Copper Cycle Lab Report

2. Platinum and other group 10 metals often act as solid phase hydrogenation catalysts for unsaturated hydrocarbons such as propylene, CH3CHCH2. In order for the reaction to be catalyzed the propylene molecules must first adsorb onto the surface. In order to completely cover the surface of a piece of platinum that has an area of 1.50 cm² with propylene, a total of 3.45 x 10¹7 molecules are needed. Determine the mass of the propylene molecules that have been absorbed onto the platinum surface.

MN IN The 1995 Nobel Prize in Chemistry was shared by Paul Crutzen, F. Sherwood Rowland, and Mario Molina for their work concerning the formation and decomposition of ozone in the stratosphere. Rowland and Molina hypothesized that chlorofluorocarbons (CFCS) in the stratosphere break down upon exposure to UV radiation, producing chlorine atoms. Chlorine was previously identified as a catalyst in the breakdown of ozone into oxygen gas. Using the enthalpy of reaction for two reactions with ozone, determine the enthalpy of reaction for the reaction of chlorine with ozone. (1) CIO(g) + O,(g) → Cl(g) + 20,(g) AHxn = -122.8 kJ AHn = -285.3 kJ | rxn AHn = ? (3)°O + (3)OIƆ (3)1Ɔ+(3)*o (£) (3) 0E – (3)°07 (2) rxn %3D = UXHV kJ MacBook Pro Q Search or enter website name The & %23 $4 3. 4. 5. 7. 6. delete R H. K. re B. HE MOSISO command option

The acid-catalyzed hydrolysis of sucrose, C12H22O11 + H₂O + H+ -> C6H12O6 + C6H12O6 + H+ is known as "inversion of sucrose" because the angle, a, by which the solution rotates polarized light changes from positive to negative as the reaction proceeds (data from 30 degree C): t/hr a 0 78 2 71 4 12 18 24 42 65.10 44.60 32.40 22.45 2.30 48 -1.96 61 -9 86 95 -15.80 -17.25 -21.15 ∞ Use this data to show that the reaction is first order and determine its rate coefficient (at 30 degree C).

The compound diborane (B2H6) was at one time considered for use as a rocket fuel. Its combustion reaction is B2H6(g) + 3 O2(l) → 2 HBO2(g) + 2 H2O(l). The fact that HBO2, a reactive compound, was produced rather than the relatively inert B2O3 was a factor in the discontinuation of the investigation of the diborane as a fuel. What mass of liquid oxygen (LOX) would be needed to burn 234.4 g of B2H6? Answer in units of g. (part 2 of 2) What mass of HBO2 is produced from the combustion of 94.7 g of B2H6? Answer in units of g.

Answer the following questions about the conversion of the sucrose (C 12H 22O 11) in sugarcane to ethanol (C 2H 6O) and CO 2 according to the following unbalanced equation. In this way sugarcane is used as a renewable source of ethanol, which is used as a fuel additive in gasoline. C12H22O11(s) + H2O(l)---------->C2H6O(l) + CO2(g) sucrose ethanol a. What is the molar mass of sucrose? b. Balance the given equation. c. How many moles of ethanol are formed from 2 mol of sucrose? d. How many moles of water are needed to react with 10 mol of sucrose? e. How many grams of ethanol are formed from 0.550 mol of sucrose? f. How many grams of ethanol are formed from 34.2 g of sucrose? g. What is the theoretical yield of ethanol in grams from 17.1 g of sucrose? h. If 1.25 g of ethanol are formed in the reaction in part (g), what is the percent yield of ethanol?

(3) Evaluate the following uses of catalysis in terms of the goals of green chemistry (it is up to you if you want to refer to the 12 Principles or just the more general goals proposed by Dr. Lipke). Identify benefits as well as possible downsides. 2 a. A catalytic process that uses O, to oxidize an organic substrate dissolved in hexanes as a solvent, replacing a previous process that required the use of pyridine-N-oxide as an oxidant. b. A catalytic process that allows organic plant matter to be broken down into small organic molecules that can be used to produce fuels and fine chemicals that would otherwise be made from petroleum. c. A catalytic process that uses a mercury salt to catalyze the oxidation of methane to a methanol derivative, circumventing 2 a more traditional route using H, and CO to produce methanol as an intermediate.

Why does the product (a•b), rather than the sum (a + b) appear in the Law of Mass Action? This is sometimes brought up to demonstrate how/why nonlinear terms arise in differential equations. The law of mass action states that The rate of a chemical reaction involving an interaction of two or more chemical species is proportional to the product of the concentrations of the given species.  This is NOT an assignment...I'm just curious and trying to understand mathematical relations better. Thanks!

The catalytic decomposition of hydrogen peroxide can be expressed as: 2H2O2(aq) → 2H2O(l) + O2(g) Calculate the number of moles of oxygen gas produced from the completely catalyzed decomposition of 6.60 mL sample of a 3.5% solution of H2O2. The density of the 3.5% solution of H2O2 is 1.01 g/mL.

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За. Bromine and methanoic acid react in aqueous solution. Br, (aq) + HCO0Н (ад) — 2Br (aq) + 2H" (аq) + Со, (g) The reaction was monitored by measuring the volume of carbon dioxide produced as time progressed. o 5 10 15 20 25 [Source: © International Baccalaureate Organization 2019] 30 20 40 60 80 100 120 140 160 Time / s [Source: © International Baccalaureate Organization 2019] Determine from the graph the rate of reaction at 20 s, in cm³ s1, showing your working. 3b. Outline, with a reason, another property that could be monitored to measure the rate of this reaction. 3c. Describe one systematic error associated with the use of the gas syringe, and how the error affects the calculated rate. 3d. Identify one error associated with the use of an accurate stopwatch. Volume of carbon dioxide / cm T m mm mo

What is the Qc value for this equation? Which direction will the reaction shift? Given: CO(g)+H2O(g)=CO2(g)+H2(g) Kc = 1.0 • [CO2(g)]= 2.0M • [H2(g)]= 2.0 M • [CO(g)]= 1.0 M • [H2O(g)]= 1.0 M

8 Reactions between certain organic (alkyl) halides and water produce alcohols. Consider the overall reaction for t-butyl bromide (2-bromo-2-methylpropane). (CH3)3CBr(aq) + H2O(1) →(CH3)3COH(aq) + H*(aq) + Br "(ag) k[(CH3)3CB1]. The accepted mechanism for the The experimental rate law is rate = %3D reaction is shown below. (1) (CH3)3C-Br(aq) →(CH3)3C*(aq) + Br "(aq) [slow] (2) (CH3)3C*(aq) + H2O(1) →(CH3)3C-OH2*(aq) [fast] (3) (CH3)3C-OH2*(aq) →H*(aq) + (CH3)3C-OH(aq) [fast] a) Why doesn't H2O appear in the rate law? b) Write rate laws for the elementary steps. c) What intermediates appear in the mechanism? d) Show that the mechanism is consistent with the experimental rate law. ed to the of consumption of N

The reaction between peroxodisulphate (VI) ions, S2O8^2- and iodide ions, I- can be catalyzed by iron(III) ions, Fe^3+. a). Suggest a mechanism for the catalytic reaction   b). Sketch energy profile diagram for the catalyzed and uncatalyzed reaction s..ns.

Identify the reaction type for reactions #1, #2, and #3. Large Element Element #: %232: Hydrocarbon punodwo) B. CO2(g) (6)2) Element → CO, Large Element (6)o°H + +. # 3: B. punodwom Tap below to toggle through answer options and to identify the reaction type for each of the three reactions. The type of reaction for Reaction #1 The type of reaction for reaction for The type of Reaction #2 Reaction # 3 is Decomposition Combustion Tap here to select answer. +.

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Consider the reaction a A(aq) → bB(aq) (1) Where a and b are stoichiometric coefficients for the balanced chemical reaction The average reaction rate r can be measured if the concentration change of the reagents or products is known: 1 ΔΙΑ 1 Δ r = and r = At b At a where A and B notate the concentration of A and B in solution, and A is always defined as the difference between "final" and "initial": A[4] = [A],2 - [4],1 and At = t2 – t . - A particular case of eq. (1) could be A(aq) → 2 B(aq) If the initial concentration of B is 0.2569 mol L1, and after 415.6 s it increases to 0.4633 mol L1, what is the rate of the reaction in mol L1s? mol L-1 s1. (Use scientific notation)

The enzyme urease increases the rate of urea hydrolysis at pH 8.0 and 20 °C by a factor of 1014. Suppose that a given quantity of urease can completely hydrolyze a given quantity of urea in 19 minutes at pH 8.0 and 20 °C. How long would it take for this amount of urea to be hydrolyzed in the absence of urease at the same temperature and pH in sterile conditions? Include two significant figures in your answer. timeuncatalyzed years * TOOLS x10

I can’t understand part 17:33 please can you explain it for me ?