Which of the following statements is/are true about an exothermic reaction? Choose all the apply The potential energy of the reactants is less than the potential energy of the products The thermal kinetic energy of the surroundings will increase The energy absorbed in bond breaking is more than the energy released in bond formation The system absorbs energy

Which of the following statements is/are true about an exothermic reaction? Choose all the apply The potential energy of the reactants is less than the potential energy of the products The thermal kinetic energy of the surroundings will increase The energy absorbed in bond breaking is more than the energy released in bond formation The system absorbs energy

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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For an exothermic reaction, how is the measured temperature change affected if some of the heat produced transfers to the calorimeter? How will the determination of the specific heat of the metal be affected if the thermometer used to record the temperature of the water bath reads too low?
The energy of an exothermic reaction is released into the environment O consumed in the reaction converted to another form absorbed by the reaction
On an endothermic potential energy diagram, what is true for all products? The products are at the same energy level as the reactants. The products are at a lower energy level than the reactants. The products are at a higher energy level than the reactants. The products do not have energy.
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The Law of Conservation of Energy states, when applied to Calorimetry, states that heat is neither lost nor generated, but merely changes form during processes. Which of these calorimetry equations corresponds to that law?
The amount pf heat required to raise the temperature of a given amount of substance b by 1 degree Celsius.
One proposed source of clean energy is the combustion of hydrogen in the presence of oxygen. This reaction releases a significant amount of energy, and the only product of the reaction is water. The balanced chemical equation is shown here: 2H₂(g) + O₂(g) →→→ 2H₂O(g) + energy
The energy released by a reaction is 657 kJ/mol. Is this reaction endothermic or exothermic? Please explain why
A 2.50 g sample of solid NaOH is dissolved in 100.0 ml of water in a calorimeter. The heat of solution was -57 kJ/mol. Calculate the final temperature of the solution if the initial temperature was 16 OC. Atomic mass for Na is 23.0 g/mol, for O is 16.0 g/mol and for H is 1.0 g/mol. (Specific heat of the solution is 4.184 J/g.0C, and density is 1.00g/ml) *
In order to break water into hydrogen and oxygen, water is heated to more than 500°C. Which kind of reaction is this and why? It is exothermic because heat needs to be released by the reactants to form the products. It is endothermic because heat needs to be released by the reactants to form the products It is exothermic because heat needs to be absorbed by the reactants to form the products. It is endothermic because heat needs to be absorbed by the reactants to form the products.
During an exothermic reaction, H for the reactants was 890 kJ/mol. Which of the following statements is correct about the H for the products and the comparison of the energy in bonds? A)It is less than 890 kJ/mol, and the amount of energy required to break bonds is greater than the amount of energy released in forming bonds. B) It is less than 890 kJ/mol, and the amount of energy required to break bonds is less than the amount of energy released in forming bonds. C) It is greater than 890 kJ/mol, and the amount of energy required to break bonds is greater than the amount of energy released in forming bonds D) It is greater than 890 kJ/mol, and the amount of energy required to break bonds is less than the amount of energy released in forming bonds.
The enthalpy change for a chemical reaction is the sum of the energy consumed in breaking bonds and the energy released during bond formation. One way to determine the overall energy change for a chemical reaction is to apply Hess’s law to add together a group of reactions which can be arranged such that the chemical equations, when combined, give the overall equation we are trying to characterize. a. Write a balanced chemical equation for the combustion of gaseous propane in gaseous oxygen to produce gaseous carbon dioxide and liquid water. C3H8(g)+ O2(g) ---->CO2(g)+ H2O(g) b. Combine the following equations to determine the enthalpy change for the combustion of 1 mole of propane. Assume that solid carbon is graphite. 3C(s,graphite)+4H2(g)--->C3H8(g) ΔHo = -103.8 kJ/mol C(s,graphite)+O2(g)--->CO2(g) ΔHo= -393.5 kJ/mol H2(g)+1/2 O2(g)--->H2O(g) ΔHo= -285.8 kJ/mol kJ/mol…