Chemistry 114 First Hour Exam Name:____________ (4 points) Please show all work for partial credit All problems are worth 12 points 1. Define the following terms: Surface tension The energy needed to expand the surface of a liquid Cohesive forces The forces within a liquid or solid that tend to hold it together. Normal melting or freezing point The temperature at which the vapor pressure of a solid and a liquid are in equilibrium, and the over pressure is 1 atm. Delocalized covalent bond Also a metallic covalent bond. The type of bond found in metals where the electron that holds the metal together is not constrained to a particular place, so the electrons holding the metal together are free to move anywhere in the metal lattice. Critical Pressure - The pressure required to compress a gas into a liquid when the liquid is at its critical temperature. Second order reaction A reaction where the order parameter is 2. 2. When I shine an X-ray with a wavelength of 1.54Å at a crystal, I get a reflection from the crystal at 15.2o. What is the distance between atom layers in this crystal. (Assume that n=1) 1 3. Below are 4 pairs of solids. melting point and why. For each pair circle the compound with the HIGHER MgO and CO Why? CCl4 and CH3Cl Why? Ionic compound Charge-Charge forces found in Ionic compound are very strong CH3Cl is polar which gives it a stronger interactive force than the non-polar CCl4 CCl4 and CBr4 Why? CH3NH2 and NH2CH2NH2 Why? Both compounds are nonpolar and held together by London forces But London forces are proportional To the number of electrons so CBr4 has more electrons and a stronger London force The NH2 in both compounds has a potential to make strong hydrogen bonds, but NH2CH2NH2 has 2 NH2's so it can make twice as many hydrogen bonds 4. I am going to make a solution by mixing 20 grams of NaOH with 80 grams of water A. What is the weight or mass % of NaOH in this solution? B. What is the mole fraction of NaOH in this solution C. Assuming the solution has a volume of 95 mls, what is the molarity of NaOH in the solution? D. What is the colligative molality of the solution? 2 5. I am going to make a solution with 25 grams of methanol (CH3OH) and 50 grams of ethanol (CH3CH2OH). What is the mole fraction of each liquid in this solution? If the vapor pressure of methanol is 260 torr @ 40o C, and ethanol has a vapor pressure of 150 torr at 40oC, what is the vapor pressure of this solution at 40oC? What is the mole fraction of methanol in this vapor? If the actual vapor pressure of the solution was HIGHER than your answer in part B, would that be a positive or negative deviation from Raoult’s law, and what would that indicate about the interactions between methanol and ethanol in solution? When the vapor pressure is higher than predicted by Raoult’s law this is called a positive deviation and it is associated with poor solvent-solute interactions. 6.You may have heard of the ‘Bends’ a painful, potentially fatal problem that occurs when divers ascend too fast. It is caused by air bubbles forming in the bloodstream as a diver comes up from the bottom and nitrogen dissolved in their blood forms bubbles in the bloodstream. A. If the Henry’s Law constant for N2 is 1500 atm/M, and we assume that at sea level the pressure of N2 is 0.8 atm, what is the molar concentration of N2 in your blood. B. If you dive to 66 feet, where the pressure on your body is 3 atm, what is the molar concentration of N2 in your blood now? C. If an average body contains 5.5 liters of blood, use the difference between your answers for A and B to determine the volume of bubbles in your blood that could form as a diver rises from 66 feet to the surface (Assume the temperature is 25oC) . The Ä molarity = .002-.00053 or .00147M .00147 moles/Liter X 5.5 liters = .0081 moles of N2 must escape from the blood using good ol’ PV=nRT V=nRT/P V = (.0081 molesA.08206 lAAtm/KAmol A298K)/1atm =.198L or ~200 mLs of gas that needs to escape from the blood 3 7. I am investigating the reaction A + B 6C. obtained the data shown in the table below: [A](M) [B] (M) 0.7 1 1 Using the method of initial rates I have rate M/min 0.7 0.7 1.4 1.19 1.70 3.89 What are the order parameters for A and B in this reaction, and what is the rate constant for this reaction? 8. I have a first order reaction with a rate constant of .2 min-1. If the initial concentration of my reactant, Z is 1.5 M, how long will it take for the concentration of Z to reach .75M? Two ways to do this. 1. If you notice that the second concentration is ½ of this first, you can do this with the half-life for a first order reaction t1/2 = .693/k = .693/.2 min-1 = 3.465 minutes 2. If you don’t see that this is a half-life problem, then you must use the equation ln[A]t = ln[A]0 -kt ln(.75)=ln(1.5)-.2X -.288=.405 -.2X -.693=-.2X .693=.2X X=.693/.2 =3.465 min 4