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Tutorial 3 solutions

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- Write the rate laws for the following reactions assuming each reaction follows an elementary rate laws.
- C2H6 → C2H4 + H2
- (CH3)3COOC(CH3)3 ⇌ C2H6 + 2CH3COCH3

- Write the rate law for the reaction:
2A + B → C

if the reaction

- is second order in B and overall third order,
- is zero order in A and first order in B
- is zero order in both A and B
- is first order in A and overall zero order

- The formation of ortho-nitroanilineis formed from the reaction of ortho-nitrochlorobenzene(ONCB) and aqueous ammonia.
The liquid-phase reaction is first order in both ONCB and ammonia with k= 0.0017 m3/kmol-min at 188°C with E = 11,273 cal/mol. The initial entering concentration of ONCB and ammonia are 1.8 kmol/m3 and 6.6 kmol/m3 respectively.

- Write the rate law for the rate of disappearance of ONCB in terms of concentration.
- Set up stoichiometric table for this reaction for a flow system.
- Explain how part (a) and (b) would be different for a batch system.
- Write –rAsolely as a function of conversion.
- What is the initial rate of reaction (X=0) at 188°C and at 25°C?
- What is the rate of reaction when X = 0.9 at 188°C and at 25°C?
- What would be the corresponding CSTR volume at 25°C to achieve 90% conversion at 188°C for a feed rate of 2 dm3/min

- Write the rate laws for the following reactions assuming each reaction follows an elementary rate laws.
- C2H6 → C2H4 + H2
- (CH3)3COOC(CH3)3 ⇌ C2H6 + 2CH3COCH3

(a)

(b)

- C2H6 → C2H4 + H2
- A → B + C

- (CH3)3COOC(CH3)3 ⇌ C2H6 + 2CH3COCH3
- A ⇌ B + 2C

- Write the rate law for the reaction:
2A + B → C

if the reaction

- is second order in B and overall third order
- is zero order in A and first order in B
- is zero order in both A and B
- is first order in A and overall zero order

(a)

(b)

(c)

(d)

The formation of ortho-nitroanilineis formed from the reaction of ortho-nitrochlorobenzene(ONCB) and aqueous ammonia.

The liquid-phase reaction is first order in both ONCB and ammonia with k= 0.0017 m3/kmol-min at 188°C with E = 11,273 cal/mol. The initial entering concentration of ONCB and ammonia are 1.8 kmol/m3 and 6.6 kmol/m3 respectively.

- Write the rate law for the rate of disappearance of ONCB in terms of concentration.
Let A = ONCB, B = NH3, C = Nitroaniline , D = NH4Cl

A + 2B → C + D

- Set up stoichiometric table for this reaction for a flow system

- Explain how part (a) and (b) would be different for a batch system
For batch system,

- Write –rAsolely as a function of conversion.
For liquid phase rxn, υ= υ0

Substituting the concentration of A & B;

---(1)

- What is the initial rate of reaction (X=0) at 188°C and at 25°C
i) At T= 188°C, k =0.017m3/kmol-min

Substituting X=0 and k =0.017m3/kmol-min into (1);

---(1)

- What is the initial rate of reaction (X=0) at 188°C and at 25°C
ii) At T= 25°C (298.15 K), k =? m3/kmol-min

Find k at T =25°C first

k at initial T is

k at any temperature is

Taking the ratio;

---(1)

- What is the initial rate of reaction (X=0) at 188°C and at 25°C
ii) Now we know that, at T= 25°C (298.15 K), k = 2.039 x 10-6 m3/kmol-min

Therefore, we can calculate –rA at 25° by susbtituting

k= 2.039 x 10-6m3/kmol-min, and X = 0 in eq (1).

---(1)

- What is the rate of reaction when X = 0.9 at 188°C and at 25°C?
(i) At T= 188°C, k =0.0017m3/kmol-min

Substituting X=0.9 and k =0.017m3/kmol-min into (1);

---(1)

- What is the rate of reaction when X = 0.9 at 188°C and at 25°C?
(ii) From part (e) when T= 25°C, k = 2.039 x 10-6 m3/kmol-min

Substituting X=0.9 and k = k = 2.039 x 10-6 m3/kmol-min into (1);

- What would be the corresponding CSTR volume at 25°C to achieve 90% conversion at 188°C for a feed rate of 2 dm3/min?
Substituting the value of CA0, υ0 and –rA(at 288°C & X=0.9);