chlorine gas‚ Cl2‚ is 70.9 g/mol‚ what mass of chlorine gas contains 0.652 moles of chlorine gas? Question 5 options: 109 g 92.4 g 46.2 g 23.1 g 9.20 g Save Question 6 (2.7 points) What is the molar mass of dinitrogen pentoxide? Question 6 options: 108 g/mol 30 g/mol 150 g/mol 94 g/mol 44 g/mol Save Question 7 (2.7 points) How many nitrogen atoms are present in 3.00 × 10–3 moles of nitrogen gas‚ N2? Question 7 options: 1.81 × 1019 3.61 ×
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glycolitic enzymes during carbohydrate metabolism. Hydrogen is released and glucose is metabolized to pyruvic acid. In the presence of oxygen‚ the pyruvic acid is converted into acetyl coenzyme A. (Acetyl CoA). 1 mole of glucose produce 2 moles of ATP or 1 mole of glycogen produces 3 moles of ATP. * In the Kreb Cycle system‚ once the acetyl CoA is formed‚ it enters the krebs cycle‚ a complex series of chemical reactions that permit the complete oxidation of acetyl coenzyme A. in this process‚
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mass of ascorbic acid = 176mg‚ mass of ascorbic acid used = 1.25mg Number of moles in 0.00125g of ascorbic acid = 1/176 x 0.00125 = 7.102 x 10-6 moles Mole ratio of DCPIP: Ascorbic acid = 1:1 Number of moles of DCPIP used = 7.102 x 10-6 moles If 20mL of DCPIP = 7.102 x 10-6 moles Then 1 mL of DCPIP = 7.102 x 10-6/20 = 3.55 x 10-7 moles Therefore 5 mL of DCPIP = 3.55 x 10-7 x 5 = 1.775 x 10-6 moles Since mole ratio of DCPIP: Ascorbic acid
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To determine the percentage by mass of Calcium carbonate in an egg shell Aim: is to find and work out the percentage of calcium carbonate by mass in eggshells by using acid base “back titration” Introduction: Calcium Carbonate‚ CaCO₃‚ is a compound which is polymorphic and therefore means that it can be found in a variety of different objects or organisms. For example: Rocks (limestone‚calcite)‚ sea snail shells‚ Eggshells‚ pearls and many more. This investigation will focus on finding out the
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large amount of dissolved solute. C¬1V1 = C2V2 Systems for Expressing Concentrations of Solutions Name of System Symbol Definition Molarity M moles of solute / liter of solution Molality M moles of solute / kg of solvent Formality F gram-formula weight of solute /liters of solution Mole Fraction N‚ X moles of solute / moles of solvent + moles of solute Normality N equivalents of solute / liters of solution Weight percent wt. % 100 x grams of solute / grams of solvent + grams of solute
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Lab: STOICHIOMETRY The reaction of Iron with Copper(II) Sulfate Purpose: In this experiment we will use stoichiometric principles to deduce the appropriate equation for the reaction between metallic iron and a solution of copper (II) sulfate. This reaction produces metallic copper‚ which is seen precipitating as a finely divided red power. Materials: Flask beaker Copper solution Balance Hot plate •150 ml beaker •1 gram of iron power
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control the CV | Concentration of acid | Rate of reaction | Vol of acid | 20 ml | Measure using a 50ml Measuring cylinder | 2 moles pr. L | Vol of gas | Temp of acid | Room temp. | Not controlled‚ only montored | 1 moles pr. L | | Amount of Mg | 5 cm or ribbon/ 0.07g | Ruler‚ and weight | 0.5 moles pr. L | | Precence of catalyst | No | Not have a catalyst | 0.25 moles pr. L | | Type of acid | Hydrocloric | Have same type of acid | Method: 1. Gather aparatus and materials‚ and set up as
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sides of the beaker. Na2CO3 + CaCl22H2O = CaCO3 + 2NaCl + 2H2O Convert 1g of CaCl22H2O to moles‚ 1g CaCl22H2O x 1mol = .00689Moles CaCl22H2O 144.9994 Consider the mole ratio of Na2CO3 to CaCl22H2O 1:1 Thus‚ 1 mole of CaCl22H2O will equal 1 mole of Na2CO3 Convert moles of Na2CO3 to grams: .00689moles Na2CO3 x 105.99 = .73027g Na2CO3 1 mole Na2CO3 How much CaCO3 can we expect? .00689 moles of CaCl22H2O x 1mole CaCO3 = .00689Moles CaCO3 1mole CaCl22H2O Convert .00689Moles CaCO3
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precipitation reaction. This is a reaction where two soluble salts Sodium Carbonate and Calcium Chloride are added together and the result is the precipitation of single Product while the other product remains in solution. This means by using the moles in this lab we could find the limiting reactant‚ percentage yield and the percent purity Materials: * Electronic Scale * Sodium Carbonate * Calcium Chloride * Wayne Paper
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the crucible with hydrate‚ and the crucible with an anhydrous and write down each weight‚ then repeat. Once we completed that task then we were to find the number of moles of water lost‚ the number of moles of anhydrous copper sulfate‚ percent comp of water in the hydrated copper sulfate‚ the mole ratio of moles of water and moles of anhydrous copper sulfate. Once this is all done‚ we found our percent error and compared it to the exact value. In the lab‚ we used the following tools: lab apron
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