1. A + 3B → 2C If the rate that B is changing at the beginning of a reactions is 0.546 atm/min, how fast is A changing? Keep the units the same and remember rates are (+) by convention.
Part 2.
A + 3B → 2C
If the rate that B is changing at the beginning of a reactions is 0.521 atm/min, how fast is C changing?
Keep the units the same and remember rates are (+) by convention.
we have relation from eq
d[A] /dt = (1/3) d[B] /dt , given d[B] /dt = 0.546 atm / min
hence d[A]/dt = ( 1/3) ( 0.546) atm/min = 0.182 atm / min
2) (1/3) d[B] /dt = ( 1/2) d[C] /dt
d[C] /dt = ( 2/3) [d[B] /dt = ( 2/3) ( 0.521 atm/min) = 0.347 atm /min
For reaction 2A + 3B → 2C + D, following data of concentration and rate was obtained Trial Initial [A] Initial [B] Initial Rate (M/sec) 1 0.015 M 0.200 M 3.67 x 10^-6 20.030 M 0.200 M 7.33 x 10^-6 30.015 M 0.400 M 1.47 x 10^-5 The special rate constant k = A 1.2 x 10^-3 (1/M.sec) 9.2 x 10^-4 (1/M-sec) C 1.6 x 10^-3 (1/M-sec) 6.1 x 10^-3 (1/M^2-sec) E 8.2 x 10^-3 (1/M^2-sec)
5. Find the parametric form of the solutions of the system 2a +3b+c-1 a+b+c3 Ba+4b+2c
Need answers in clear writing.
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Part 1 please!
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part B please
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