For the reaction of nitrogen monoxide, NO, with chlorine, Cl2,
the observed rate law is
What is the reaction order with respect to nitrogen monoxide and with respect to Cl2? What is the overall order?
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- At 500 K in the presence of a copper surface, ethanol decomposes according to the equation C2H5OH(g)CH3CHO(g)+H2(g) The pressure of C2H5OH was measured as a function of time and the following data were obtained: Time(s) PC2H5OH(torr) 0 250. 100. 237 200. 224 300. 211 400. 198 500. 185 Since the pressure of a gas is directly proportional to the concentration of gas, we can express the rate law for a gaseous reaction in terms of partial pressures. Using the above data, deduce the rate law, the integrated rate law, and the value of the rate constant, all in terms of pressure units in atm and time in seconds. Predict the pressure of C2H5OH after 900. s from the start of the reaction. (Hint: To determine the order of the reaction with respect to C2H5OH, compare how the pressure of C2H5OH decreases with each time listing.)arrow_forwardAt 573 K, gaseous NO2(g) decomposes, forming NO(g) and O2(g). If a vessel containing NO2(g) has an initial concentration of 1.9 102 mol/L, how long will it take for 75% of the NO2(g) to decompose? The decomposition of NO2(g) is second-order in the reactant and the rate constant for this reaction, at 573 K, is 1.1 L/mol s.arrow_forwardChlorine dioxide, ClO2, is a reddish-yellow gas that is soluble in water. In basic solution it gives ClO3 and ClO2 ions. 2ClO2(aq)+2OH(aq)ClO3(aq)+ClO2(aq)+H2O To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of ClO2 was determined. Obtain the rate law and the value of the rate constant.arrow_forward
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- Ozone, O3, in the Earths upper atmosphere decomposes according to the equation 2 O3(g) 3 O2(g) The mechanism of the reaction is thought to proceed through an initial fast, reversible step followed by a slow, second step. Step 1: Fast, reversible O3(g) O2(g) + O(g) Step 2: Slow O3(g) + O(g) 2 O2(g) (a) Which of the steps is rate-determining? (b) Write the rate equation for the rate-determining steparrow_forwardIn the gas phase, the production of phosgene from chlorine and carbon monoxide is assumed to proceed by the following mechanism: Cl2k1k12ClFastEquilibriumCl+COk2k2COClFastEquilibriumCOCl+Cl2k3COCl2+ClSlow2Clk1Cl2Fast Overall reaction: CO + Cl2 COCl2 a. Write the rate law for this reaction. b. Which species are intermediates?arrow_forwardOne experimental procedure that can be used to determine the rate law of a reaction is the method of initial rates. What data are gathered in the method of initial rates, and how are these data manipulated to determine k and the orders of the species in the rate law? Are the units for k. the rate constant, the same for all rate laws? Explain. If a reaction is first order in A, what happens to the rate if [A] is tripled? If the initial rate for a reaction increases by a factor of 16 when [A] is quadrupled, what is the order of n? If a reaction is third order in A and [A] is doubled, what happens to the initial rate? If a reaction is zero order, what effect does [A] have on the initial rate of a reaction?arrow_forward
- For the reaction A+BC, explain at least two ways in which the rate law could be zero order in chemical A.arrow_forwardThe reaction NO(g) + 1/2 Cl2(g) NOCl(g) is first-order in [Cl2] and second-order with respect to [NO]. Under a given set of conditions, the initial rate of this reaction is 620 106 mol/L s. What is the rate of this reaction if the concentration of NO is doubled and the concentration of Cl2 is reduced to half the original value? (a) 6.20 106 mol/L s (b) 124 105 mol/L s (c) 2.48 105 mol/L s (d) 4.96 105 mol/L sarrow_forwardThe isomerization of cyclopropane, C3H6, is believed to occur by the mechanism shown in the following equations: C3H6+C3H5k1C3H6+C3H6(Step1)C3H6k2C2=CHCH3(Step2) Here C3H6 is an excited cyclopropane molecule. At low pressure, Step 1 is much slower than Step 2. Derive the rate law for this mechanism at low pressure. Explain.arrow_forward
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