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A2 Equilibrium calculations help

Hey,

can can someone please tell me if I have done this question the right way:

the equation: SO2Cl2 = SO2 + Cl2
6.75g of SO2Cl2 in a container volume of 2.00dm3 heated to temp of 375 until equilibrium reached.
the equilibrium mixture was found to contain 0.0345 mol of Cl2.
calculate the value of Kc for this reaction at 375c and give units.

so i got 2.23 as the final answer, is this right?
star08
Hey,

can can someone please tell me if I have done this question the right way:

the equation: SO2Cl2 = SO2 + Cl2
6.75g of SO2Cl2 in a container volume of 2.00dm3 heated to temp of 375 until equilibrium reached.
the equilibrium mixture was found to contain 0.0345 mol of Cl2.
calculate the value of Kc for this reaction at 375c and give units.

so i got 2.23 as the final answer, is this right?


Initial moles of SO2Cl2 = 6.75/135 = 0.05 mol

@ equilibrium
------------
0.0345 mol of Cl2
0.0345 mol of SO2
0.05 - 0.0345 mol = 0.0155 mol of SO2Cl2

concentrations (it's in a 2 litre flask)
--------------
0.0345/2 = 0.01725
0.0155/2 = 0.00775

Kc = (0.01725 x 0.01725)/0.00775 = 0.0384 mol dm-3
Reply 2
Avatar for Andylol
Andylol
14
star08
Hey,

can can someone please tell me if I have done this question the right way:

the equation: SO2Cl2 = SO2 + Cl2
6.75g of SO2Cl2 in a container volume of 2.00dm3 heated to temp of 375 until equilibrium reached.
the equilibrium mixture was found to contain 0.0345 mol of Cl2.
calculate the value of Kc for this reaction at 375c and give units.

so i got 2.23 as the final answer, is this right?


SO2Cl2<=>SO2+Cl2SO_2Cl_2 <=> SO_2 + Cl_2
@Start: 6.75g of so2cl2 is 0.0500mol
@Equil: 0.0345mol of cl2 and 0.0345mol of so2
Which leaves 0.05 - 0.0345 = 0.0155mol of so2cl2

Kc=0.03452×0.034520.01552K_c = \frac {\frac {0.0345}{2} \times \frac {0.0345}{2}}{\frac {0.0155}{2}}
Which unfortunately is not the same as your answer. Oh, and you also missed out the units!
Reply 3
Avatar for Orihime
Orihime
2
star08
Hey,

can can someone please tell me if I have done this question the right way:

the equation: SO2Cl2 = SO2 + Cl2
6.75g of SO2Cl2 in a container volume of 2.00dm3 heated to temp of 375 until equilibrium reached.
the equilibrium mixture was found to contain 0.0345 mol of Cl2.
calculate the value of Kc for this reaction at 375c and give units.

so i got 2.23 as the final answer, is this right?

No# moles of SO2CL2 =6.75/135= 0.05
1SO2Cl2 = 1 SO2 + 1 Cl2
0.05-0.0345 = 0.0155 0.0345 0.0345
1:1 ratio
0.0155/2 0.0345/2 0.0345/2

0.00775 0.01725 0.01725


KC= 0.01725 * 0.01725 /0.00775= 0.0383951....

And that's how you do it my friend :cool: ( really easy 1:1 by-the-way!)
Reply 4
Avatar for Orihime
Orihime
2
Andylol
SO2Cl2<=>SO2+Cl2SO_2Cl_2 <=> SO_2 + Cl_2
@Start: 6.75g of so2cl2 is 0.0500mol
@Equil: 0.0345mol of cl2 and 0.0345mol of so2
Which leaves 0.05 - 0.0345 = 0.155mol of so2cl2

Kc=0.03452×0.03452[color="Magenta"]0.155[/color]2K_c = \frac {\frac {0.0345}{2} \times \frac {0.0345}{2}}{\frac {[color="Magenta"]0.155[/color]}{2}}
Which unfortunately is not the same as your answer. Oh, and you also missed out the units!



Your answer is wrong with a capital W :yes: It's meant to be 0.0155 not 0.155 ( hehehe ) :o:
Reply 5
Avatar for Andylol
Andylol
14
Orihime
Your answer is wrong with a capital W :yes: It's meant to be 0.0155 not 0.155 ( hehehe ) :o:


That's exactly what I meant :biggrin:

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