Problem: The reaction below has an initial rate of 0.070 M/s. What will the initial rate be if [A] is halved and [B] is tripled?  A  +  B  →  C  +  D         Rate = k [A][B]  2 a) 0.105 M/s b) 0.000343 M/s c) 0.315 M/s d) 0.210 M/s e) 0.0098 M/s

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The reaction below has an initial rate of 0.070 M/s. What will the initial rate be if [A] is halved and [B] is tripled? 

A  +  B  →  C  +  D         Rate = k [A][B]  2

a) 0.105 M/s

b) 0.000343 M/s

c) 0.315 M/s

d) 0.210 M/s

e) 0.0098 M/s

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