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At 40 degrees celsius the vapor pressure of methyl alcohol is 254 mmHg and at the same temperature the vapor pressure of ethyl alcohol is 135 mmHg.
Given the following substitution reaction, what would the effect be of changing the solvent from CH3OH to (CH3)2S=O? CH3(CH2)5Br + NaOH as it goes to CH3(CH2)5OH + Br-
Categorize each of the following as either ionic, covalent, or metallic bonding. 1. Molecular formula= 2. electron sharing= 3. alloy= 4. nonmetal with nonmetal
A variety of different products could be formed in this reaction; for this problem assume all unique products are formed that only 1 Br is present in each alkyl halide product. how many of the poten
(NH4)2Cr2O7(s) ? N2(g) + 4 H2O(g) + Cr2O3(s) If 0.95 g of ammonium dichromate is used and the gases from this reaction are trapped in a 15.0 L flask at 23 °C, what is the total pressure of the g
1. the halide ion from HBr will act as the nucleophile in the first step of the reaction 2. the halide ion will act as the nucleophile in the second step of the reaction
carbon dioxide was allowed to effuse through a small opening under constant pressure conditions. It required 683 s for 1.00 L of this gas to effuse. Calculate the effusion time of ozone (O3) under i
What amount of HCl gas must be added to 1 L of a buffer solution that contains [acetic acid]= 2.0 M and [acetate]= 1.0M in order to produce a solution with a pH of 4.26
Given the following value, tell whether the starting material or product is favored at equilibrium. Keq=0.2 Is this a starting material favored or a product favored
Calculate the rms (average) speed of NF3 atoms or molecules at 202 oC. Use R = 8.314 kg-m2/K-s2-mol for the value of the gas constant.
If you have a 25 mL solution that contains 47 ug/dL of iron, how many grams of iron must be removed to reach a concentration of 23 ug/dL? How many moles of iron is this
Given the following value, tell whether the starting material or product is favored at equilibrium. delta H=6.5 kcal/mol. Is this a starting material favored, or product favored
A mixture of gases contains 5.18 g of CO, 3.65 g of NH3, and 5.01 g of O2. If the total pressure of the mixture is 2.65 atm, what is the partial pressure of each component
What would be the concentrations of acetic acid and sodium acetate in this solution. Would we expect this solution to be a buffer
Arrange the following elements from greatest to least tendency to accept an electron. Rank from greatest to least tendency to accept an electron. To rank items as equivalent, overlap them.
Do the pH values for the more dilute solutions approach the pH of the distilled water. What would we expect to happen if we continued to dilute these samples even further
Compare the pH values in the dilution experiment for the strong acid(HCl) and the weak acid (acetic acid). HCl : 10^-2 : 3.03 10^-3 :4.48 10^-4:5.95 10^-5:6.55 10^-6:6.60 10^-7:6.70
Compare the pH values in the dilution experiment for each of the acids and bases used to the pH detemined for distilled water.
Calculate the number of grams of NaOH per 100ml to give a pH8.0 solution if pure water at pH7.0 is used in the experiment. Repeat this calculation for a pH6.0 solution using HCl.
If the actual pressure of the vapour was less than the surrounding , will molecular weight you determine (heptane) be too low or too high
If .43 g of aluminum foil was dissolved in sufficient 3M KOH solution, and the solution was acidified with 4M H2SO4, what was the theoretical yield of KAl(SO4)2 * 12H2O? If only 5.87g of alum were o
Which of the following expressions hold for 0.10 mol/L Na2HA(aq). (HA2- is the doubly-ionized form of H3A, a weak triprotic acid.)
if .43g of aluminum foil was dissolved in sufficient 3M KOH solution, and the solution was acidified with 4M H2SO4, what was the theoretical yield of KAl(SO4)2 * 12H2O
1)Acetic acid, CH3COOH, is a weak monoprotic acid (pKa=4.74 at 25oC). What is the pH of 0.191 mol/L CH3COOH(aq) at 25oC? Give your answer accurate to two decimal places. 2)Diethylamine, (C2H5)2NH, i
Given the following equilibrium constants at 427 °C: Na2O(s) <=> 2Na(l) + 1/2 O2(g) Kc = 2 x 10-25 NaO(g) <=> Na(l) + 1/2 O2(g) Kc = 2 x 10-5 Na2O2(s) <=> 2Na(l) + O2(g) Kc = 5