Appendix B lists the vapor pressure of water at various external pressures.
(a) Plot the data in Appendix B, vapor pressure (torr) versus temperature \(\left({ }^{\circ} \mathrm{C}\right)\). From your plot, estimate the vapor pressure of water at body temperature, \(37^{\circ} \mathrm{C}\).
(b) Explain the significance of the data point at 760.0 torr, \(100^{\circ} \mathrm{C}\).
(c) A city at an altitude of 5000 ft above sea level has a barometric pressure of 633 torr. To what temperature would you have to heat water to boil it in this city?
(d) A city at an altitude of 500 ft below sea level would have a barometric pressure of 774 torr. To what temperature would you have to heat water to boil it in this city?
Text Transcription:
(^{\circ} C)
37^{\circ} C
100^{\circ} C
Step 1 of 5) In contrast, Br2 is an intermediate because it is first formed (Equation 14.32) and then consumed (Equation 14.33). The color change we see in Figure 14.22 illustrates that the presence of intermediates can in some cases be readily detected. Neither the catalyst nor the intermediate appears in the equation for the overall reaction. Notice, however, that the catalyst is present at the start of the reaction, whereas the intermediate is formed during the course of the reaction. How does a catalyst work If we think about the general form of rate laws 1 Equation 14.7, rate, we conclude that the catalyst must affect the numerical value of k, the rate constant. On the basis of the Arrhenius equation (Equation, k is determined by the activation energy 1Ea2 and the frequency factor 1A2. A catalyst may affect the rate of reaction by altering the value of either Ea or A. We can envision this happening in two ways: The catalyst could provide a new mechanism for the reaction that has an Ea value lower than the Ea value for the uncatalyzed reaction, or the catalyst could assist in the orientation of reactants and so increase A. The most dramatic catalytic effects come from lowering Ea. As a general rule, a catalyst lowers the overall activation energy for a chemical reaction.
