Question

Given the following initial rate law data for the following reaction: \(2HgCl_2(aq) + C_2O_4^{2-}(aq) \xrightarrow{k} Cl^-(aq) + 2CO_2(g) + Hg_2Cl_2(s)\) Trial \([HgCl_2]\) \([C_2O_4^{2-}]\) Initial Reaction Rate (M/min) 1 \(0.105\ M \) \(0.150\ M\) \(1.80 \times 10^{-5}\) 2 \(0.105\ M\) \(0.300\ M\) \(7.10 \times 10^{-5}\) 3 \(0.052\ M\) \(0.300\ M\) \(3.50 \times 10^{-5}\) Part A) Determine the order of reaction with respect to \(HgCl_2(aq)\) \(\circ\) Zero Order \(\circ\) First Order \(\circ\) Second Order \(\circ\) Third Order Part B) Determine the order of reaction with respect to \(C_2O_4^{2-}(aq)\) \(\circ\) Zero Order \(\circ\) First Order \(\circ\) Second Order \(\circ\) Third Order Part C) Determine the rate constant. k = 

          Given the following initial rate law data for the following reaction:
\(2HgCl_2(aq) + C_2O_4^{2-}(aq) \xrightarrow{k} Cl^-(aq) + 2CO_2(g) + Hg_2Cl_2(s)\)

Trial \([HgCl_2]\) \([C_2O_4^{2-}]\) Initial Reaction Rate (M/min)
1 \(0.105\ M \) \(0.150\ M\) \(1.80 \times 10^{-5}\)
2 \(0.105\ M\) \(0.300\ M\) \(7.10 \times 10^{-5}\)
3 \(0.052\ M\) \(0.300\ M\) \(3.50 \times 10^{-5}\)

Part A) Determine the order of reaction with respect to \(HgCl_2(aq)\)
\(\circ\) Zero Order
\(\circ\) First Order
\(\circ\) Second Order
\(\circ\) Third Order

Part B) Determine the order of reaction with respect to \(C_2O_4^{2-}(aq)\)
\(\circ\) Zero Order
\(\circ\) First Order
\(\circ\) Second Order
\(\circ\) Third Order

Part C) Determine the rate constant.
k =
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Given the following initial rate law data for the following reaction: 2HgCl2(aq) + C2O4^2-(aq) k Cl^-(aq) + 2CO2(g) + Hg2Cl2(s) Trial [HgCl2] [C2O4^2-] Initial Reaction Rate (M/min) 1 0.105 M 0.150 M 1.80 × 10^-5 2 0.105 M 0.300 M 7.10 × 10^-5 3 0.052 M 0.300 M 3.50 × 10^-5 Part A) Determine the order of reaction with respect to HgCl2(aq) ∘ Zero Order ∘ First Order ∘ Second Order ∘ Third Order Part B) Determine the order of reaction with respect to C2O4^2-(aq) ∘ Zero Order ∘ First Order ∘ Second Order ∘ Third Order Part C) Determine the rate constant. k =

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Chemistry: Structure and Properties
Chemistry: Structure and Properties
Nivaldo Tro 2nd Edition
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Given the following initial rate law data for the following reaction: HgCl2(aq) + Cl(aq) + 2CO2(g) + Hg2Cl2(s) Trial [HgCl2] [C2O4^2-] Initial Reaction Rate (M/min) 1 0.105 M 0.150 M 1.80 x 10^-5 2 0.105 M 0.300 M 7.10 x 10^-5 3 0.052 M 0.300 M 3.50 x 10^-5 O Zero Order O First Order O Second Order O Third Order O Zero Order O First Order O Second Order O Third Order Part C) Determine the rate constant.
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Transcript

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00:01 To determine the rate constant, we first need to calculate the, or determine the order with respect to each reactant.
00:09 To do that, we'll look at experiments 1 and 2, where we see that the concentration of a is constant at 0 .02 molar, and only the concentration of b is changing.
00:25 It doubles.
00:26 When it doubles, we see that the rate doubles.
00:36 We go from 0 .01 to 0 .02 molar b, and the rate goes from 0 .001 to 0 .002.
00:45 So if what we do to the concentration, we do to the rate, this is representative of first order.
00:54 Essentially, we doubled the concentration, we doubled the rate.
00:59 If we raise the 2 to 1, we get to, that means its first order.
01:07 Now if we look at experiments 1 and 3, we see that only the concentration of a is changing...
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