Calculate the absolute and relative uncertainties for the total delivered volume. Trial Volume delivered (ml) 1 5.002 ml 2 4.998 ml 4.996 ml 3 4 5 6 7 4.984 ml 4.981 ml 4.990 ml 4.999 ml
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- What are the uses of Laboratory Apparatus below: 1. Aspirator or Pipette Bulb 2. Evaporating Dish 3. Mortar and Pestle 4. Graduated Pipette 5. Acid Burette 6. Spatula 7. Stirring RodConsider a manometer (a barometer-like device used for measuring pressure) constructed using ethyl alcohol (ρ =0.789 g/mL). What would be the column height if the pressure is 24.5 mm Hg? The density of Hg is 13.56 g/mL) h = ____ cmCalculate the volume of the flask using the mass of water which filled the flask and the density of water at the measured temperature. In addition to the volume of the flask, you will need to add 3.0 mL to account for the volume of the tube that leads to the pressure sensor. Table 1 Density of water Temp. (ºC) 20 21 22 23 24 25 26 27 28 29 30 Density (g/mL) 0.9972 0.9970 0.9968 0.9966 0.9964 0.9962 0.9959 0.9957 0.9955 0.9952 0.9949 Mass of flask and stopper: 95.1868 g Mass of flask and stopper filled with water: 230.244 g Temperature of water: 23 C
- Using the equation for the best linear fit to the data (1128.8x + 0.5934), determine the pressure (in atm) in the syringe, if the gas volume was 9.20 mL. (HINT. 1 atm = 760 torr, 1 atm = 760 mm Hg, 1 atm = 101.325 kPa)Covert 797 mm Hg to atm.Calculate the pressure at the base of a mercury column 400 mm high. The mercury density at room temperature is 13.5951 g / cm3.Express the result in column, atmosphere, psi, pascal, and bar units. Calculate the pressure exerted on the drum skin of a diver located at a depth of 20 feet below sea level. Assume that the seawater density is: 1 gr / cm3. Calculate the molar volume of Cu2Te. Express this volume in mol/liter and mol/cm 3 units. ( rm=7.270 g/cm3) Use the ideal gas law and the van der Waals equation to calculate the pressure of ammonia gas at a temperature. T = 300 K the molar volume is V = 24 liters / mol
- Arterial blood pressure is traditionally measured in mm Hg. And the style pressure of 85 mm Hg it’s considered borderline between normal and high blood pressure convert this pressure to kPa units. ( 1atm =760 mm Hg= 101.33 kPa )The data below was collected using the procedure described in your lab notebook: Mass (before reaction): test tube + HCl(aq) + stir bar + capsule 27.000 g Mass (after reaction): test tube + HCl(aq) + stir bar + capsule 25.000 g Volume of water displaced from the squirt bottle 146 mL Temperature of the CO2(g) 298.5 K Pressure (atm) 1.012 atm Using this data answer each of the questions below. Enter your answer to three significant figures and enter only the numerical value in the answer box. Calculate the mass of CO2(g). Calculate the number of moles of CO2(g). Calculate the density of CO2(g) in g/L. Calculate the molar mass of CO2 assuming a temperature of 298.5 K. Calculate the Gas constant, R, in L*atm/K*mol. Calculate the % error of the value of the Gas constant, R.High-pressure liquid chromatography (HPLC) is a method used in chemistry and biochemistry to purify chemical substances. The pressures used in this procedure range from around 500 kilopascals (500,000 PaPa) to about 60,000 kPakPa (60,000,000 PaPa). It is often convenient to know the pressure in torr. If an HPLC procedure is running at a pressure of 5.50×108 Pa, what is its running pressure in torr? Express the pressure numerically in torr.
- A pipet delivers 10.9 mLmL , 10.1 mLmL , and 10.9 mLmL in consecutive trials. Find the mean volume of the samples.A previous Chem 100 student carried out the experiment you did by reacting 0.036 g of magnesium. The following data was collected in their lab notebook. The water temperature was 19.8°C. The barometer in the lab read 755.5 mm Hg and 31.97 mL of gas was collected The vapor pressure of water at this temperature is 17.32 mm Hg. Calculate the student’s experimental value of R. Report your answer to four places after the decimal.Recorded barometric pressure: 758.9 mmHg Mass of Aluminum used= .021 g Volume of gas in gas burette after placing into leveling tank= 23 mL temperature in levelling tank: 21 oC Room Temperature: 294.45 K Partial pressure of water vapor: 17.5 mmHg 2 Al (s)+ 6HCl (aq)>>>>2 AlCl3 (aq)+ 3 H2 (g) 1. How to calculate the theoretical yield of H2 gas (mL) based on the mass of Aluminum used. 2. How to calculate the % error of H2 gas.