20. mol H2 reacts with 8.0 mol O2 to produce H2O. Determine the number of grams reactant in excess and number of grams H2O produced. Identify the limiting reactant. 8.1 g H2 , 2.9 x 102 g H2O 17. How many litres of O2 gas are required to produce 100. g Al2O3?
A) How many mosm solute will 1 gram of NaCl yield? Show your calculations. (1gNaCl/1)*(1000mg/1gNaCl)(2/58mg)=34.5mOsm. 3. Mixed Solutions: If 1 mmole of glucose (180mg=1mOsm) and 1 mmole of NaCl (58mg=2mmOsm) are put into a beaker and distilled water added to make 1 liter, the osmolarity is 3 mOSm/L.
What is the molar mass of the antibiotic? Show your work. Data Table 2. Temperature Readings for Freezing Point Time (seconds) |Temp (°C) of control (tap water) |Temp (°C) of solution + 0.5 tsp (~2.5 mL) salt |Temp (°C) of solution + 1.0 tsp (~5 mL) salt | 30 |5|5|2| 60 |5|6|2| 90 |5|4|2| 120 |5|3|2| 150 |5|3|2| 180 |5|3|2| 210 |5|3|2| 240 |5|3|2| 270 |5|3|2| 300 |5|3|2| 330 |5|3|2| 360 |5|3|2| 390|5|3|2| 420 |5|3|2| 450 |5|2|2| 480 |5|3|2| 510 |4|3|2| 540 |4|3|2| 570 |4|3|2| 600 |4|3|2| www.HOLscience.com Colligative Properties and Osmotic Pressure Questions | A. Describe the three freezing points.
1. Be sure the data table is viewable. 2. Right-click (PC) or Command-Click (Mac) on the table and select print. Part I: Density of Unknown Liquid | | Trial 1 | Trial 2 | Trial 3 | Mass of Empty 10 mL graduated cylinder (grams) | 25.5g | 25g | 25g | Volume of liquid (milliliters) | 8.6mL | 8.7mL | 8.4mL | Mass of graduated cylinder and liquid (grams) | 36g | 36g | 35.5g | Part II: Density of Irregular-Shaped Solid | Mass of solid (grams) | 38.74g | 39.002g | 42.489g | Volume of water (milliliters) | 50mL | 49mL | 51mL | Volume of water and solid (milliliters) | 54mL | 53mL | 56mL | Part III: Density of Regular-Shaped Solid | Mass of solid (grams) | 26g | 27g | 26g | Length of solid (centimeters) | 5.2cm | 5cm | 4.5cm | Width of solid (centimeters) | 3cm | 4cm | 3.5cm | Height of solid (centimeters) | 2.5cm | 3cm | 2cm | Calculations Show all of your work for each of the following calculations and be careful to follow significant figure rules in each calculation.
(0.050) (0.1) = 0.0083 moles b. Pour 8.3 mL of the stock solution to get the amount needed. c. Measure out 8.3 mL in a graduated cylinder 8. Exercise 8: a. 41.8 mL are used b. 0.00079 moles EDTA4- c. 0.00079 moles ZnI2 d. 0.0517 grams of ZnI2 are in the sample e. 0.0517/0.237= 21.8% f. Error Is 6.34% Lab Report: Part 1: In this lab we used the following supplies: * Zinc Iodide * Na2H2EDTA(s) * Calmagite indicator solution * pH 10 buffer solution * 6M Acetic Acid * Unknown Zinc Compound The main purpose for this part of the lab was to determine the amount of zinc ion in a sample of ZnI2 by titration.
test tube to contain the solution of cyclohexane plus the unknown solute, and an empty graph. The procedure was: 1. Make an ice bath 2. Measure the test tube of pure cyclohexane 3. Measure pure solvent 4.
Add color indicator 4. Obtain a burette and fill it with NaOH 5. Titrate the 10 mL with NaOH until it turns pink 6. Weigh a dry funnel with a filter paper and record the weight 7. Obtain an Erlenmeyer flask that has a vacuum opening and attach the vacuum tube to it 8.
5. Record the data in a chart with the times. Experiment Basically the experiment is on what household items can insulate and hold the circulation of cold air inside the ice box which allows freezing points or melting points to take course. Data/ Graphs Ice Boxes | Test 1(none) | Test 2 (salt) | Test 3(Sugar) | Cardboard | 7:14.8 | 12:52.7 | 8:35.2 | Paper | 9:28.4 | 12:14.8 | 7:43.6 | Aluminum Foil | 16:35.1 | 17:21.6 | 13:17.8 | Time Graph Observations When I experimented I noticed that one of the ice boxes melted quickly than the others, which could mean that those ice boxes vents heat. The substance added to the ice box could have either helped it stay cool or melted it quicker.
from the penny. * Dry the penny and retest x4 * Determine the number of drops of Chocolate milk it takes to fill a penny, holding the eye dropped 2 cm. from the penny. * Dry the penny and retest x4. * Calculate data.
29.4 atm B. 4.89 atm C. 25.1 atm D. 36.0 atm _____ 5. The vapor pressure of pure ethanol at 60 °C is 349 mm Hg. Calculate the vapor pressure at 60 °C of a solution prepared by dissolving 10.0 mol of naphthalene (nonvolatile) in 90.0 mol of ethanol. A.