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Orders of a reaction ...
Have worked my way through some questions concerning the order of reactions - my thoughts are highlighted in lilac text. Confirmations or corrections of any sort would be absolutely wonderful ... thankyou in advance 
1) The rate equation for a reaction between substances A, B and C is of the form
rate = k[A]xy[C]z where x+y+z=4
The following data were obtained in a series of experiments at constant temperature. Please refer to attachment.
a) Use the data in the table to deduce
i) the order of the reaction with respect to A
ii) the order of the reaction with respect to B
iii) Hence deduce the order of the reaction with respect to C
Respect to A, order =2
Respect to B, order = 1
Respect to C, order = 1
I haven't come across an example in which the concentration actually gets smaller, so got somewhat confused with this. I did apply the same principle in practice, but a writen explanation of obtaining these orders would definately be useful in clarifying the procedure.
b) Calculate the value of the rate constant, k, stating its units, and also the value of the initial rate in experiment 4.
k = 8 * 10-5 / (0.12*0.2*0.2)
= 0.2
Units I got are mol-2 dm9 s-1
Initial rate in expt 4
r = 0.2 * 0.12*0.1*0.1
= 2 * 10-5
2) Esters can be hydrolyssed by heating with a dilute hydrochloric acid to form an alcohol and a carboxylic acid. The rate equation for the hydrolysis of this ester is
rate = k [CH3COOCH3][H+]
i) Calculate the value of the rate constant at this temperature and give its units.
k = rate / {[CH3COOCH3][H+]}
= 2.4*10-3 / (0.5*1)
= 4.8 * 10-3
The units I got are mol-1 dm3 s-1
ii) Calculate the initial rate of the reaction if the concentration of hydrochloric acid is increased to 1.5M but all other conditions remain unchanged.
rate = 4.8*10-3 * 0.5 * 1.5
= 3.6 * 10-3
iii) Calculate the initial rate of the reaction at 320 K if more solvent is added to the original mixture so that the total volume is doubled.
Im at a total end with this question. Having trouble tryna figure out what values to use ...
1) The rate equation for a reaction between substances A, B and C is of the form
rate = k[A]xy[C]z where x+y+z=4
The following data were obtained in a series of experiments at constant temperature. Please refer to attachment.
a) Use the data in the table to deduce
i) the order of the reaction with respect to A
ii) the order of the reaction with respect to B
iii) Hence deduce the order of the reaction with respect to C
Respect to A, order =2
Respect to B, order = 1
Respect to C, order = 1
I haven't come across an example in which the concentration actually gets smaller, so got somewhat confused with this. I did apply the same principle in practice, but a writen explanation of obtaining these orders would definately be useful in clarifying the procedure.
b) Calculate the value of the rate constant, k, stating its units, and also the value of the initial rate in experiment 4.
k = 8 * 10-5 / (0.12*0.2*0.2)
= 0.2
Units I got are mol-2 dm9 s-1
Initial rate in expt 4
r = 0.2 * 0.12*0.1*0.1
= 2 * 10-5
2) Esters can be hydrolyssed by heating with a dilute hydrochloric acid to form an alcohol and a carboxylic acid. The rate equation for the hydrolysis of this ester is
rate = k [CH3COOCH3][H+]
i) Calculate the value of the rate constant at this temperature and give its units.
k = rate / {[CH3COOCH3][H+]}
= 2.4*10-3 / (0.5*1)
= 4.8 * 10-3
The units I got are mol-1 dm3 s-1
ii) Calculate the initial rate of the reaction if the concentration of hydrochloric acid is increased to 1.5M but all other conditions remain unchanged.
rate = 4.8*10-3 * 0.5 * 1.5
= 3.6 * 10-3
iii) Calculate the initial rate of the reaction at 320 K if more solvent is added to the original mixture so that the total volume is doubled.
Im at a total end with this question. Having trouble tryna figure out what values to use ...
[QUOTE="h1nna"]Have worked my way through some questions concerning the order of reactions - my thoughts are highlighted in lilac text. Confirmations or corrections of any sort would be absolutely wonderful ... thankyou in advance
1) The rate equation for a reaction between substances A, B and C is of the form
rate = k[A]xy[C]z where x+y+z=4
The following data were obtained in a series of experiments at constant temperature. Please refer to attachment.
a) Use the data in the table to deduce
i) the order of the reaction with respect to A
ii) the order of the reaction with respect to B
iii) Hence deduce the order of the reaction with respect to C
Respect to A, order =2
Respect to B, order = 1
Respect to C, order = 1
I haven't come across an example in which the concentration actually gets smaller, so got somewhat confused with this. I did apply the same principle in practice, but a writen explanation of obtaining these orders would definately be useful in clarifying the procedure.
b) Calculate the value of the rate constant, k, stating its units, and also the value of the initial rate in experiment 4.
k = 8 * 10-5 / (0.12*0.2*0.2)
= 0.2
Units I got are mol-2 dm9 s-1
Initial rate in expt 4
r = 0.2 * 0.12*0.1*0.1
= 2 * 10-5
2) Esters can be hydrolyssed by heating with a dilute hydrochloric acid to form an alcohol and a carboxylic acid. The rate equation for the hydrolysis of this ester is
rate = k [CH3COOCH3][H+]
i) Calculate the value of the rate constant at this temperature and give its units.
k = rate / {[CH3COOCH3][H+]}
= 2.4*10-3 / (0.5*1)
= 4.8 * 10-3
The units I got are mol-1 dm3 s-1
ii) Calculate the initial rate of the reaction if the concentration of hydrochloric acid is increased to 1.5M but all other conditions remain unchanged.
rate = 4.8*10-3 * 0.5 * 1.5
= 3.6 * 10-3
iii) Calculate the initial rate of the reaction at 320 K if more solvent is added to the original mixture so that the total volume is doubled.
Im at a total end with this question. Having trouble tryna figure out what values to use ...[/C]
but they don't get smaller if you read backwards (i.e. expt 4 first then 3 etc)
yes, all your orders are correct
The units of the rate constant only depends on the total order (4)
mol dm^-3 s^-1 = k(mol dm-3)^4
k is in dm9 mol-3 s-1
sorry, I can't be arsed to check the others ... I've run out of steam....time for bedddd sed zebedee
1) The rate equation for a reaction between substances A, B and C is of the form
rate = k[A]xy[C]z where x+y+z=4
The following data were obtained in a series of experiments at constant temperature. Please refer to attachment.
a) Use the data in the table to deduce
i) the order of the reaction with respect to A
ii) the order of the reaction with respect to B
iii) Hence deduce the order of the reaction with respect to C
Respect to A, order =2
Respect to B, order = 1
Respect to C, order = 1
I haven't come across an example in which the concentration actually gets smaller, so got somewhat confused with this. I did apply the same principle in practice, but a writen explanation of obtaining these orders would definately be useful in clarifying the procedure.
b) Calculate the value of the rate constant, k, stating its units, and also the value of the initial rate in experiment 4.
k = 8 * 10-5 / (0.12*0.2*0.2)
= 0.2
Units I got are mol-2 dm9 s-1
Initial rate in expt 4
r = 0.2 * 0.12*0.1*0.1
= 2 * 10-5
2) Esters can be hydrolyssed by heating with a dilute hydrochloric acid to form an alcohol and a carboxylic acid. The rate equation for the hydrolysis of this ester is
rate = k [CH3COOCH3][H+]
i) Calculate the value of the rate constant at this temperature and give its units.
k = rate / {[CH3COOCH3][H+]}
= 2.4*10-3 / (0.5*1)
= 4.8 * 10-3
The units I got are mol-1 dm3 s-1
ii) Calculate the initial rate of the reaction if the concentration of hydrochloric acid is increased to 1.5M but all other conditions remain unchanged.
rate = 4.8*10-3 * 0.5 * 1.5
= 3.6 * 10-3
iii) Calculate the initial rate of the reaction at 320 K if more solvent is added to the original mixture so that the total volume is doubled.
Im at a total end with this question. Having trouble tryna figure out what values to use ...[/C]
but they don't get smaller if you read backwards (i.e. expt 4 first then 3 etc)
yes, all your orders are correct
The units of the rate constant only depends on the total order (4)
mol dm^-3 s^-1 = k(mol dm-3)^4
k is in dm9 mol-3 s-1
sorry, I can't be arsed to check the others ... I've run out of steam....time for bedddd sed zebedee
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