For the chemical reaction between mercuric chloride and potassium oxalate, the mass of Hg2Cl2 precipitated in different time intervals at 100oC is given belowExp. no[HgCl2]0 (M)[K2C2O4]0 (M)Time (Min)Hg2Cl2 formed (g)10.08360.404650.006820.08360.2021200.003130.04180.404600.0032What is the rate law expression of this reaction?

r = K[HgCl 2 ] 2 [K 2 C 2 O 4 ]

For the chemical reaction between mercuric chloride and potassium oxalate, the mass of Hg2Cl2 precipitated in different time intervals at 100oC is given belowExp. no[HgCl2]0 (M)[K2C2O4]0 (M)Time (Min)Hg2Cl2 formed (g)10.08360.404650.006820.08360.2021200.003130.04180.404600.0032What is the rate law expression of this reaction?

r = K[HgCl 2 ] 2 [K 2 C 2 O 4 ]

r = K[HgCl 2 ] 2 [K 2 C 2 O 4 ] 2

r = K[HgCl 2 ] 2 [K 2 C 2 O 4 ]

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For the chemical reaction between mercuric chloride and potassium oxalate, the mass of Hg₂Cl₂ precipitated in different time intervals at 100^oC is given below
Exp. no [HgCl₂]₀ (M) [K₂C₂O₄]₀ (M) Time (Min) Hg₂Cl₂ formed (g)
1 0.0836 0.404 65 0.0068
2 0.0836 0.202 120 0.0031
3 0.0418 0.404 60 0.0032
What is the rate law expression of this reaction?

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r = K[HgCl₂]²[K₂C₂O₄]²

r = K[HgCl₂][K₂C₂O₄]²

r = K[HgCl₂][K₂C₂O₄]

r = K[HgCl₂]²[K₂C₂O₄]

answer is D.

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Detailed Solution

r₁ = 0.0068 / 65 = 1.046 x 10^-4 gm / min
r₂ = 0.0031 / 120 = 2.583 x 10^-5gm / min
r₃ = 0.0032 / 60 = 5.333 x 10^-5 gm / min
From (1) and (2): order with respect to K₂C₂O₂ = 2
From (1) and (2): order with respect to HgCl₂ = 1

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Exp. no	[HgCl₂]₀ (M)	[K₂C₂O₄]₀ (M)	Time (Min)	Hg₂Cl₂ formed (g)
1	0.0836	0.404	65	0.0068
2	0.0836	0.202	120	0.0031
3	0.0418	0.404	60	0.0032