The '/s ' or per second term is present possibly to highlight the order of the reaction which will help you to solve for n in the PV=nRT equation.
my chemistry lab did the composition of hydrogen peroxide. i am having trouble trying to fugure...
From the data table determine the rate law for reactions 1-4 and calculate the value of k for each. Thanks I-IV BACKGROUND INFORMATION Given: 3% H2O2 Concentration= 0.88M & 1.5% H2O2 Concentration= 0.44 M •Calculation of H2O2 after mixing for parts I,II, IV= 0.704 M •Calculation of I^- after mixing for parts I,II, IV= 0.10 M •Calculation of Initial (mol/L-s) Filled in Table Now the solutions for Rate Order and Rate Constant are needed Reactants 8 ml 30% HO, 2...
Hi. I'm having trouble solving the rate law for my chemistry lab report sheet. I'm unsure if I'm doing it right. Below is my trials To calculate rate law, I choose experiment 1 and 2 for [I]x and experiment 2 and 3 for [H2O2]y. I got x=1 and y=1. This would make my rate law: rate = k [I-] [H2O2] Is this correct? Please help! Thanks in advance Trial [1] [H202] Rate (M/s) 1 3.00 x 10^-2 M 1.50 x...
2) 20 points in the lab you studied the decomposition of peroxide in ACIDIC solution If the reaction is run under BASIC conditions a different result is obtained. 2 H2O2(aq) + 2 H2O(l) + O2(g) The rate of reaction can be determined by measuring the rate at which the volume of O2 increases at a pressure of latm. Use the data below to determine the rate law including! the value of the rate constant, “rate =k [H2021 [ITY". Show your...
4. Experimental Procedure, Part A, Table 5.1 a. In Trial 1, what is the function of the sodium thiosulfate in studying the kinetics of the hydrogen peroxide-iodide reaction? b. Calculate the moles of S,0,2 that are consumed during the course of the reaction in Trial 1 produced during the course of the reaction. See equation 5.1 that are c. Calculate the moles of I Eveian 3 noitoviioA b d. Calculate the initial molar concentration of I (at time 0), [I...
Please help me find the average k, determining the order with respect to H2O2 (B) and H+ (y), and what is the complete rate law by including the experimentally numerical value of k, a, b and y. The lodine Clock: Initial Rate Law Kinetics - 71 Calculations Below is a description and outline for the calculations you need to complete for this laboratory. Make sure to include all of your calculations. Use extra paper if you need to Initial Concentrations:...
Final M of Acetone, Final M of H+ (hydrogen) and I2 (iodide)? Procedure: • Collect about 5 mL of each of the three solutions (IM HCl and 0.005M I/KI) in separate 10 ml beakers. Collect 4M acetone in an Erlenmeyer flask and cover it with a stopper it to avoid evaporation. Perform each of the runs three times. Record the individual time and take the average. Run #1 Use an automatic delivery pipet. Pipet exactly 200 ul acetone, 200 uL...
I can calculate molarity. But I don't know how to balance the acidic equation. Explain just about Balancing please. Thank you much! 3. The concentration of hydrogen peroxide, H2O2, in a solution is determined by titrating a 11.5 mL sample of the solution with permanganate ion, producing Mn2+ ion and oxygen gas. Balance the chemical equation for the redox reaction that occurs in acidic solution. H2O2 + MnO4 +H+ ► 02 + H2O + Mn2+ How will you able to...
I need help with the rate constants for trials 1 through 4. I put as much info as I thought would be necessary. The last question I posted I was told I didn't have enough info, so I hope this is enough. This is all the info I was given to solve the questions, so this has to be enough to solve them. Rate Constant, k', for the reaction occurring in Solution 1 (M1.51) NG 0.5 Info Rate Constant, k',...
2 H2O2(aq) + 2 H2O(l) + O2(g) 5. Hydrogen peroxide decomposes according to the equation above. a. An aqueous solution of H2O, that is 6.00 percent H,O, by mass has a density of 1.03 g ml. Calculate each of the following. (i) The original number of moles of H2O, in a 125 ml sample of the 6.00 percent H2O2 solution (ii) The number of moles of O,(g) that are produced when all of the H2O2 in the 125 mL sample...
Please show work I am not getting the correct answers 1. Hydrogen peroxide, H2O2, decomposes spontaneously through the following reaction. 2H2O2(aq) 2H2O(g) + O2(g) The kinetics are second order, and the half‐life is 17.3 min when a 1.75 M solution of H2O2 is made. What is the concentration of the solution after 24.8 min? 2. The decomposition of N2O5 occurs by the following reaction: 2N2O5(g) 4NO2(g) + O2(g) The rate constant is experimentally determined to be 3.4 x 10‐4 s‐1....