Given: 2A(g) + B(g) C(g) + D(g)
When [A] = [B] = 0.10 M,the rate is 2.0 M.s - 1; for [A] = [B] = 0.20,the rate is 8.0 M.s - 1; and for [A] = 0.10 M,[B] = 0.20 M,the rate is 2.0 M.s - 1.The rate law is
A) rate = k[A].
B) rate = k[B]2.
C) rate = k[A][B]0.
D) rate = k[A][B].
E) rate = k[A]2.
Correct Answer:
Verified
Q3: For a given first-order reaction, after 2.00
Q10: It is important to distinguish between the
Q11: The concentration-time dependence for two first order
Q12: For the reaction S2O82 - (aq)+
Q15: The concentration-time curves for two sets of
Q17: A first-order reaction has a rate constant
Q18: The concentration-time curves for two sets of
Q19: The rate of formation of oxygen
Q20: The concentration-time dependence is shown below for
Q35: Given: A
Unlock this Answer For Free Now!
View this answer and more for free by performing one of the following actions
Scan the QR code to install the App and get 2 free unlocks
Unlock quizzes for free by uploading documents