3. What is the difference in weight, in pounds, between 1 L of water and 1 L of mercury? The density of water is 1.00 g/mL, and the density of mercury is 13.56 g/mL
Q: A certain liquid has a density of 2.67 g/cm3. 30.5mL of this liquid would have a mass of what in kg?
A:
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A: Given that : Mass of earth = 5.98 ×10²⁴ kg
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A: Given: density of diamond = 3.52 g/mL. And mass of diamond = 15.1 g
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A: To find: volume is occupied by 42.5 g of organic solvent
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A: Given, density = 11.3 g/cm3. Mass = 1432 gm
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A: The volume and mass of a substance are related by the density of a substance.
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A: Given Density= 1.5 g/ml Volume= 16.0ml Mass= ?
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A: The density, of a substance is it's mass per unit volume and is denoted by ρ. ρ = mv
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A: Given;
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A: Given : Mass = 64.02g
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A: Given : Length of brick = 15.24 cm Width of brick = 7.62 cm And height of brick = 2.54 cm
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- pls complete the 2nd table given the data1. 500.0 mL 0.2 M KI2. 500.0 mL 0.2 M KCl3. 500.0 mL 0.1 M K2S2O84. 500.0 mL 0.1 M K2SO45. 500.0 mL 4.0 mM Na2S2O3 (from Na2S2O3∙5H2O)5- What are the following abbreviations stands or? PPM, TMS, , Hz?using exactly 5.00 mL of 0.0400 M stock CuSO4 solution. Add 100 mL of water. Data for Part IMass of empty dish: 32.470 g empty dishVolume of 0.0400 M solution: 5.00 mL CuSO4 solution.Mass of dish and 0.0400 M solution: 37.497 g dish and solutionMass of dish and CuSO4 solid: 32.503 g dish and CuSO4 solidCalculations for Part I1. Calculate the mass of solution? 5.027 g 2. Calculate the mass of solid CuSO4 dissolved in the solution? 0.033 g 3. Calculate the number of moles of solid CuSO4 dissolved in the solution? 2.07 x 10-4 mol4. Calculate the mass of water evaporated from the solution? 0.0414 M5. Calculate the density of solution, (g solution/mL solution)?6. Calculate the % by mass, CuSO4 in solution (100 x g CuSO4/g solution)?7. Calculate the molality of solution (moles CuSO4/kg solvent)?8. Calculate the molarity of solution (moles CuSO4/L solution)?9. Given that the true molarity is 0.0400 M, calculate the percent error…
- a. If 55mg of CaC2O4 is placed in a 250mL pack of H2O nanopure at 25 celcius, how much (in mg) of CaC2O4 remains undesolved? b. If 100mg of CaC2O4 is placed in a 500mL pack of HCl at 25 celcius, how much (in mg) of CaC2O4 remains undesolved? FM: 128g/mol Pksp= 7.907. A procedure for measuring the amount of creatinine in blood was applied to a standard blood sample and the following results were produced: 0.787, 0.812, 0.796, 0.739, 0.802, and 0.823 mg/dL. a) Can any of the data points be rejected by the Grubbs test? b) What is the 95% confidence interval for the data?using exactly 5.00 mL of 0.0400 M stock CuSO4 solution. Add 100 mL of water. Data for Part IMass of empty dish: 32.470 g empty dishVolume of 0.0400 M solution: 5.00 mL CuSO4 solution.Mass of dish and 0.0400 M solution: 37.497 g dish and solutionMass of dish and CuSO4 solid: 32.503 g dish and CuSO4 solidCalculations for Part I1. Calculate the mass of solution2. Calculate the mass of solid CuSO4 dissolved in the solution.3. Calculate the number of moles of solid CuSO4 dissolved in the solution.4. Calculate the mass of water evaporated from the solution.5. Calculate the density of solution, (g solution/mL solution).6. Calculate the % by mass, CuSO4 in solution (100 x g CuSO4/g solution).7. Calculate the molality of solution (moles CuSO4/kg solvent).8. Calculate the molarity of solution (moles CuSO4/L solution).9. Given that the true molarity is 0.0400 M, calculate the percent error of your result.
- In the UV assay of paracetamol you are required to weigh tablet powder “…containing 0.150 g of Paracetamol…”. If the stated content of paracetamol per tablet is 500 mg and the weight of 20 tablets is 11.223 g then the amount of paracetamol tablet powder to be weighed isData Given. no Trial 3 information neededA student dissolves a Jefferson nickel to make 100.00 mL of solution in a volumetric flask. The student takes a 5.00 mL5.00 mL aliquot of the first solution and dilutes it to make 100.00 mL100.00 mL of a second solution. The student places a sample of the second solution in a cuvette for analysis using spectrophotometry. The molarity of the copper solution in the cuvette was determined by spectrophotometric analysis to be 2.90×10−2 M Cu.2.90×10−2 M Cu. Calculate the mass of copper in the Jefferson nickel used to make the first solution.
- A blood concentration of 0.065 M ethyl alchohol is sufficient to induce a coma. Blood alcohol content is a measure of alcohol in the blood as a percentage. It is calculated in grams per 100mL of blood, so a BAC os 0.08 means your blood is 0.08% alcohol by volume. a) What is the total mass of alcohol (in grams) that it represents for the same adult male whose total blood volume is 5.6L? b) What percentage does it represent from the coma induced level?Substance Melting Points in ℃ Benzoic acid 122.3 ℃ Succinimide 125-127 Urea 133 ℃ Cinnamic acid (trans). 133 ℃ Thiourea 182 ℃ Hippuric acid. 187 ℃ For Questions 1-3 assume that you were given 5.00 g of an unknown A for this lab, one of the six compounds whose melting points you looked up for prelab. 1. You recrystallized A and obtained 2.23 g pure product. What was your percent recovery? That is, what percent of the original mass did you get back? Show your work. 2. Assume you took the melting point of the pure product and it was 123oC. Considering…If l = 3, how many values of ml are possible? -- 1 3 5 7 9
