in the folloeing reaction xA=yB log[-d[A]/dt]=log[d[B]/dt]+0.3 thus x:y ratio is:a)1:2b)2:1c)3:1d)3:10

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sam · Answer

it will be 2:1 as we know for a simple chemical reaction average rate of dissapearance= average rate of apperance A → B -dA/dT= dB/dT So for this reaction, (-dA/dT)/ x = (dB/dT)/y ….(i) We can write 0.3 as log 2 (Approx) then applying property of log... log a + log b= log ab we get log(-dA/dT)= log 2(dB/dT) taking antilog both sides and dividing by 2 and compare with (i) x=2, y=1 hence x:y =2:1

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in the folloeing reaction xA=yB log[-d[A]/dt]=log[d[B]/dt]+0.3 thus x:y ratio is:a)1:2b)2:1c)3:1d)3:10

in the folloeing reaction xA=yB log[-d[A]/dt]=log[d[B]/dt]+0.3 thus x:y ratio is:a)1:2b)2:1c)3:1d)3:10

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in the folloeing reaction xA=yB log[-d[A]/dt]=log[d[B]/dt]+0.3 thus x:y ratio is:a)1:2b)2:1c)3:1d)3:10

in the folloeing reaction xA=yB log[-d[A]/dt]=log[d[B]/dt]+0.3 thus x:y ratio is:a)1:2b)2:1c)3:1d)3:10

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