Answer all please Which of the statements below accurately describe the rate of

Question

Answer all please Which of the statements below accurately describe the rate of the reaction BrO_3^- + 5Br^- + 6H^+ rightarrow 3Br_2 + 3 H_2O Rate = 3 Delta[H_2O]/Delta t The rate of disappearance of BrO_3^- is 6 times the rate of disappearance of H^+ The rate of disappearance of H^+ is 2 times the rate of appearance of Br_2 Rate = + Delta [Br]/5 Delta t Given the following balanced equation, determine the rate of reaction with respect to [NOCl]. If the rate of Cl_2 loss is 4.84 times 10^-2 M/s, what is the rate of formation of NOCl? 2NO(g) + Cl_2(g) rightarrow 2 NOCl(g) 4.84 times 10^-2 M/s 2.42 times 10^-2 M/s 1.45 times 10^-1 M/s 9.68 times 10^-2 M/s Nitric oxide gas (NO) reacts with hydrogen gas to form nitrous oxide and water. Use the following data to determine the rate law for the reaction. 2NO_(g) + H_2(g) rightarrow N_2O_(g) + H_2O_(l) Which of the following is the rate law (rate equation) for this reaction? rate = k[NO] rate = k[NO][H_2]^2 rate = k[NO][H_2] rate = k[NO]^2

Explanation / Answer

Q1.

BrO3- + 5Br- + 6H+ --> 3Br2 + 3H2O

a)

this is true, for the overall reaction

b)

this is inverted, since H+ must be 6 times that of BrO3-

c)

This is correct, since H+ must dissapear 2 times faster than Br2 due to 6:3 ratio

d)

False, since this is dissapearing, it must be negative

Q2

[Cl2] = 4.84*10^-2

for NOCl --> ratio is 2x

so it must be

2 times faster

2*(4.84*10^-2) = 0.0968

choose D

Q3

quickly --> changin [H2] in 1 and 2, will have NO effect in rate so [H2] is not an important value

then

for NO

rate 1 / rate 2 = (0.021)^a(0.065)^b / (0.042)^a(0.065)^b

(1.46) / (5.84) = (0.021)^a / (0.042)^a

0.25 = (1/2)^a

a = ln(0.25) / ln(0.5) = 2

then

rate = k[NO]^2

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