Question 14The net reactionNO₂(g) + CO(g) → NO(g) + CO₂(g)Proceeds by the following mechanismStep 1.2 NO₂(g)NO3(g) + NO(g)Step 2. NO3(g) + CO(g) → NO2(g) + CO₂(g)The rate law for the net reaction is k[NO₂]².Identify the rate determining step and the reaction intermediate.→>>O Not possible to determine given the data.Step 2, NO3Step 2, NO2Step 1, NO₂Step 1, NO33.4 pts Question 15How does the presence of a catalyst affect the enthalpy change of a reaction?3.4 pO It depends on if the reaction is exothermic or endothermicA catalyst does not affect the enthalpy change of a reactionA catalyst increases the enthalpy change of a reactionO A catalyst increase the enthalpy change for the forward reaction but reduces it for the reverse reactionO A catalyst decreases the enthalpy change of a reaction

14) The rate law for a chemical reaction is an expression that provides a relationship between the…

Question 14 The net reaction NO₂(g) + CO(g) → NO(g) + CO₂(g) Proceeds by the following mechanism Step 1. 2 NO₂(g) NO3(g) + NO(g) Step 2. NO3(g) + CO(g) → NO2(g) + CO₂(g) The rate law for the net reaction is k[NO₂]². Identify the rate determining step and the reaction intermediate. →>> O Not possible to determine given the data. Step 2, NO3 Step 2, NO₂ Step 1, NO₂ Step 1, NO3 3.4 p

Question 14 The net reaction NO₂(g) + CO(g) → NO(g) + CO₂(g) Proceeds by the following mechanism Step 1. 2 NO₂(g) NO3(g) + NO(g) Step 2. NO3(g) + CO(g) → NO2(g) + CO₂(g) The rate law for the net reaction is k[NO₂]². Identify the rate determining step and the reaction intermediate. →>> O Not possible to determine given the data. Step 2, NO3 Step 2, NO₂ Step 1, NO₂ Step 1, NO3 3.4 p

Chemistry

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ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 2RQ: Consider the following potential energy diagrams for two different reactions. Which plot represents...

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Correlate the fuel values and caloric values calculated in Problem-Solving Example 4.15 with the relative number of oxygen atoms per molecule. Provide a nanoscale explanation for any correlation you find.
Nitrogen oxide (NO) has been found to be a key component in many biological processes. It also can react with oxygen to give the brown gas NO2. When one mole of NO reacts with oxygen, 57.0 kJ of heat are evolved. (a) Write the thermochemical equation for the reaction between one mole of nitrogen oxide and oxygen. (b) Is the reaction exothermic or endothermic? (c) Draw an energy diagram showing the path of this reaction. (Figure 8.6 is an example of such an energy diagram.) (d) What is H when 5.00 g of nitrogen oxide react? (e) How many grams of nitrogen oxide must react with an excess of oxygen to liberate ten kilojoules of heat?
Explain how the heat measured in Example 5.5 differs from the enthalpy change for the exothermic reaction described by the following equation: HCl(aq)+NaCl(aq)H2O(l)
Small amounts of oxygen gas can be prepared in the laboratory by decomposing potassium chlorate with heat. A by-product of the decomposition is potassium chloride. When one mole of potassium chlorate decomposes, 44.7 kJ are evolved. (a) Write a balanced thermochemical equation for the decomposition of one mole of potassium chlorate. (b) Is the reaction exothermic? (c) Draw an energy diagram showing the path of this reaction. (Figure 8.6 is an example of such an energy diagram.) (d) What is H when 3.00 g of potassium chlorate decompose? (e) How many grams of potassium chlorate need to be decomposed to liberate fifteen kilojoules of heat?
Consider the following potential energy diagrams for two different reactions. Which plot represents an exothermic reaction? In plot a, do the reactants on average have stronger or weaker bonds than the products? In plot b, reactants must gain potential energy to convert to products. How does this occur?
Hypothetical elements A2 and B2 react according to the following equation, forming the compound AB. A2(aq)+B2(aq)2AB(aq);H=+271kJ/mol If solutions A2(aq) and B2(aq), starting at the same temperature, are mixed in a coffee-cup calorimeter, the reaction that occurs is a exothermic, and the temperature of the resulting solution rises. b endothermic, and the temperature of the resulting solution rises. c endothermic, and the temperature of the resulting solution falls. d exothermic, and the temperature of the resulting solution falls. e exothermic or endothermic, depending on the original and final temperatures.
Quinone is an important type of molecule that is involved in photosynthesis. The transport of electrons mediated by quinone in certain enzymes allows plants to take water, carbondioxide, and the energy of sunlight to create glucose. A 0.1964-g sample of quinone (C6H4O2) is burned in a bomb calorimeter with a heat capacity of 1.56 kJ/C. The temperature of the calorimeter increases by 3.2C. Calculate the energy of combustion of quinone per gram and per mole.
When one mole of calcium carbonate reacts with ammonia, solid calcium cyanamide, CaCN2, and liquid water are formed. The reaction absorbs 90.1 kJ of heat. (a) Write a balanced thermochemical equation for the reaction. (b) Using Table 8.3, calculate Hf for calcium cyanamide.
Explain how calorimetry works to calculate H or E for a reaction. Does the temperature of the calorimeter increase or decrease for an endothermic reaction? For an exothermic reaction? Explain.
The equation for the combustion of 2 mol of butane can be written 2C4H10(g)+O2(g)8CO2(g)+10H2O(g);HO Which of the following produces the least heat? a Burning 1 mol of butane. b Reacting 1 mol of oxygen with excess butane. c Burning enough butane to produce 1 mol of carbon dioxide. d Burning enough butane to produce 1 mol of water. e All of the above reactions (a, b, c, and d) produce the same amount of heat.
Question 13 The enthalpy of combustion of methane gas, CH4(g), is about -9.0*102kJ/mol. When methanegas reacts with O2(g), the products are carbon dioxide CO2(g) and water H2O(l). How much heatis released during the combustion of methane gas when 2.0 mols of O2(g) are consumed. Expressyour answer in kJ. A. 3.0*102kJ B. 6.0*102kJ C. 9.0*102kJ D. 12*102kJ E. 18*102kJ
2 (a) In this investigation, you will use a polystyrene-cup calorimter to determine the amount of heat released during acid-base neutralization reactions. Find information in your textbook, an encyclopedia, or a web site about calorimetry. Sketch the apparatus for a polystrene-cup calorimeter. (b) For more precise heat of reaction measurnments, chemists use a device called bomb calorimeter. How is a bomb calorimeter similar to and different from a polystyrene-cup calorimeter?

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