for the first, second, and third reactions, the novice chemist observed that each successive half-life was longer than the previous one. Offer a comprehensive explanation for this observation.

Give two reasons (short statements) why the rate of a catalyzed reaction mightdecrease as the pressure of one of its products increases.

can you please help with anything?  1) Calculate the mole flow rates of all components in stream. 2) Calculate the single pass conversion 3) overall conversion

Determine the Michaelis constant and the maximum velocity of the reaction. Using direct linear plot

Please answer ALL parts of the question and show your work. Consider this reaction: N2(g) + 3H2(g)  <------>  2NH2(g)          H= -123kJ Describe how the concentration of H2 will be affected by each of the following changes to the system at equilibrium. Will it increase, decrease, or not change? (a) The volume of the reaction chamber is decreased (b) Helium gas is added to the reaction chamber (c) The temperature is increased (d) N2 has is added to the reaction chamber

You are carrying out a reaction in the laboratory. You need to convert 1.00 mole of reactant X into products. This reaction shows first-order kinetics, and the reaction mixture has a constant volume of 1.00 L. At 1:00pm, you start the reaction at 25\deg C with 1.00 mole of reactant X. At 2:00pm, you find that 0.70 moles of reactant X remain. You immediately increase the temperature of the reaction mixture to 35\deg C. At 3:00pm, you discover that 0.25 moles of reactant X are still present. You want to be able to finish the reaction by 4:00pm, but you cannot stop the reaction until only 0.01 moles of reactant X remain. You must increase the temperature again. What is the minimum temperature required to complete the reaction by 4:00pm? (Remember, the reaction is complete when only 0.01 moles of X remain.)

The kinetics of the hydrolysis of methyl methanoate, CH;COOCH;, in aqueous solution were investigated by measuring the concentration of the ester after different time intervals. The reaction was found to be first order in the concentration of the ester. Use the data below to determine the rate constant for the reaction. time (t/s) concentration (c/mol.dm-3) 1800 3600 5400 7200 9000 0.300 0.191 0.135 0.081 0.055 0.035

Explosions occur when the rate of reaction increases dramatically over a short period of time. There are several types of explosions such as autocatalytic explosions, thermal explosions and branched chain explosions. The mole balance of radical species in branched chain reaction can be expressed as: (Refer attachment) With appropriate assumption, prove that the branched chain explosion can occur exponentially and provide two (2) ways to prevent the occurrence of radical chain explosion in chemical laboratory.

Problem IX (10 p): Consider the isomerization of compound A from its cis to its trans isomer at 298 K, which is first order in both directions: ki cis-A = trans-A k2 The rate constant for the forward reaction is k1 = 4.2 × 10* s', and the rate constant for the reverse reaction is k2 = 2.1 × 10-ª s-1. %3D a) Calculate the equilibrium concentrations [cis-A]eq and [trans-A]eq, assuming that at time t= 0 all of A was in the cis-form, i.e., [cis-A]o = [A]o. (Hint: Use the fact that at any time, [cis-A] + [trans-A] = [A]o.) %3D b) Which reaction is spontaneous, the forward reaction or the reverse reaction? Provide your reasoning. Total /100 p

The rate of a certain reaction is given by the following rate law:   rate =kNO2O2 Use this information to answer the questions below.   What is the reaction order in NO?   What is the reaction order in O2?   What is overall reaction order?   At a certain concentration of NO and O2, the initial rate of reaction is 5.0 x 104 M / s. What would the initial rate of the reaction be if the concentration of NO were doubled? Be sure your answer has the correct number of significant digits. Ms The rate of the reaction is measured to be 40.0 M / s when [NO] = 0.57 M and [O2] = 2.0 M. Calculate the value of the rate constant. Be sure your answer has the correct number of significant digits. =k⋅M−2s−1