Chemistry, 23.09.2021 09:00 jasarochel
Bob Cat ran an experiment where he monitored the intensity of the color of a reactant with a spectrophotometer, and used Beer's Law to convert that intensity to a concentration in molarity. He monitored the experiment for 5 minutes. When the experiment was finished, he calculated the natural log of the concentration at each time, and the reciprocal of the concentration at each time. When he graphed all three forms of the data, the plot of the concentration versus time was a line with a slope of -0.045 M-1. What are the order and the rate constant for this reaction?
a. zero, 0.045 M/s.
b. zero, -0.045 M/s.
c. first. 0.045 M/s.
d. first. -0.045 M/s.
e. second0.045 M/s.
f. second -0.045 M/s.
Answers: 3
Chemistry, 22.06.2019 10:30, kluckey3426
Asample of air with a volume of 2.20m3 at a pressure of 105 kpa and a temperature of 30c is cooled to 10c and the pressure is reduced to 75.0 kpa. what is the new volume? 6.9 1.34 2.56 43.0 2.88
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What is the percentage of hydrogen in nitrogen trihydride
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Chemistry, 22.06.2019 13:30, makenziehook8
Which is true of a liquid? it has a definite volume but not a definite mass. it has a definite mass but not a definite volume. it has a definite volume but not a definite shape. it has a definite shape but not a definite volume.
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Chemistry, 22.06.2019 18:00, kingamir
Answer asap need it by wednesday morning carry out the following calculations on ph and ka of from data. i. calculate the ph of 0.02m hcl ii. calculate the ph of 0.036m naoh iii. calculate the ph of 0.36m ca(oh)2 iv. calculate the ph of 0.16m ch3cooh which has ka = 1.74 x 10-5 mol dm-3 v. calculate ka for weak acid ha which has a ph of 3.65 at 0.30m concentration vi. calculate the ka of a solution made by mixing 15.0 cm3 0.2m ha and 60.0 cm3 0.31m a-. [ph= 3.80] vii. calculate the ph of a solution made by mixing 15.0 cm3 0.1m naoh and 35.0 cm3 0.2m hcooh. [ka = 1.82 x 10-4 m]
Answers: 1
Bob Cat ran an experiment where he monitored the intensity of the color of a reactant with a spectro...
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