What is the value of the rate law constant for the reaction shown in the picture? a) -1.9 x10^4 b) +1.9 x 10^4 c) -5.2 x 10^-5 d) +5.2 x 10^-5 e) +6.2

For the following balanced equation, what is the rate of reaction with respect to [NH3]. N2 (g) + 3H2(g) →→ 2NH3 (g) A. ????=−2Δ[??3]Δ?Rate=−2Δ[NH3]Δt    B. ????=−Δ[??3]2Δ?Rate=−Δ[NH3]2Δt C. ????=+3Δ[?2]Δ?Rate=+3Δ[H2]Δt    D. ????=+Δ[??3]3Δ?Rate=+Δ[NH3]3Δt   E. there is not enough information to answer the question

A general reaction written as A + 2B → C + 2D is studied and yields the following data:   [A]0 [B]0 Initial Δ[C]/Δt   0.150 M 0.150 M 8.00 × 10–3 mol/L·s   0.150 M 0.300 M 1.60 × 10–2 mol/L·s   0.300 M 0.150 M 3.20 × 10–2 mol/L·s Determine the initial rate of C production (Δ[C]/Δt) if [A] = 0.200 M and [B] = 0.500 M.

2. Select the energy profile templates below (A or B) that correctly represents the enthalpy change calculated for the decomposition of ammonium nitrate and label it showing the reactants, products, change in enthalpy for the reaction, AHRXn and the activation energy, Ea. Potential Energy Reactants A Reaction Progress->> Products ΔΗ Potential Energy Reactants ΔΗ B Products Reaction Progress-> 3. Use your understanding of reaction kinetics and collision theory to explain why an increase in temperature causes an increase in reaction rate. 4. Evaluate the changes in physical state that occur during the decomposition of ammonium nitrate and predict the sign on AS for the reaction. 5. Use the standard entropies, S° to determine the AS (in J K-¹ mol¹ ) for the reaction. Does the sign on AS match your prediction?

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E= 64.0 kJ/mol. If the rate constant of this reaction is 3.3 x 10² M-¹-1 S at 243.0 °C, what will the rate constant be at 205.0 °C? Round your answer to 2 significant digits. 1 1 k = M 0 S x10 X 3

The rate law for the reaction 2NO(g) + 2H₂(g) → N₂(g) +2H₂O(g) is rate = k[NO]²[H₂] If the rate of reaction is 7.00 x 10-3 mol L¹s ¹ when the concentrations of NO and H₂ are both 1.8 x 106 mol L-1, what is the value of the rate constant and what are the units for the rate constant?, k= i 3.8 x 1015 L³ mol-3 s-1 L² mol-² 5-1 S-1 OL mol-¹ s-1 mol L-15-1 e Textbook and Media Hint Save for Later Attempts: 3 of 15 used Submit Answer

The following data were collected for this reaction: 2NO2(g) + 2F2(g) > 2NO2F(g) [NO2] [F2] [2NO2F] 0.100 0.100 0.026 0.200 0.100 0.051 0.200 0.200 0.103 0.400 0.400 0.411 A) Write the expression for the reaction rate law B) Find n value for [NO2] C) Find m value for [F2] D) Calculate the k value of k for this reaction

A certain reaction has the following general form: aA → bB At a particular temperature and [A], = 4.50 x 10-3 M, concentration versus time data were collected for this reaction, and a plot of 1/[A] versus time resulted in a straight line with a slope value of + 4.49 x 10-2 L/mol-s. a Determine the rate law for this reaction. (Use k for the rate constant.) Rate = Determine the integrated rate law for this reaction. 1 %3D [A] Determine the value of the rate constant for this reaction. Rate constant = L mol-1

[References] The reaction I (ag) + OCI (aq) → IO¯(aq) + Cl¯(aq) was studied, and the following data were obtained: I], (mol/L) [OCI"], (mol/L) Initial Rate (mol/L · s) 0.12 0.16 7.80 x 10-2 0.060 0.16 3.90 x 10-2 0.030 0.080 9.80 x 10-3 0.24 0.080 7.80 x 10- What is the rate law? (Use k for the rate constant.) Rate Calculate the value of the rate constant. k = L/mol · s Calculate the initial rate for an experiment where both I and OcI are initially present at 0.16 mol/L. Rate = mol/L · s

a. Reaction rate is expressed in terms of changes in concentration of reactants and products. Write a balanced equation for Rate = Δ[N2O4] /Δtime  = – Δ[O2] / Δtime  = – Δ[NO] / 2 Δtime b. A reaction has the experimental rate expression, rate = k[A]2/ [B]. When the concentration of A is tripled, then the rate (increases or decreases) by a factor of _________. A. increases            w. 2 B. decreases           x. 3                               y. 6                               z. 9