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    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?
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    (Original post by 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
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    (Original post by 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?
    SO_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

    K_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!
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    (Original post by 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!)
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    (Original post by Andylol)
    SO_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

    K_c = \frac {\frac {0.0345}{2} \times \frac {0.0345}{2}}{\frac {<font color="Magenta">0.155</font>}{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:
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    (Original post by 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
 
 
 
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