Answer:
a) Check explanation for this
b)Rate law is ![Rate = \frac{k_{1}k_{4} }{k_{3}+ 2k_{4} } [H_{2} ]](https://tex.z-dn.net/?f=Rate%20%3D%20%5Cfrac%7Bk_%7B1%7Dk_%7B4%7D%20%20%7D%7Bk_%7B3%7D%2B%202k_%7B4%7D%20%20%7D%20%5BH_%7B2%7D%20%5D)
c) The rate does not depend on the concentration of CO₂
Explanation:
a) Elementary steps for the RWGS reaction:
- Dissociative adsorption of the H₂ Molecule
(Fast process)
- Reversible Reaction between CO₂ and H
(Fast Process)
- Slow dissociation of COOH into gaseous CO and absorbed OH
(Slow process)
- Fast hydrogenation of the OH to form H₂O
(Fast process)
b) Derivation of the rate law
We need to determine the rate law for H, OH and COOH because these are the intermediates for this reaction.
The steady state approximation is applied to a consecutive reaction with a slow first step and a fast second step (k1≪k2). If the first step is very slow in comparison to the second step, there is no accumulation of intermediate product.
Rate of consumption = Rate of production
For COOH:
Using steady state approximation
![\frac{d[COOH]}{dt} = 0](https://tex.z-dn.net/?f=%5Cfrac%7Bd%5BCOOH%5D%7D%7Bdt%7D%20%3D%200)
![k_{2} [CO_{2} ][H] = k_{3} [COOH] k_{4} [COOH]\\](https://tex.z-dn.net/?f=k_%7B2%7D%20%5BCO_%7B2%7D%20%5D%5BH%5D%20%3D%20k_%7B3%7D%20%5BCOOH%5D%20k_%7B4%7D%20%5BCOOH%5D%5C%5C)
![[COOH] = \frac{k_{2} [CO_{2} ][H]}{k_{3}k_{4} } \\](https://tex.z-dn.net/?f=%5BCOOH%5D%20%3D%20%5Cfrac%7Bk_%7B2%7D%20%5BCO_%7B2%7D%20%5D%5BH%5D%7D%7Bk_%7B3%7Dk_%7B4%7D%20%20%7D%20%5C%5C)
For H:
![\frac{d[H]}{dt} = 0](https://tex.z-dn.net/?f=%5Cfrac%7Bd%5BH%5D%7D%7Bdt%7D%20%3D%200)
![k_{1}[H_{2}] = k_{2}[CO_{2} [H]+k_{5} [ OH][H]](https://tex.z-dn.net/?f=k_%7B1%7D%5BH_%7B2%7D%5D%20%3D%20k_%7B2%7D%5BCO_%7B2%7D%20%5BH%5D%2Bk_%7B5%7D%20%5B%20OH%5D%5BH%5D)
![[H]= \frac{k_{1}[H_{2}] }{k_{5}[OH] +k_{2}[CO_{2}]}\\](https://tex.z-dn.net/?f=%5BH%5D%3D%20%5Cfrac%7Bk_%7B1%7D%5BH_%7B2%7D%5D%20%20%7D%7Bk_%7B5%7D%5BOH%5D%20%2Bk_%7B2%7D%5BCO_%7B2%7D%5D%7D%5C%5C)
For OH:
![\frac{d[OH]}{dt} = 0](https://tex.z-dn.net/?f=%5Cfrac%7Bd%5BOH%5D%7D%7Bdt%7D%20%3D%200)
![k_{4} [COOH] = k_{5} [OH][H]\\\k[OH] = \frac{k_{4} [COOH]}{k_{5} H}\\](https://tex.z-dn.net/?f=k_%7B4%7D%20%5BCOOH%5D%20%3D%20k_%7B5%7D%20%5BOH%5D%5BH%5D%5C%5C%5Ck%5BOH%5D%20%3D%20%5Cfrac%7Bk_%7B4%7D%20%5BCOOH%5D%7D%7Bk_%7B5%7D%20H%7D%5C%5C)
The rate of the overall reaction is determined by the slowest step of the reaction. The slowest process is the dissociation of COOH
Therefore the overall rate of reaction is:
![Rate = k_{4} [COOH]\\](https://tex.z-dn.net/?f=Rate%20%3D%20k_%7B4%7D%20%5BCOOH%5D%5C%5C)
![Rate = k_{4} \frac{k_{2} [CO_{2} ][H]}{k_{3}k_{4} }\\Rate = k_{4} \frac{k_{2}[CO_{2}]\frac{k_{1}[H_{2}] }{k_{5}[OH] +k_{2}[CO_{2}]} }{k_{3}k_{4}}\\Rate = k_{4} \frac{k_{2}[CO_{2}]\frac{k_{1}[H_{2}] }{k_{5}\frac{k_{4}COOH }{k_{5}H } +k_{2}[CO_{2}]} }{k_{3}k_{4}}](https://tex.z-dn.net/?f=Rate%20%3D%20k_%7B4%7D%20%20%5Cfrac%7Bk_%7B2%7D%20%5BCO_%7B2%7D%20%5D%5BH%5D%7D%7Bk_%7B3%7Dk_%7B4%7D%20%20%7D%5C%5CRate%20%3D%20k_%7B4%7D%20%20%5Cfrac%7Bk_%7B2%7D%5BCO_%7B2%7D%5D%5Cfrac%7Bk_%7B1%7D%5BH_%7B2%7D%5D%20%20%7D%7Bk_%7B5%7D%5BOH%5D%20%2Bk_%7B2%7D%5BCO_%7B2%7D%5D%7D%20%20%7D%7Bk_%7B3%7Dk_%7B4%7D%7D%5C%5CRate%20%3D%20k_%7B4%7D%20%20%5Cfrac%7Bk_%7B2%7D%5BCO_%7B2%7D%5D%5Cfrac%7Bk_%7B1%7D%5BH_%7B2%7D%5D%20%20%7D%7Bk_%7B5%7D%5Cfrac%7Bk_%7B4%7DCOOH%20%7D%7Bk_%7B5%7DH%20%7D%20%20%2Bk_%7B2%7D%5BCO_%7B2%7D%5D%7D%20%20%7D%7Bk_%7B3%7Dk_%7B4%7D%7D)
Simplifying the equation above, the rate law becomes
![Rate = \frac{k_{1}k_{4} }{k_{3}+ 2k_{4} } [H_{2} ]](https://tex.z-dn.net/?f=Rate%20%3D%20%5Cfrac%7Bk_%7B1%7Dk_%7B4%7D%20%20%7D%7Bk_%7B3%7D%2B%202k_%7B4%7D%20%20%7D%20%5BH_%7B2%7D%20%5D)
c) It is obvious from the rate law written above that the rate of the RWBG reaction does not depend on the concentration of CO₂
Answer:
Overconfidence in more male drivers, particularly those under 25 years old, results in them being involved in crashes.
ANSWER: True
Answer:
hdwhifniuewohfoyyhyeiudhwbwuxvgusvfgcvxg
Explanation:
Answer:
kk
Explanation:
dkdndidodd ndidkjeeiwonejeeidmdnddkdidfmndd
Answer:
S = 0.5 km
velocity of motorist = 42.857 km/h
Explanation:
given data
speed = 70 km/h
accelerates uniformly = 90 km/h
time = 8 s
overtakes motorist = 42 s
solution
we know initial velocity u1 of police = 0
final velocity u2 = 90 km/h = 25 mps
we apply here equation of motion
u2 = u1 + at
so acceleration a will be
a =
a = 3.125 m/s²
so
distance will be
S1 = 0.5 × a × t²
S1 = 100 m = 0.1 km
and
S2 = u2 × t
S2 = 25 × 16
S2 = 400 m = 0.4 km
so total distance travel by police
S = S1 + S2
S = 0.1 + 0.4
S = 0.5 km
and
when motorist travel with uniform velocity
than total time = 42 s
so velocity of motorist will be
velocity of motorist = 
velocity of motorist =
velocity of motorist = 42.857 km/h