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chemistry and chemical reactivity

Questions and Answers of Chemistry And Chemical Reactivity

An organic compound contains carbon (71.17%), hydrogen (5.12%) with the remainder nitrogen. Dissolving 0.177 g of the compound in 10.0 g of benzene gives a solution with a vapor pressure of 94.16 mm
In chemical research we often send newly synthesized compounds to commercial laboratories for analysis. These laboratories determine the weight percent of C and H by burning the compound and
When salts of Mg2+, Ca2+, and Be2+ are placed in water, the positive ion is hydrated (as is the negative ion). Which of these three cations is most strongly hydrated? Which one is least strongly
Explain why a cucumber shrivels up when it is placed in a concentrated solution of salt.
If you dissolve equal molar amounts of NaCl and CaCl2 in water, the CaCl2 lowers the freezing point of the water almost 1.5 times as much as the NaCl. Why?
Outline a two-dimensional unit cell for the pattern shown here. If the black squares are labeled A and the white squares are B, what is the simplest formula for a “compound” based on this pattern?
A portion of the crystalline lattice for potassium is illustrated below.(a) In what type of unit cell are the K atoms arranged?(b) If one edge of the potassium unit cell is 533 pm, what is the
One way of viewing the unit cell of perovskite was illustrated in Example 12.2. Another way is shown here. Prove that this view also leads to a formula of CaTiO3.Data given in Example 12.2
The unit cell of silicon carbide, SiC, is illustrated below.(a) In what type of unit cell are the (dark gray) C atoms arranged?(b) If one edge of the silicon carbide unit cell is 436.0 pm, what is
Rutile, TiO2, crystallizes in a structure characteristic of many other ionic compounds. How many formula units of TiO2 are in the unit cell illustrated here? (The oxide ions marked by an x are wholly
Cuprite is a semiconductor. Oxide ions are at the cube corners and in the cube center. Copper ions are wholly within the unit cell.(a) What is the formula of cuprite?(b) What is the oxidation number
The mineral fluorite, which is composed of calcium ions and fluoride ions, has the unit cell shown here.(a) What type of unit cell is described by the Ca2+ ions?(b) Where are the F− ions located,
The osmotic pressure exerted by seawater at 25°C is about 27 atm. Calculate the concentration of ions dissolved in seawater that is needed to give an osmotic pressure of this magnitude.
Give the relative rates of disappearance of reactants and formation of products for each of the following reactions. (a) 2 03(g) → 3 O₂(g) (b) 2 HOF(g) → 2 HF(g) + O₂(g)
Give the relative rates of disappearance of reactants and formation of products for each of the following reactions. (a) 2 NO(g) + Br₂(g) → 2 NOBr(g) (b) N₂(g) + 3 H₂(g) → 2 NH3(g)
Experimental data are listed here for the reaction A → 2 B.(a) Prepare a graph from these data; connect the points with a smooth line; and calculate the rate of change of [B] for each 10-second
In the reaction 2 O3(g) → 3 O2(g), the rate of formation of O2 is 1.5 × 10−3 mol/L ∙ s. What is the rate of decomposition of O3?
Phenyl acetate, an ester, reacts with water according to the equationThe data in the table were collected for this reaction at 5°C.(a) Plot the phenyl acetate concentration versus time, and describe
Using the rate equation Rate = k[A]2 [B], define the order of the reaction with respect to A and B. What is the total order of the reaction?
A reaction has the experimental rate equation Rate = k[A]2. How will the rate change if the concentration of A is tripled? If the concentration of A is halved?
The reaction between ozone and nitrogen dioxide at 231 K is first-order in both [NO2] and [O3].(a) Write the rate equation for the reaction.(b) If the concentration of NO2 is tripled (and [O3] is not
The data in the table are for the reaction of NO and O2 at 660 K.(a) Determine the order of the reaction for each reactant.(b) Write the rate equation for the reaction.(c) Calculate the rate
Nitrosyl bromide, NOBr, is formed from NO and Br2:Experiments show that this reaction is second-order in NO and first-order in Br2.(a) Write the rate equation for the reaction.(b) How does the
The reactionwas studied at 904°C, and the data in the table were collected.(a) Determine the order of the reaction for each reactant.(b) Write the rate equation for the reaction.(c) Calculate the
Data for the following reaction are given in the table below.(a) What is the rate law for this reaction?(b) What is the rate constant for the reaction?(c) What is the initial rate of the reaction in
Data for the reaction NO(g) + 1⁄2 O2(g) → NO2(g) are given (for a particular temperature) in the table.(a) What is the rate law for this reaction?(b) What is the rate constant for the
The rate equation for the hydrolysis of sucrose to fructose and glucoseis −Δ[sucrose]/Δt = k[C12H22O11]. After 27 minutes at 27°C, the sucrose concentration decreased from 0.0146 M to 0.0132 M.
The decomposition of SO2Cl2 is a first-order reaction:The rate constant for the reaction is 2.8 ×10−3 min−1 at 600 K. If the initial concentration of SO2Cl2 is 1.24 × 10−3 mol/L, how long
The conversion of cyclopropane to propene (Example 14.5) occurs with a first-order rate constant of 2.42 × 10−2 h−1. How long will it take for the concentration of cyclopropane to decrease from
The decomposition of nitrogen dioxide at a high temperatureis second-order in this reactant. The rate constant for this reaction is 3.40 L/mol ∙ min. Determine the time needed for the concentration
Hydrogen peroxide, H2O2(aq), decomposes to H2O(ℓ) and O2(g) in a reaction that is first-order in H2O2 and has a rate constant k = 1.06 × 10−3 min−1 at a given temperature.(a) How long will it
The decomposition of ammonia on a metal surface to form N2 and H2 is a zero-order reaction (Figure 14.7c). At 873°C, the value of the rate constant is 1.5 × 10−3 mol/L ∙ s. How long it will
At 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 × 10−2 mol/L, how long will it take for 75% of the NO2(g) to
The dimerization of butadiene, C4H6, to form 1,5-cyclooctadiene is a second-order process that occurs when the diene is heated. In an experiment, a sample of 0.0087 mol of C4H6 was heated in a 1.0-L
Gaseous azomethane, CH3N=NCH3, decomposes in a first-order reaction when heated:The rate constant for this reaction at 600 K is 0.0216 min−1. If the initial quantity of azomethane in the flask is
Hydrogen iodide decomposes when heated, forming H2(g) and I2(g). The rate law for this reaction is −Δ[HI]/Δt = k[HI]2. At 443°C, k = 30. L/mol · min. If the initial HI(g) concentration is 1.5
The rate equation for the decomposition of N2O5 (giving NO2 and O2) is Rate = k[N2O5]. The value of k is 6.7 × 10−5 s−1 for the reaction at a particular temperature.(a) Calculate the half-life
The decomposition of SO2Cl2is first-order in SO2Cl2, and the reaction has a half life of 245 minutes at 600 K. If you begin with 3.6 × 10−3 mol of SO2Cl2 in a 1.0-L flask, how long will it take
Data for the decomposition of dinitrogen monoxideon a gold surface at 900°C are given below. Verify that the reaction is first-order by preparing a graph of ln[N2O] versus time. Derive the rate
The compound Xe(CF3)2 decomposes in a first order reaction to elemental Xe with a half-life of 30. minutes. If you place 7.50 mg of Xe(CF3)2 in a flask, how long must you wait until only 0.25 mg of
The radioactive isotope 64Cu is used in the form of copper(II) acetate to study Wilson’s disease. The isotope has a half-life of 12.70 hours. What fraction of radioactive copper(II) acetate remains
Ammonia decomposes when heated according to the equationThe data in the table for this reaction were collected at a high temperature. Plot ln [NH3] versus time and 1/[NH3] versus time. What is the
Radioactive gold-198 is used in the diagnosis of liver problems. The half-life of this isotope is 2.7 days. If you begin with a 5.6-mg sample of the isotope, how much of this sample remains after 1.0
The decomposition of HOF occurs at 25°C.Using the data in the table below, determine the rate law, and then calculate the rate constant. HOF(g) → HF(g) + 1/2O₂(g)
Gaseous NO2 decomposes at 573 K.The concentration of NO2 was measured as a function of time. A graph of 1/[NO2] versus time gives a straight line with a slope of 1.1 L/mol ∙ s. What is the rate law
Butadiene, C4H6(g), dimerizes when heated, forming 1,5-cyclooctadiene, C8H12. The data in the table were collected.(a) Use a graphical method to verify that this is a second-order reaction.(b)
For the reaction C2F4 → 1⁄2 C4F8, a graph of 1/ [C2F4] versus time gives a straight line with a slope of +0.04 L/mol ∙ s. What is the rate law for this reaction?
Calculate the activation energy, Ea, for the reactionfrom the observed rate constants: k at 25°C = 3.46 × 10−5 s−1 and k at 55°C = 1.5 × 10−3 s−1. 2 N₂O5 (g) →→→ 4 NO₂(g) +
When heated, cyclopropane is converted to propene (Example 14.5). Rate constants for this reaction at 470°C and 510°C are k =1.10 × 10−4 s−1 and k = 1.02 × 10−3 s−1, respectively.
When heated to a high temperature, cyclobutane, C4H8, decomposes to ethylene:The activation energy, Ea, for this reaction is 260 kJ/mol. At 800 K, the rate constant k =0.0315 s−1. Determine the
If the rate constant for a reaction triples when the temperature rises from 3.00 × 102 K to 3.10 × 102 K, what is the activation energy of the reaction?
The reaction of H2 molecules with F atomshas an activation energy of 8 kJ/mol and an enthalpy change of −133 kJ/mol. Draw a diagram similar to Figure 14.11 for this process. Indicate the activation
Answer the following questions based on the diagram below.(a) Is the reaction exothermic or endothermic?(b) Does the reaction occur in more than one step? If so, how many?
According to the Michaelis–Menten model, if 1/ Rate is plotted versus 1/[S], the intercept of the plot (when 1/[S] = 0) is 1/Ratemax. Using the data below at a given temperature, for a given enzyme
The enzyme carbonic anhydrase catalyzes the transformation of carbon dioxide into hydrogen carbonate ions. This reaction was studied by H. DeVoe and G. B. Kistiakowsky (Journal of the American
To which species should an enzyme bind best: the substrate, transition state, or product of a reaction?
What is the rate law for each of the following elementary reactions? (a) NO(g) + NO3(g) → 2 NO₂(g) (b) Cl(g) + H₂(g) → HCl(g) + H(g) (c) (CH3)3CBr(aq) → (CH3)3C+ (aq) + Br¯(aq)
Ozone, O3, in the Earth’s upper atmosphere decomposes according to the equationThe mechanism of the reaction is thought to proceed through an initial fast, reversible step followed by a slow,
What is the rate law for each of the following elementary reactions? (a) Cl(g) + ICI(g) → I(g) + Cl₂(g) (b) O(g) + O2(g) → 2 O₂(g) (c) 2 NO₂(g) → N₂O4(g)
The reaction of NO2(g) and CO(g) is thought to occur in two steps to give NO and CO2:Step 1: SlowStep 2: Fast(a) Show that the elementary steps add up to give the overall, stoichiometric equation.(b)
A proposed mechanism for the reaction of NO2 and CO isStep 1: Slow, endothermicStep 2: Fast, exothermicOverall Reaction: Exothermic(a) Identify each of the following as a reactant, product, or
The mechanism for the reaction of CH3OH and HBr is believed to involve two steps. The overall reaction is exothermic.Step 1: Fast, endothermicStep 2: Slow(a) Write an equation for the overall
Data for the following reaction are given in the table.What is the order of the reaction with respect to [NO] and [Br2], and what is the overall order of the reaction? 2 NO(g) + Br₂(g) → 2
To determine the concentration dependence of the rate of the reactionyou might measure [OH−] as a function of time using a pH meter. (To do so, you would set up conditions under which [H2PO3−]
A reaction has the following experimental rate equation: Rate = k[A]2[B]. If the concentration of A is doubled and the concentration of B is halved, what happens to the reaction rate?
For a first-order reaction, what fraction of reactant remains after five half-lives have elapsed?
When heated, tetrafluoroethylene dimerizes to form octafluorocyclobutane.To determine the rate of this reaction at 488 K, the data in the table were collected. Analysis was done graphically, as shown
Isomerization of CH3NC occurs slowly when CH3NC is heated.To study the rate of this reaction at 488 K, data on [CH3NC] were collected at various times. Analysis led to the following graph.(a) What is
Formic acid decomposes at 550°C according to the equationThe reaction follows first-order kinetics. In an experiment, it is determined that 75% of a sample of HCO2H has decomposed in 72 seconds.
Data in the table were collected at 540 K for the following reaction: (8)ON + (8)¹00 (8) ON + (8)00
Ammonium cyanate, NH4NCO, rearranges in water to give urea, (NH2)2CO.Using the data in the table:(a) Decide whether the reaction is first-order or second-order.(b) Calculate k for this reaction.(c)
At temperatures below 500 K, the reaction between carbon monoxide and nitrogen dioxidehas the following rate equation: Rate = k[NO2]2. Which of the three mechanisms suggested here best agrees with
Nitryl fluoride can be made by treating nitrogen dioxide with fluorine:Use the rate data in the table to do the following:(a) Write the rate equation for the reaction.(b) Indicate the order of
NOx, a mixture of NO and NO2, plays an essential role in the production of pollutants found in photochemical smog. The NOx in the atmosphere is slowly broken down to N2 and O2 in a first-order
The decomposition of dinitrogen pentaoxidehas the following rate equation: Rate = k[N2O5]. It has been found experimentally that the decomposition is 20.5% complete in 13.0 hours at 298 K. Calculate
The data in the table give the temperature dependence of the rate constant for the reaction N2O5(g) → 2 NO2(g) + 1⁄2 O2(g). Plot these data in the appropriate way to derive the activation energy
The decomposition of gaseous dimethyl ether at ordinary pressures is first-order. Its half-life is 25.0 minutes at 500°C:(a) Starting with 8.00 g of dimethyl ether, what mass remains (in grams)
The decomposition of phosphine, PH3, proceeds according to the equationIt is found that the reaction has the following rate equation: Rate = k[PH3]. The half-life of PH3 is 37.9 seconds at 120°C.(a)
The thermal decomposition of diacetylene, C4H2, was studied at 950°C. Use the following data to determine the order of the reaction. Time Concentration of
The ozone in the Earth’s ozone layer decomposes according to the equation 2 O3(g) → 3 O2(g)The mechanism of the reaction is thought to proceed through an initial fast equilibrium and a slow
Kinetic experiments were conducted to determine the value of the rate constant, k, for the thermal decomposition of diacetylene, C4H2, at temperatures below 1100 K . Calculate Ea for this reaction
Hundreds of different reactions occur in the stratosphere, among them reactions that destroy the Earth’s ozone layer. The table below lists several (second order) reactions of Cl atoms with ozone
Data for the reactionare given in the table. Calculate Ea from a plot of ln k versus 1/T. [Mn(CO) 5 (CH3CN)]+ + NC5H5 [Mn(CO)5(NC5H5)]+ + CH³CN
A reaction that occurs in our atmosphere is the oxidation of NO to the brown gas NO2.The mechanism of the reaction is thought to beStep 1:Step 2:Which is the rate determining step? Is there an
The gas-phase reactionhas an activation energy of 103 kJ/mol, and the rate constant is 0.0900 min−1 at 328.0 K. Find the rate constant at 318.0 K. (8)³0 + (8) ON ←(8) ³0²7
The decomposition of SO2Cl2 to SO2 and Cl2 is first-order in SO2Cl2.Rate = k[SO2Cl2] where k = 0.17/hr(a) What is the rate of decomposition when [SO2Cl2] =0.010 M?(b) What is the half-life of the
Hydrogen peroxide, H2O2(aq), decomposes to H2O(ℓ) and O2(g)At a particular temperature, the following data were collected for the initial rate of appearance O2.(a) What is the rate law for this
The decomposition of nitrogen dioxide at a high temperatureis second-order in this reactant.(a) Determine the rate constant for this reaction if it takes 1.76 min for the concentration of NO2 to
The compound 1,3-butadiene (C4H6) forms 1,5-cyclooctadiene, C8H12 at higher temperatures C4H6(g) → 1⁄2 C8H12(g). Use the following data to determine the order of the reaction and the rate
Egg protein albumin is precipitated when an egg is cooked in boiling (100°C) water. Ea for this first-order reaction is 52.0 kJ/mol. Estimate the time to prepare a 3-minute egg at an altitude at
Hypofluorous acid, HOF, is very unstable, decomposing in a first-order reaction to give HF and O2, with a half-life of 30. minutes at room temperature:HOF(g) → HF(g) + 1⁄2 O2(g)If the partial
We know that the decomposition of SO2Cl2 is first-order in SO2Cl2, SO2Cl2(g) → SO2(g) + Cl2(g) with a half-life of 245 minutes at 600 K. If you begin with a partial pressure of SO2Cl2 of 25 mm Hg
Lanthanum oxalate decomposes when heated to lanthanum(III) oxide, CO, and CO2.(a) If, at equilibrium, the total pressure in a 10.0-L flask is 0.200 atm, what is the value of Kp?(b) Suppose 0.100 mol
Nitrosyl bromide, NOBr, dissociates readily at room temperature.Some NOBr is placed in a flask at 25°C and allowed to dissociate. The total pressure at equilibrium is 190 mm Hg and the compound is
A solution of hydrofluoric acid, HF, has a pH of 2.30. Calculate the equilibrium concentrations of HF, F−, and H3O+, and calculate the amount of HF originally dissolved per liter.
Boric acid and glycerin form a complexwith an equilibrium constant of 0.90. If the concentration of boric acid is 0.10 M, how much glycerin should be added, per liter, so that 60.% of the boric acid
Calculate the hydronium ion concentration and pH in a 0.20M solution of ammonium chloride, NH4Cl.
The dissociation of calcium carbonate has an equilibrium constant of Kp = 1.16 at 800°C.(a) What is Kc for the reaction?(b) If you place 22.5 g of CaCO3 in a 9.56-L container at 800°C, what is the
Calculate the hydronium ion concentration and pH for a 0.015 M solution of sodium formate, NaHCO2.
A sample of N2O4 gas with a pressure of 1.00atm is placed in a flask. When equilibrium is achieved, 20.0% of the N2O4 has been converted to NO2 gas.(a) Calculate Kp.(b) If the original pressure of

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