In the lab you measure a clean, dry, crucible & cover to be 24.36 grams. You obtain a 2 cm piece of pure magnesium metal. After polishing the magnesium, you place it into your crucible and together the mass of the crucible, cover and magnesium was determined to be 24.66 grams. You observe that the magnesium is gray and shiny. You heat the crucible gently at first then vigorous for 10 minutes until the magnesium ignites. After the crucible cools you add a few drops of distilled water and heat again. The mass of the magnesium compound, crucible, and cover was determined to be 24.85 grams.  Determine the empirical formula of the compound. Show all work & units. The empirical formula can be determined via stepwise calculation of the quantities below. Mass of the Mg Mass of the MgO Mass of O Moles of Mg & Moles of O: Molar ratio of Mg/O: Empirical formula of compound, MgxOy

Porosity is a measure of the void or empty spaces in a material and is a fraction of the volume of voids over the total volume. The density of the solid material used to create 13 pieces of 0.6 cm diameter and 0.67 cm height cylindrical beads is determined to be 1.53 g/mL. These beads were then placed in a flask and was filled to the 42 mL mark with a salt solution. The total weight measured of the beads and the salt solution was 51.68 g. Upon further inspection, it was found that manufacturing defects caused the measured porosity of the beads to be at 21%. Assuming that the solution was able to fully fill the empty spaces inside the beads, calculate the density of the salt solution. Show your solutions in the next item Round your answer to 2 decimal places. Add your answer

4. A new procedure for the determination of sulfur in coal was tested on a standard coal sample with a certified value of 2.14% sulfur by mass. The new procedure gave results of 2.11%, 2.07%, 2.04%, 2.06%, and 2.16% for five separate determinations.  a) Does the new procedure give the correct result at the 95% confidence level?  b) Does the new procedure give the correct result at the 90% confidence level?

For the gravimetric determination of manganese, 1.8762 g of sample containing Mn was dissolved in acid solution and made up to 100 mL in a calibrated volumetric flask. A 25.00 mL aliquot of this solution was transferred to a beaker. The solution was heated to boiling and chemical substances required were added till precipitating MnNH4PO4. After filtering, rinsing, and igniting, 0.5365 g of Mn2P2O7 was obtained. Calculate the % manganese in the sample (Mn: 55, P: 31, O: 16 g/mol).

Luke needs to measure the iron (Fe) content of a 2.007 g steel sample. He starts by completely converting the iron in the steel to Fe²+ and dissolving it in 50.00 mL of water. Then, Luke determines the amount of Fe²+ by reacting it with a standardized aqueous 0.150 M potassium permanganate (KMnO4) solution. Mn²+ + 5 Fe³+ + 4H₂O The titration of the Fe²+ solution requires 37.47 mL KMnO, solution to reach the end point. What is the percentage by weight of iron (Fe) in the steel sample? MnO +8H+ + 5 Fe²+ - → percentage by weight: 75.02 Incorrect % Fe

The relative error calculated for the analysis of Zn alloy was -4.1%. Assuming that the sample is supposed to contain 60 mg Zn. Calculate the measured mass of Zn.

How many grams of Mn3O4 can be obtained from 1.00 g MnO2? how many ounces of Mn3O4 can be obtained from1.00 lb  MnO2?  Whatwt of Mn ore should  be taken so that the percentage of MnO2 in the ore can be found by multiplying by 5 to the number of centigrams og Mn3O4

I would need help answering this question with the steps please

७.ग. 4.74 x 100 = 22.217. 4. Bleach products are sold as 5.25-7.5% hypochlorite concentration depending on whether they are "regular" or "extra-strength"? How do your mass percentages compare to these values? One of my valves falls into that range but the other two fall a little short. 5. Bleach products slowly decompose over time eventually rendering them useless. What steps can be taken to slow this (think back to the chapter on Kinetics) when storing your bleach product? The bleach products could be stored at a certain temperature and kept away from the light. This will help slow the decomposition. 6. As mentioned in the introduction, one type of bleach alternative uses hydrogen peroxide to remove stains. The H₂O2 in the product can be titrated with the MnO4 under acidic conditions by the reaction: 5 H₂O2(aq) + 2 MnO4 (aq) + 6 H* (aq) 5 02(g) + 2 Mn+2 (aq) + 8 H₂O(). If a 0.505g sample of a product containing H₂O₂ required 16.55mL of a 0.01158M MnO4 solution to reach the end point,…

A sample of steel weighing 0.1798 g was dissolved and the manganese present was converted to MnO4– (aq). Water was then added to give a final solution volume of 100.00 mL. The concentration of MnO4– (aq) in this solution was 1.71 x 10-4 M. What is the percent Mn in this sample of steel?