Use the following data to determine the individual and overall reaction orders. NO(g)+ CO2(g) rate kINO,1"[coj...
Work set 2 Using the experimental data given in the table, determine the reaction order on each reactant and compute the overall rate of the following chemical reaction: NO2CI(g)+3 CO (g) ->NO (g) + 3 CO2(g) Rate (mol/L-s) Exp. Run [NO2](M) [COJ(M) 0.10 0.0021 1 0.10 0.0082 0.20 0.10 3 0.0083 0.033 0.20 0.20 4 0.10 0.40
Exhibit 13-8 Consider the gas phase reaction and data below to answer the following question(s). NO2 (g)+ CO (R)NO (g)+CO2 (g) Initial Rate M/sec) 0.0050 0.080 NO2], M ICO, M Experiment 1 0.10 0.40 0.10 2 0.10 0.10 0.20 0.0050 4. Refer to Exhibit 13-8. What is the rate law for this reaction? a. Rate- k[NO2l[CO] b. Rate k[NO2][CO]2 c. Rate = k[NO2] [CO] d. Rate k[NO2]Ico2 e. Rate
Consider the reaction F2(g) + 2ClO2(g) →2FClO2(g) Use the data in the table to calculate the initial rate of the reaction when [F2] = 0.20 M and [ClO2] = 0.045 M. Experiment [F2] M [ClO2] M Initial rate (M/s) 1 0.10 0.010 1.2 x10−3 2 0.10 0.040 4.8 ×10−3 3 0.20 0.010 2.4 ×10−3 _____ M/s
question 6, please! 5. Consider the following gas phase reaction and data to answer the next five questions. NO2 (g)CO (g) NO (g) +CO2 (g) Experiment [NO2, M [CO], MInitial Rate (M/sec) 0.10 0.10 0.0050 0.40 0.10 0.080 2 3 0.100.200.0050 What is the rate law for this reaction? A) Rate KNO22 B) Rate KINO2lICO]2 C) Rate = 서NO2][CO] D) Rate KNO21Co12 E) Rate KNO212co] 6. What is the numerical value for the rate constant, k of the reaction above?...
Experimental rate data for the reaction 2H2(g) + Cl2(g) → 2HCl(g) are given in the chart below. Experiment [H2] [Cl2] Rate in M×s-1 1 0.0020 0.0075 3.8 x 10-3 2 0.0020 0.0025 1.3 x 10-3 3 0.0050 0.0025 1.3 x 10-3 4 0.0050 0.0010 0.5 x 10-3 a). What are the orders of the reaction for H2 and Cl2 individually? SHOW WORK. b).Then write the rate law for this overall reaction:
Using the following data, determine the rate law and calculate k: rate = k[F2]x[ClO2]y Experiment [F2] (M) [ClO2] (M) Initial rate (M/s) 1 0.40 0.05 1.2 M/s 2 0.20 0.10 0.60 M/s 3 0.40 0.10 2.4 M/s
Homework 8-3_1 Reaction Rate Orders, Temp Effects Reaction Rates and Rate Orders The following initial rate data was collected for the reaction: HI(g) + CHşl(g) à CH.(g) +1-(9) Experiment (HI) (CHI) Initial Rate 0.015 M0.900 M 4.01 x 10M's 0.030 M0.900 M 8.04 x 10'Ms 0.030 M0.450 M 3.99 x 10 m/s 1. What is the rate law for this reaction? a. Rate =k [HI] [CHI] b. Rate = k [HI] [C,H,I] c. Rate = k [HI] (C,H,I] d. Rate...
21. Calculate the equilibrium concentration of the reactants and products if K·5.0 x 08 and initial, ulate the equilibrium concentration of the reactants and products if K 5.0 x 10and ini the [A] = 2.0 M (7 pts) C(g) B(g) + A(g) ←→ pts) 22. Use the following kinetic data to determine the rate law for the reaction. (7 Initial Rate (mol/L s 3.3 Experiment Initial [NO2l(M) Initial [O21(M 0.40 0.10 1.7 0.20 0.10 1.7 0.20 0.20 23. Calculate the...
Consider the reactionX + Y→ ZFrom the following data, obtained at 360 K, (a)determine the order of the reaction, and (b)determine the initial rate of disappearance of X when the concentration of X is 0.30 M and that of Y is 0.40 M.Initial Rate of Disappearance of X (M/s)[X](M)[Y](M)0.0530.100.500.1270.200.301.020.400.600.2540.200.600.5090.400.30
3. For the reaction C3H3(g) + 5 O2(g) ----> 3 CO2(g) + 4H20(1) the following rate data were determined at 30°C. Experiment Initial C3H8 Initial O2 id. Rate 0.200M 0.200 M 3.00 x 101 0.400 M 0.200 M 6.00 x 101 0.200 MO 0.400 M 1 .20 x 102 a) Determine the reaction order with respect to C3H8. b) Determine the reaction order with respect to 02. c) Calculate the rate constant at this temperature. d) Write the rate law...