In the reaction A -> B, the plot of Ln[A] versus t resulted in a straight line with equation (Ln[A] = -0.08t + 1.2). What is the initial concentration of A? * 0.18 M 0.08 M 1.2 M 0.83 M 3.32 M
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- At the start of the reaction, the concentration of YOI is equal to 5.142 M. After 118.0 seconds, its concentration was reduced to 2.361 M. Meanwhile, another run of the same reaction but with 3.789 M [YOI]0 showed that after 110.0 seconds, a 1.350 M decrease in concentration of YOI was observed. Based on these: 1. How much YOI will be consumed if a run with [YOI]0 = 1.234 M is allowed to form MIYA for 4.00 minutes.Find the rate law constant and the order of the reaction a and b K[H2O]a[I-]b Concentrations: Starch 0.01 mol/L Buffer 0.5 mol/L Thiosulfate 0.02 mol/L Kl 0.25 mol/L H2O2 0.12 mol/L New concentrations after dilutions Reaction # V S2O3 (ml) V Kl (ml) V H2O2 (ml) Final volume (ml) S2O3 final M (mol/L) Kl final M (mol/L H2O2 final M (mol/L) t initial (s) t final (s) Rate S2O3 Rate of the reaction Log of rates Log of I Log of H2O2 1 5 6 5 100 0.001 0.015 0.006 81 718 7.85E-07 7.85E-07 -6.105169428 -1.823908741 -2.22184875 2 5 6 10 100 0.001 0.015 0.012 241 572 1.51E-06 1.51E-06 -5.820857989…Given below is the dissociation of NH3 in water having a Kb value of 1.8 × 10-5. The reaction started with the equilibration of 0.65 M NH3. A common ion that is 0.25 M NH4Cl, was added to the initial solution and waited for some time for the reaction to reach equilibrium once again. NH3(aq) + H2O(l) ↔ NH4+(aq) + OH-(aq) Determine the pH of the solution given after the addition of the common ion. The Kw of water is 1.0 × 10-14.
- The efficiency of a particular catalyst is highly dependent on its zirconium content. The starting material for this preparation is received in batches that assay between 68% and 84% ZrCl4. Routine analysis based on precipitation of AgCl is feasible, if having been established that there are no sources of chloride ion other than the ZrCl4 in the sample. (a) What sample mass should be taken to ensure an AgCl precipitate that weighs at least 0.400g? (b) If this sample mass is used, what is the maximum mass of AgCl that can be expected in this analysis? (c) To simplify calculations, what sample mass should be taken to have the percentage of ZrCl4 exceed the mass of AgCl produced by a factor of 100?A general reaction written as 2A + 2B → C + 2D is studied and yields the following data. [A]0 [B]0 Initial Δ[C]/Δt 0.100 M 0.100 M 4.00 × 10–5 mol/L • s 0.200 M 0.100 M 4.00 × 10–5 mol/L • s 0.100 M 0.200 M 8.00 × 10–5 mol/L • s For the first of the reactions in the table of data, determine –Δ[B]/Δt. Question 5 options: A) 8.00 × 10–5 B) 1.60 × 10–4 C) 4.00 × 10–5 D) 2.00 × 10–5 E) none of theseA rate is equal to 0.0200 M/s. If [A] = 0.100 M and rate = k[A]0[B]2, what is the new rate if the concentration of [A] is increased to 0.200 M? It says the answer was 0.0200 but im not sure, could you check and give me a step by step solution?
- 2.3. A mixture of Na and K (m(K+Na) = 6.2 g) was dissolved in excess of water. In this reaction 2.24 L of gas were formed. Find mass fraction (in %) of K and Na in the mixtureI included my data table please answer the following questions Find the delta(S2O8^2-),M (2nd to last row on data table), THEN find the Reaction rate for all 4 runs (last row). IGNORE THE NUMBERS THAT ARE IN THOSE COLOUMNS RIGHT MOW THEY ARE MOST LIKELY INCORRECT! Next find the average rate consant k for the 4 runs using the numbers you calculated.Reaction of interest : S2O82-(aq) + 3I- (aq)→ 2SO42-(aq) + I3-(aq). rate= k[S2O82-]1[I-]1.