GmailYouTubeMapsTranslateGE NewsS Solutions to Algeb...Course ConnectThe half life of some made-up, 1st order reaction is 10 days. If you start with 1.00 g ofthe imaginary reactant, how much is left after 30 days?Select one:O a. 1.00 gO b. 0.125 gO c. 0.50 gO d. 0.25 g14C dating works because the amount of 14C produced from nitrogen reacting withcosmic radiation and has a steady-state concentration. We know how much 14Cshould be in a living organism at the time of its death (when it stops incorporatingfint order decay of 14C is 5720 years, we carbon

Answered: Image /qna-images/answer/ee17b130-5f13-4b80-b8f2-a1669dd16b01.jpg

The half life of some made-up, 1st order reaction is 10 days. If you start with 1.00 g of the imaginary reactant, how much is left after 30 days? Select one: O a. 1.00 g O b. 0.125 g O c. 0.50 g O d. 0.25 g Awith

The half life of some made-up, 1st order reaction is 10 days. If you start with 1.00 g of the imaginary reactant, how much is left after 30 days? Select one: O a. 1.00 g O b. 0.125 g O c. 0.50 g O d. 0.25 g Awith

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

At a particular temperature, N 20 5 decomposes according to a first-order rate law with a half-life of 3.0 s. If the initial concentration ofN 20 5 is 1.0 х 10 16 molecules/cm what will be the concentration in molecules/cm 3 after 11.5 s? O a. 1.0 × 1016 O b.2.3 × 10-1 O. 7.0× 1014 O d. 3.4 x 101 O e. 2,0 × 1014
The decomposition of gaseous dinitrogen pentaoxide (N2O5) to NO2 and O2 is a first-order reaction. At 60°C the half-life of the reaction is 2.48 x 102 s. If the initial concentration of N2O5 is 1.58 mol/L, then: a. What is [N2O5] after 3 minutes? b. What fraction of N2O5 has decomposed after 3 minutes?
8) A first order reaction starts with a concentration of reactant equal to 0.040 M. After two hours, the molarity is 0.020M. What is the molarity after four hours? a. 0.015M c. 0.005M e.0.03 М b. 0.010 M d.0.0025 M
The half-life of a first order reaction is constant and equal to 0.693/k. CA first order reaction with k= 3.465 x 10-2 s-1 is started with [A]o=0.800 M. What is the concentration of A after 60 seconds? Oa. 0.100 M Ob. 0.400 M Oc. c. 0.200 M Od. 0.0800 M
If the half-life of a first order reaction is 3.00 minutes, the rate constant is...? (One of the options below is correct) a. 1.50 min-1 b. 1.05 min-1 c. 4.34 min-1 d. 0.405 min-1 e. 0.231 min-1
17. A first order decomposition reaction was found to have an initial rate of 0.19 M-min- when the initial reactant concentration was 0.33 M. What is the initial rate of reaction if the initial concentration is increased to 0.45 M? D. 0.19 M·min E. 0.58 M·min- A. 0.26 M·min- B. 1.3 M-min¬1 C. 0.78 M·min-
7. DETAILS The first-order rate constant for the conversion of cyclobutane to ethylene at 1000.°C is 101 s ¹. C4H8 → 2 C₂H4 A. What is the half-life of the reaction at 1000."C? [ B. If you started with 3.350 g of cyclobutane, how long would it take to consume 0.4020 g of it? C. How much of a 2.50 g sample of cyclobutane would remain after 0.03430 s? Useful Information: 1.013 bar = 760 torr = 1 atm = 760 mm Hg h = 6.62607x10-34 3.s c = 2.99792 x 108 m/s R = 8.314472 3/mol.K NA = 6.02214 x 1023 1/mol R = 0.08205746 L.atm/mol.K F = 9.648534 x 104 c/mol Equations: K= K (RT)An AG=AHⓇ - TASⓇ MY NOTES pH = pk +log. E = E [A] [HA] 7=45 0.05916 n ASK YOUR TEACHER PRACTICE ANOTHER log Qrxn AG=-RTINK AG=-nFE 1 [A]t In(2) k [A] = [A]okt 1 =kt + [A] 9 [A] t= k[A] [A] 2k -kt -Ea k Ae RT
2. A certain second order reaction has a half-life of 58.0 s. Determine the time (in seconds) needed for the reaction to be 88.0 % complete if the starting concentration is 14.20 M. (Hint: you're given the half-life, what can you determine? Once you have that, are you able to solve for the time?)
The decomposition of NO2 is a second order reaction and the rate constant is 0.755 L/mol-s. In an experiment, the initial concentration of NO2 was 0.00650 mol/L. What is the half-life? Select one: a. 103.45 sec b. 304.56 sec c. 303.76 d. 203.76
27 The reaction: 2NO + Cl2 → 2NOCl is second order in NO, first order in Cl2 and third order. Compare the initial rate of reaction a mixture of 0.02 mol of NO and 0.02 mol of Cl2 in one liter container with the rate of reaction when two third of NO was consumed? Select one: a. 2/27 b. 3/27 c. 5/27 d. 4/27
43-46 Consider the time and concentration data for: 2 NO2(g) 2 NO(g) + O2(g). Time, s [NO2] 43 a. How long is the first half-life? Write the value and units 0.100 0.072 20 b. How long is the second half-life? Write the value and units 0.050 50 44. Write the rate law for this reaction. Explain why you made this choice. 0.036 90 0.025 150 45. What is the value of the rate constant? Write the general equation, the calculation equation with units, and the answer with units 46. How much time is needed until only 0.010 M NO2 remains? Write the general equation, the calculation with units, and the answer with units c
The first-order decomposition of cyclopropane has a rate constant of 6.7 x 10-4 s-1. If the initial concentration of cyclopropane is 1.33 M, what is the concentration of cyclopropane after 644 s? A) 0.43 M B) 0.86 M C) 0.94 M D) 0.15 M E) 0.67 M