What is the overall reaction order for the following rate law: rate = k [a]2[b]? a. zero b. first c. second d. third

The correct answer is Option D.

Explanation:

Rate law states that the rate of a reaction is directly proportional to the concentration of the reactants each raised to the power their stoichiometric coefficient which is determined experimentally and is known as order.

k = rate constant

x = order with respect to A

y = order with respect to B

n = x+y = Total order

For the given rate:  

The order with respect to A is 2 and the order with respect to B is 1.

So, the total order of the reaction will be = (2 + 1) = 3

Hence, the correct answer is Option D.

given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g

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