Consider the following reaction:

SO2Cl2(g)⇌SO2(g)+Cl2(g)

A reaction mixture is made containing an initial [SO2Cl2] of 2.4×10−2 M . At equilibrium, [Cl2]= 1.3×10−2 M .
Calculate the value of the equilibrium constant (Kc) .

the answer is a. co2, this would be colder than the : )

explanation:

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"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"

20 drops hope this