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) | 2.56g | 2.55g | 2.60g | Volume of liquid (milliliters) | 8.50mL | 8.80mL | 8.90mL | Mass of graduated cylinder and liquid (grams) | 36.10g/mL | 36.60g/mL | 36.90g/mL | Part II: Density of Irregular-Shaped Solid | Mass of solid (grams) | 41.000g | 38.890g | 42.960g | Volume of water (milliliters) | 50mL | 55.5mL | 53.1mL | Volume of water and solid (milliliters) | 54.9g/mL | 60g/mL | 58.1g/mL | Part III: Density of Regular-Shaped Solid | Mass of solid (grams) | 28.00g | 27.70g | 28.10g | Length of solid (centimeters) | 5.20cm | 5.00cm | 4.50cm | Width of solid (centimeters) | 3.00cm | 4.00cm | 3.50cm | Height of solid (centimeters) | 2.50cm | 3.00cm | 2.00cm | Calculations Show all of your work for each of the following calculations and be careful to follow significant figure rules in each calculation.
There will have some error. 2) A volatile liquid was allowed to evaporate in a 43.298 g flask that has a total volume of 252 ml. the temperature of the water bath was 100˚C at the atmospheric pressure of 776 torr. The mass of the flask and condensed vapor was 44.173 g. calculate the molar mass of the liquid. T = 273 + 100 = 373 V = 252 mL = 1 L / 1000 mL = 0.252 L P = 776 Torr R= 0.0821 mass of 44.173 - 43.298 g = 0.875g moles of gas = PV / RT = 776 x .252 / 62.363 x (273+100) =0.00841 moles molar mass = 0.875g / 0.00841 moles = 104.1 g/
Part D: Density of Methanol 1) Find the mass of an empty 10 mL graduated cylinder, and then fill approximately 9 mL of methanol and record volume. 2) Find the mass of the cylinder and methanol, subtracting the initial mass from the new mass to determine the mass of methanol. 3) Determine the density and percent error. Data: Part A: Density of a Rectangular Solid/Cube Block # 9 (cube – brass) 1. Mass – 132.32g 2.
| Object | Estimated Mass (g) | Actual Mass (g) | Actual Mass (kg) | Pen or pencil | 5 | 5.4 | .0054 | 3 Pennies | 6 | 7.6 | .0076 | 1 Quarter | 5 | 5.7 | .0057 | 2 Quarters, 3 Dimes | 15 | 18.2 | .0182 | 4 Dimes, 5 Pennies | 15 | 21.6 | .0216 | 3 Quarters, 1 Dime, 5 Pennies | 25 | 31.9 | .0319 | Key | 10 | 9.2 | .0092 | Key, 1 Quarter, 4 Pennies | 20 | 24.9 | .0249 | Data Table 4: Liquid measurements. | | | Mass A | Mass B | Mass B - A | | | Liquid | Volume(mL) | GraduatedCylinder (g) |
0.00512g ZnI2/mL of solution 0.00512g/319.18 g/mol=1.6*10-5 mol 1.6*10-5 mol/(1*10-3L)=0.016M c. 0.00806 moles of ZnI2/500 mL of solution 0.00806mol/(500*10-3)L=0.016M d. 0.0161 moles of ZnI2/L of solution 0.0161mol/1L=0.016M Exercise 4: a. The moles of ZnI2: 0.25M*(250*10-3)L=0.0625mol b. 0.25M*(250*10-3)L=0.0625mol The mass of ZnI2: 0.0625mol*319.18 g/mol=19.95g c. 0.25M*(500*10-3)L=0.125mol 0.125mol*319.18 g/mol=39.9g ZnI2 d. 0.0125mol/0.25M=0.05L Exercise 5: a. 0.125M*(100*10-3)L=0.0125mol b. 0.0625mol/0.125M=0.5L=500mL Calculation for preparing the EDTA solution Exercise 6 a.
What is the final pressure in the drum if the final temperature is 60oC? A. 0.055 MPa B. 2.0 MPa C. 10 MPa D. 55 MPa Problems 35 and 36 are based on the following statement. Ten kilograms of oxygen and 2 kg of hydrogen are mixed in a 1 m3 vessel.
1. 25 cm3 of a solution of 0.1 moldm-3 NaOH reacts with 50 cm3 of a solution of hydrochloric acid. What is the molarity of the acid? 2. 25.0 cm3 of a 0.10 moldm-3 solution of sodium hydroxide was titrated against a solution of hydrochloric acid of unknown concentration.
Procedure: Refer to Chemistry Lab Manual pp. 33-35, 37. Results: The density of the yeast-sugar solution on day 1 was 1.05g/mL. On day 2, the density of the solution had dropped down to 1.00g/mL. We found the mass of our pure alcohol to be 10.23g.
Experimental Data Trial 1 Trial 2 Trial 3 Sample Volume 10 mL 10 mL 10 mL Weight sample + capped vial 26.5g 26.5g 26.3g Weight vial + cap 15.5g 15.4g 15.4g Sample weight 11.0g 11.1g 10.9g Calculated Results Trial 1 Trial 2 Trial 3 Density of samples: 1.10g/mL 1.11g/mL 1.09g/mL Average density: 1.10g/mL 1.10g/mL 1.10g/mL Deviation from Average: ±0.00g/mL ±0.01g/mL -0.01g/mL Average Deviation: add absolute values of deviations from average and divide by the number of trials. +0.00++0.01+-0.01= 0.02 ∴ Therefore, the average deviation in density = ±0.02/3 = ±0.01 Average weight of 10mL Volume Samples 10mL x 1.1g/mL = 11g Percent Inherent Error in Average Weight of Samples ±0.1 g/reading*2 readings 11* 100 = 1.8~2% Percent Inherent Error in Average Volume of Samples ±0.1 mL/reading*1 readings 10 mL*100 = 1% Total Percent Inherent Error in Density ±2%+ ±1%= ±3% Inherent Error in Density 1.10g/mL x (±3/100) = ±0.03g/mL Conclusions Since the deviations from the average density are equal to or less than the total possible inherent error computed, it is concluded that the precision of the data collected was good. Second
- 0.5 M: Add 6.25 mL of the 2M HCl and mix with distilled water until the entire solution is measured to be about 25 mL Length and Mass of Magnesium Ribbon: • Original length: 30 cm • Original mass: 0.35 g • Length of ribbon used for experiment: 1.5 cm • Mass of ribbon used for experiment: 0.0175 g Concentration and Time data: 2.0 M 1.5 M 1.0 M 0.75 M 0.5 M Time (s) #1 13 s 18 s 38 s 81 s 225 s Time (s) #2 11 s 17 s 39 s 87 s 418 s Concentration and Temperature data: 2.0 M 1.5 M 1.0 M 0.75 M 0.5 M Temperature (Celsius) #1 30.1 30.1 30.2 30.5 28.5 Temperature (Celsius) #2 30.8 30.4 30.5 30.3 29.1 Results Table: Rate of Reaction for each concentration: 2.0 M 1.5 M 1.0 M 0.75 M 0.5 M Rate of Reaction 0.00145 0.001 0.000454 0.000208 0.0000755 Plot of Concentration vs Rate of