(a)
Interpretation:
The average rate of consumption of hydrogen is to be determined.
Concept Introduction:
The average rate of the reaction is referred to the change in the molar concentration in the distinct interval of time. Mathematically the ratio of change in molar concentration of a reactant or a product to the change in the time interval gives the average
The average rate of consumption or the disappearance of reactant is negative. Mathematical expression is shown below.
The average rate of formation or the appearance of reactant is positive. Mathematical expression is shown below.
(b)
Interpretation:
The unique rate of reaction is to be determined.
Concept Introduction:
The unique rate of reaction is regardless of the reactant and products. It does depend upon the coefficient of the species in the balanced
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CHEM PRINCIPLES LL W/ACHIEVE ONE-SEM
- Amoxicillin is an antibiotic packaged as a powder. When it is used to treat babies and small animals, the pharmacist or veterinarian must suspend it in water, so that it can be administered orally with a medicine dropper. The label says to dispose of unused suspension after 14 days. It also points out that refrigeration is required. In the context of this chapter, what is implied in the latter two statements?arrow_forwardSilicon 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.arrow_forwardDefine stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.arrow_forward
- 7-43 (Chemical Connections 7A and 7B) Why is a high fever dangerous? Why is a low body temperature dangerous?arrow_forwardThe following equation represents a reversible decomposition: CaCO3(s)CaO(s)+CO2(g) Under what conditions will decomposition in a closed container proceed to completion so that no CaCO3 remains?arrow_forwardExplain how a species might be part of a rate law but not part of a balanced chemical reaction.arrow_forward
- . Account for the increase in reaction rate brought about by a catalyst.arrow_forwardThe label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?arrow_forwardDistinguish between the differential rate law and the integrated rate law. Which of these is often called just the rate law? What is k in a rate law, and what are orders in a rate law? Explain.arrow_forward
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