Reaction A + B + C  D has the following differential rate law: rate = k[A][B]2.a) If the concentration of A is tripled, what happens to the rate- increase or decrease and by what factor?b) If the concentration of A is doubled and the concentration of C is halved, what happens to the rate – increase or decrease and by what factor?

step-by-step explanation:

the simplified form is

step-by-step explanation:

we want to simplify the expression,

let us change the middle bar to a normal division sign to obtain,

we multiply the first fraction by the reciprocal of the second fraction to obtain,

we factor to obtain,

we cancel the common factors to get,

we simplify to get,

the correct answer is b

60: 45 =12: 9 =4: 3 so the answer is 4: 3