The decomposition of ethylene oxide at 690 K is monitored by measuring the total gas pressure as a function of time. The data obtained are t = 10 min,
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EBK GENERAL CHEMISTRY
- Iodomethane (CH3I) is a commonly used reagent in organic chemistry. When used properly, this reagent allows chemists to introduce methyl groups in many different useful applications. The chemical does pose a risk as a carcinogen, possibly owing to iodomethanes ability to react with portions of the DNA strand (if they were to come in contact). Consider the following hypothetical initial rates data: [DNA]0 ( mol/L) [CH3I]0 ( mol/L) Initial Rate (mol/Ls) 0.100 0.100 3.20 104 0.100 0.200 6.40 104 0.200 0.200 1.28 103 Which of the following could be a possible mechanism to explain the initial rate data? MechanismIDNA+CH3IDNACH3++IMechanismIICH3ICH3++ISlowDNA+CH3+DNACH3+Fastarrow_forwardCandle wax is a mixture of hydrocarbons. In the reaction of oxygen with candle w ax in Figure 11.2, the rate of consumption of oxygen decreased with time after the flask was covered, and eventually' the flame went out. From the perspective of the kinetic-molecular theory, describe what is happening in the flask. FIGURE 11.2 When a candle burns in a closed container, the flame will diminish and eventually go out. As the amount of oxygen present decreases, the rate of combustion will also decrease. Eventually, the rate of combustion is no longer sufficient to sustain the flame even though there is still some oxygen present in the vessel.arrow_forwardThe following equation represents a reversible decomposition: CaCO3(s)CaO(s)+CO2(g) Under what conditions will decomposition in a closed container proceed to completion so that no CaCO3 remains?arrow_forward
- The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?arrow_forwardSubstances that poison a catalyst pose a major concern for many engineering designs, including those for catalytic converters. One design option is to add materials that react with potential poisons before they reach the catalyst. Among the commonly encountered catalyst poisons are silicon and phosphorus, which typically form phosphate or silicate ions in the oxidizing environment of an engine. Group 2 elements are added to the catalyst to react with these contaminants before they reach the working portion of the catalytic converter. If estimates show that a catalytic converter will be exposed to 625 g of silicon during its lifetime, what mass of beryllium would need to be included in the design?arrow_forwardThe rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion present. The rate of decomposition was measured at constant temperature and pressure for various concentrations of H2O2and of KI. The data appear below. Determine the order of reaction for each substance, write the rate law, and evaluate the rate constant. Rate [H2OJ [Kll (mL min-’) (mol L ’) (mol L ’) 0.090 0.15 0.033 0.178 0.30 0.033 0.184 0.15 0.066arrow_forward
- 5. The high-temperature decomposition of dimethyl ether (DME) is (CH3)2O (g) → CH4 (g) + H₂ (g) + CO (g) The following data are partial pressures of DME as a function of time at 504 °C: t = 0 s PDME = 312 torr t = 390 s PDME = 264 torr t = 777 s PDME = 224 torr t = 1195 s PDME = 187 torr t = 3155 s PDME =78.5 torr a) Show that the reaction is first order. b) What is the value of the rate constant, k? c) What is the total gas pressure at 390 s? d) What is the total gas pressure when the reaction has gone to completion? e) What is the total gas pressure at t = 1000. s?arrow_forwardThe following data are for the gas phase decomposition of phosphine at 120 °C.PH3(g) 1/4 P4(g) + 3/2 H2(g) [ PH3 ], M 3.62×10-2 1.81×10-2 9.05×10-3 4.53×10-3 time, s 0 27.3 54.6 81.9 Hint: It is not necessary to graph these data.(1)The half life observed for this reaction is ________ s .(2)Based on these data, the rate constant for this _____ order reaction is ______ s -1.arrow_forwardPlease see attached picture for the problem to solve.arrow_forward
- Peroxynitric acid (HOONO2) is an unstable molecule that decomposes to nitric acid and oxygen: 2HOONO2(aq) → 2HNO3(aq) + O2(g)When the concentration of peroxynitic acid is graphed against time, the resulting plot is curved, but if the logarithm of this concentration is plotted, we instead get a straight line. Based on this, which statement is true? a) This decay is a second order in peroxynitric acid. b) The slope of the straight-line graph is the rate constant. c) One needs the concentration of peroxynitric acid to calculate its half-life. d) The rate law appears to be of the form -Δ[HOONO2]/Δt = k[HOONO2].arrow_forwarda At 500 K, in the presence of a copper surface, ethanol decomposes according to the equation C,H5OH(g) – CH3CHO(g) + H2(g) The pressure of C2H5OH was measured as a function of time, and the following data was obtained: Time (s) | P(C2H,ОН) (torr) 250. 100. 237 200. 224 300. 211 400. 198 500. 185 Since the pressure of a gas is directly proportional to the concentration of the gas, we can express the rate law for a gaseous reaction in terms of partial pressures. Using the preceding data, choose the correct rate law. Hint: To determine the order of the reaction with respect to C,H5OH, compare how the pressure of C,H5OH decreases with each time listing. Rate = k Rate = k[CH3CHO][H,j² Rate = k[C2H5OH][CH;CHO][H2] O Rate = k[C2H5OH]arrow_forwardThe decomposition of hydrogen peroxide was studied, and the following data were obtained at a particular temperature. Calculate the average rate of decomposition of 1.0 M hydrogen peroxide solution at 45 degrees Celsius for the time interval of 0 second to 1,800 seconds.arrow_forward
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