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- Silicon forms a series of compounds analogous to the al-kanes and having the general formula SinH2n+2. The first of these compounds is silane, SiH4, which is used in the electronics industry to produce thin ultrapure silicon films. SiH4(g) is somewhat difficult to work with because it is py-ropboric at room temperature—meaning that it bursts into flame spontaneously when exposed to air. (a) Write an equation for the combustion of SiH4(g). (The reaction is analogous to hydrocarbon combustion, and SiO2 is a solid under standard conditions. Assume the water produced will be a gas.) (b) Use the data from Appendix E to calculate ? for this reaction. (c) Calculate G and show that the reaction is spontaneous at 25°C. (d) Compare G for this reaction to the combustion of methane. (See the previous problem.) Are the reactions in these two exercises enthalpy or entropy driven? Explain.Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.a 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]
- 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].1a) The decomposition of ethanol at some constant temperature (above 500°C), over a copper surface, C2H5OH(g)--> CH3CHO(g) + H2(g) was studied by monitoring the total pressure with time.The following data were obtained: t (s) Ptotal (torr) 0 120 45 131 139 154 233 177 376 212 380 213 What will be the total pressure at t = 462 s? 1b) What is the rate constant (k)?(Include appropriate units.)The data below were collected for the following reaction at 35° C: 2(CH3)3 CSOH(g) → (CH3)3CS(O)SC(CH3)3 (g) Time (min) [(CH3)3 CSOH] (mol · L−¹) 0.0 1.554 10.8 0.661 19.1 0.343 37.0 0.083 59.5 0.014 75.1 0.004 Part C From the slope of the appropriate plot, determine the value of the rate constant at this temperature. VG ΑΣΦ Submit Request Answer ? 5-1
- The following data are for the gas phase decomposition of phosphine at 120 °C. PH3(g)- → 1/4 P(g) + 3/2 H2(g) [ PH3 ), M 5.30x102 2.65x102 1.33x102 57.0 6.65x103 85.5 time, s 28.5 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is (2) Based on these data, the rate constant for this order reaction is Submit Answer Retry Entire Group 9 more group attempts remainingIn aqueous solution, hypobromite ion, BrO-, reacts to produce bromate ion, BrO3 -, and bromide ion, Br-, according to the following chemical equation.3 BrO-(aq) →→ BrO3 -(aq) + 2 Br-(aq)A plot of 1/[BrO-] vs. time is linear and the slope is equal to 0.056 M-1s-1. If the initial concentration of BrO- is 0.90 M, how long will it take one-half of the BrO- ion to react? In aqueous solution, hypobromite ion, BrO-, reacts to produce bromate ion, BrO3 -, and bromide ion, Br-, according to the following chemical equation.3 BrO-(aq) BrO3 -(aq) + 2 Br-(aq)A plot of 1/[BrO-] vs. time is linear and the slope is equal to 0.056 M-1s-1. If the initial concentration of BrO- is 0.90 M, how long will it take one-half of the BrO- ion to react? 5.0 × 10-2 s 12 s 8.0 s 20. sIf the temperature of a chemical reaction is raised by 10°C, the rate of reaction is increased by a factor of aboutA. 2B. 4C. 1.5D. 3
- Nitric oxide reacts with hydrogen to release large amounts of chemiluminescence with the characteristics of the highly cytotoxic species. The following data were measured for the reaction of nitric oxide with hydrogen: Data number 1 2 3 2 NO(g) + 2 H₂(g) → N₂(g) + 2 H₂O(g) [NO] (M) 0.1 0.1 0.2 [H₂] (M) 0.1 0.2 0.1 Based on the data, (a) Determine the rate law for this reaction. (b) Calculate the rate constant. (c) Calculate the rate when [NO] = 0.050 M and [H₂] = 0.150 M Initial rate (M/S) 1.23 x 10-³ 2.46 x 10-³ 4.92 x 10-³Consider the following gas phase reaction at constant volume: 2CH2N2(g) −→ 2N2(g) + C2H4(g) i) Given that the initial pressure is p0 calculate the total pressure after three quarters of the CH2N2(g) has reacted. ii) Derive an equation which shows how the total pressure varies as a function of the fraction, α, of the CH2N2(g) that has reacted. iii) Sketch a graph which shows how the pressure varies as a function of αThe following data are for the gas phase decomposition of dimethyl ether at 500 °C. CH3OCH3(g) –→ → CH4(g) + H2(g) + CO(g) |[ СH3ОCH3 ], М |3.75х10-2 |1.88×10-2 9.40×10-3 4.70×10-3 time, min 21.0 42.0 63.0 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is min . (2) Based on these data, the rate constant for this v order reaction is min -1