3.A core sample is saturated with an oil (po = 35°API), gas and water. The initial weight of the sample is 224.14 g. After the gas is displaced by water (pw = 1 g/cm³), the weight is increased to 225.90 g. The sample is the placed in a Soxhlet distillation apparatus, and 4.4 cm' water is extracted. After drying the core sample, the weight is now 209.75 g. The sample bulk volume, 95 cm3 is measured in a mercury pycnometer. Find the porosity, water saturation, oil saturation, gas saturation and lithology of the core sample.

3.A core sample is saturated with an oil (po = 35°API), gas and water. The initial weight of the sample is 224.14 g. After the gas is displaced by water (pw = 1 g/cm³), the weight is increased to 225.90 g. The sample is the placed in a Soxhlet distillation apparatus, and 4.4 cm' water is extracted. After drying the core sample, the weight is now 209.75 g. The sample bulk volume, 95 cm3 is measured in a mercury pycnometer. Find the porosity, water saturation, oil saturation, gas saturation and lithology of the core sample.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter31: Introduction To Analytical Separations

Section: Chapter Questions

Problem 31.19QAP

See similar textbooks

Similar questions

A pipet is used to transfer 3.00 mL of a 2.00 M stock solution in flask “S” to a 25.00-mL volumetric flask “A,” which is then diluted with DI H2O to the calibration mark. The solution is thoroughly mixed. Next, 3.00 mL of the solution in volumetric flask “A” is transferred by pipet to a 50.00-mL volumetric flask “B” and then diluted with DI H2O to the calibration mark. Calculate the molarity of the solution in volumetric flask “B.”
What is the molarity of a concentrated solution of sulfuric acid with a specific gravity of 1.84 and 95.0% by weight sulfuric acid? specific gravity = density of substance at certain temp/density of water at 4 degrees C the density of water is 0.999973 g/mL at 4 degrees celsius. Describe how to prepare 3.0 L of 0.100M. I will pipet ______ and add this to 200mL water. The solution will be stirred and diluted to 3L with water.
Prepare 1500mL of 0.5N H2SO4 solution with specific gravity of 1.84g/mL and assay of 97%
A pipet is used to transfer 6.00 mLmL of a 3.75 MM stock solution in flask “S” to a 25.00-mL volumetric flask “A,” which is then diluted with DI H2OH2O to the calibration mark. The solution is thoroughly mixed. Next, 10.00 mLmL of the solution in volumetric flask “A” is transferred by pipet to a 50.00-mL volumetric flask “B” and then diluted with DI H2OH2O to the calibration mark. Calculate the molarity of the solution in volumetric flask “B.”
A core sample is saturated with an oil (?o = 35oAPI), gas and water. The initial weight of the sample is 224.14 g. After the gas is displaced by water (?w = 1 g/cm3 ), the weight is increased to 225.90 g. The sample is the placed in a Soxhlet distillation apparatus, and 4.4 cm3 water is extracted. After drying the core sample, the weight is now 209.75 g. The sample bulk volume, 95 cm3 is measured in a mercury pycnometer. Find the porosity, water saturation, oil saturation, gas saturation and lithology of the core sample.
A spent 1.0 percent caustic soda solution (ρNaOH = 8.42 lb/gal) with a volumetric flow rate of 3.0gpm is to be neutralized using either sulfuric acid or hydrochloric acid. First, determine the massflow rate (lb/day) of NaOH in the spent caustic soda solution, and then use that value todetermine the stoichiometric amounts (lb/day) of:1. H2SO4 required for neutralizing the OH− ions contributed by the spent caustic soda.[Hints: (1) write the balanced chemical equation for the acid-base reaction betweenNaOH and H2SO4, and use it to establish the stoichiometric weight ratio H2SO4 : NaOH.]2. HCl required for neutralizing the OH− ions contributed by the spent caustic soda. [Hints:(1) write the balanced chemical equation for the acid-base reaction between NaOH andHCl and use it to establish the stoichiometric weight ratio HCl : NaOH.]
Six 50.0 ml volumetric flask 1-6 are labeled. 10.00 ml of 2.00 x 101 M Fe(NO3)3 solution was then pipet into each volumetric flask. A 1.00,2.00,3.00,4.00 and 5.00ml of 2.00 x 10-3M NaSCN solution was then pipetted to flask 2 through 6 respectively. A sufficient 0.10 M nitric acid was then added to each flask to make them total volume of 50.00ml. 1.a)Calculate the final Fe(NO3)3 concentrations for each. 1.b)Also how would you find the initial concentration of SCN- for each flask? Please show calculations to solutions.Thanks
A concentration of toxic metals in plant tissue is often found by combusting the material in a furnace and then dissolving the ash in concentrated acid. A 0.5124-gram sample of leaves was combusted to ash and transferred to a 150-mL beaker. A 25-mL portion of concentrated HCl was added and the mixture was heated on a hot plate. Three 5-mL portions of concentration HCl were added over approximately 10 minutes with continued heating in between additions. The resulting mixture was cooled to room temperature and filtered into a 50-mL volumetric flask, which was brought to volume using distilled water and mixed well. From this stock solution, a 10-mL portion was pipetted into a clean 50-mL volumetric flask, brought to volume with distilled water, and mixed. This final solution was analyzed and found to contain 12.1 ppm lead. What are the mass percent of lead in the original plant tissue?
Six 50.0 ml volumetric flask 1 through 6 are labeled. 10.00 ml of 2.00 x 10-1 M Fe(NO3)3 solution was then pipet into each volumetric flask. A 1.00,2.00,3.00,4.00 and 5.00ml of 2.00 x 10-3M NaSCN solution was then pipetted to flask 2 through 6 respectively. A sufficient amount of 0.10 M nitric acid was then added to each flask to make each a total volume of 50.00ml. Hint M1V1=M2V2 a)what would be the concentration of Fe(NO3)3 in 0.10M HNO3? b)what would be the concentration of NaSCN in 0.10M HNO3?
A 15.0% by weight solution was prepared using 90.0g of KCl and the resulting density of the solution is 1.101g/mL. (MW KCl 74g/n). volume of solution(mL)? milliosmole of solute? %w/v? weight of solvent(g? N?
The %purity of a powdered crude sample of Na2CO3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr. a. How many moles of CO2 were collected? b. What is the percent purity of the sample? Round off to the nearest whole number
The %purity of a powdered crude sample of Na2CO3 containing only inert impurities is to be determined by reacting 225.0 mg of the crude sample to 10.0 mL of 3.00 M HCl solution, and bubbling the resulting CO2(g) product in water that is at exactly 29 °C. After the reaction has completed, the level of the liquid inside the eudiometer rests 4.30 cm above the water level in the beaker. The graduation on the eudiometer indicates that the trapped gas is 44.37 mL. The experiment was done under a barometric pressure of 755.2 torr. What CASE does this experiment satisfy?