Measure 1.0 g of the copper gluconate in the weighboat on the scale. - Lesson for Kids, How to Measure & Compare Liquid Volume: Lesson for Kids, Elements Lesson for Kids: Definition & Facts, How to Estimate Measurements of Distance: Lesson for Kids, The Human Circulatory System Lesson for Kids, How to Estimate Liquid Volume: Lesson for Kids, Magnetism Lesson for Kids: Definition & Facts, Density Lesson for Kids: Definition & Facts, Perimeter Lesson for Kids: Definition & Examples, Changing States of Matter Lesson for Kids, CSET Science Subtest I - General Science (215): Practice & Study Guide, FTCE Middle Grades General Science 5-9 (004): Test Practice & Study Guide, ILTS Science - Physics (116): Test Practice and Study Guide, ILTS Science - Environmental Science (112): Test Practice and Study Guide, SAT Subject Test Chemistry: Practice and Study Guide, CSET Science Subtest II Earth and Space Sciences (219): Test Prep & Study Guide, ILTS Science - Earth and Space Science (108): Test Practice and Study Guide, CSET Science Subtest II Chemistry (218): Practice & Study Guide, UExcel Earth Science: Study Guide & Test Prep, UExcel Basic Genetics: Study Guide & Test Prep, UExcel Weather and Climate: Study Guide & Test Prep, Middle School Physical Science: Help and Review, Biological and Biomedical Use the givens and unknowns in Table 2 and Table 3 to solve. A. If 3.0 M H 2 SO 4 is available, then .01÷3.0 L or 3.3 mL of 3.0 M H 2 SO 4 are necessary to react.. 5. All other trademarks and copyrights are the property of their respective owners. 3. 1. Include your calculations if initial mass of copper gluconate is 1.4 g, copper produced =0.2 g. Copper Gluconate: Copper gluconate is the copper salt of gluconic acid. Then we're going to convert from mass to moles, divide, and determine subscripts. Determine the number of moles of copper in the copper gluconate using your results. Use the givens and unknowns in Table 3 and Table 4 to solve. The calculations are as follows: Mass of Cu wire: 1.956 g Mass of copper sulfide formed: 2.447 g Mass of combined sulfur: 0.491 g . Determine the number of moles of copper in the copper gluconate using your results. Calculate the theoretical yield of calcium carbonate, identify the limiting reactant, and given an actual yield of 6.35g, calculate the percent yield. 2. Finding molar mass starts with units of grams per mole (g/mol). Include your calculations. What is the mass of the gluconate? The ultimate goal is to find out the chemical formula of the compound as well as a few other things. Definitions of molecular mass, molecular weight, molar mass and molar weight: Molecular mass (molecular weight) is the mass of one molecule of a substance and is expressed in the unified atomic mass units (u). The reason is that the molar mass of the substance affects the conversion. In your case, every mole of copper(II) chloride, "CuCl"_2, is composed of one mole of copper atoms, two moles of chlorine atoms As you know, the molar mass of a substance tells you the mass of one mole of said substance. Include your calculations … Include your calculations 2. To calculate molar mass of a chemical compound, please enter its chemical formula and click 'Calculate'. The following chemical reaction was carried out in a hood in a university laboratory. Calculate the molar mass of each of the following compounds: (a) Fe(C 6 H 11 O 7) 2, iron(II) gluconate, a dietary supplement (b) CH 3 CH 2 CH 2 CH 2 SH, butanethiol. I have included the worksheets so if anyone will help me work through them possibly explaining them to me like I'm five, I would be eternally grateful. For hydrogen chloride, the molar mass is 1.007 + 35.453 = 36.460 g/mol. Include your calculations - 1.4g of copper gluconate – 0.2g of copper= 1.2g of gluconate 5. 3. What is the mass of the gluconate? Take the products you obtained in the previous step and add them all together to calculate the molar mass of the compound. In this case, copper(II) chloride has a molar mass of "134.452 g/mol". 3. A mole is a number of atoms or particles of a particular element or substance, which is equal to 6.02214076 × 10²³ (you may recognize this as Avogadro's constant). Include your calculations. 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