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Lena772

  • one year ago

2A + B → C Select the rate law for the reaction above using the following information: Holding the concentration of A constant and doubling the concentration of B results in the rate of the reaction increasing from 1.5E-3 M/s to 6.0E-3 M/s. Keeping the concentration of B constant and doubling A results in the rate of the reaction increasing from 1.5E-3 M/s to 3.0E-3 M/s. A) rate = k [A] [B]2 B) rate = k [A]2 [B]2 C) rate = k [A]2 [B] D) rate = k [A]2 E) rate = k [B]2 F) rate = k [B]

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  1. Lena772
    • one year ago
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    @timo86m Is it C?

  2. anonymous
    • one year ago
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    lemme think its been a while :)

  3. Lena772
    • one year ago
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    Okay @timo86m

  4. anonymous
    • one year ago
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    Keep in mind that i haven not done this in so long rate=[A]^a [B]^b 2A+B->C 1st scenerio 1.5 to 6 is 4 with B doubled 2A+2B->6 2nd scenerio 1.5 to 3 is 2 with A doubled 4A+2B-> .5 NOW use that in [A]^a [B]^b We can see that B is ^2 and A is 1

  5. anonymous
    • one year ago
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    I say A. The problem is worded oddly.

  6. anonymous
    • one year ago
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    but get a second opinion. I am no student of chemistry. I am an autodidact.

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