These images represent the first order reaction A rightarrow B initially and at

Question

These images represent the first order reaction A rightarrow B initially and at some later time. The rate law for the reaction is Rate = 0.010 s^-1 [A]. How much time has passed between the two images? 69 s 139 s 60 s 12.5 s Pick the single-step reaction that according to collision theory, has the smallest orientation factor H + H rightarrow H_2 I + HI rightarrow I_2 + H H_2 + H_2C = CH_2 rightarrow H_3 C - CH_3 All of these reactions have the same orientation factor Carbon monoxide and chloride gas react to form phosgene (COCl_2) according to the equation: CO(g) + Cl_2 rightarrow COCl_2(g) The rate law for reaction is rate = K[Cl_2]^3/2 [CO]. Which mixture of chlorine gas and carbon monoxide gas has the fastest initial rate?

Explanation / Answer

13 - t1/2= 0.693/k --- the no of reactansts consumed, before reactions, 16 and after reactions 4.... that means two t1/2 is the reaction time. t1/2= 0.693/k ---- t1/2= 69 so 2 t1/2= 139 sec

14 - in the case of c) the shape of the reactants are different so they need more collisions than the other set of reactions

15 - rate is depend on both the reactant. rate = k(Cl2)1.5(CO)

from the rate equiation, we can find out that for ideal reaction, the concentration of Cl2 should be more than CO and its actually 1.5 Cl2 + CO ------> COCl2

from the bellow options a) and d) have the same no of CO and Cl2 (the ratio is 1:1); in the case of c) the amount of CO is more than Cl2 (the ratio is 1.5:1)

but in the case of b) total amount of CO are 3 and Cl2 are 5. the ratio is almost 1 : 1.5

so the answer is b

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