Higher Chemistry Mole Calculations Moles and Number 1 mole of any substance contains the same number of atoms/molecules/ions as there are atoms in a 12g sample of carbon -12 12g of carbon-12 contains a constant number of atoms. This number is known as the Avogadro constant (L) and is equal to 6.02 x 1023. 1 mole of carbon-12 contains 6.02 x 1023 atoms. Therefore‚ 1 mole of any substance contains 6.02 x 1023 atoms/molecules/ions. For example‚ 1 mole of aluminium contains
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MEASURING AMOUNT OF SUBSTANCE MASS VOLUME MOLAR MASS AVOGADRO [pic] CONCENTRATION ATOM ION MOLECULE COURSE OUTLINE OCR Chemistry A Unit 1 – Autumn Term 2012 • Atoms and Electron Structure • Moles‚ Equations and Acids • Structure and Bonding • Redox‚ Group 2 and Group 7 Unit 1 Exam – January 2013 – 1 hour – 90 UMS – 30% of total Unit 2 – Spring Term 2013 • Basic Concepts in Organic Chemistry • Alkanes and
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Stoichiometry calculation • Limiting reactant • Theoretical yield‚ actual yield and percentage yield 1 2 Mole Concept No. of Moles = Molarity (M) • Molarity (molar concentration) is the number of moles of a solute that is contained in 1 liter of solution Mass (g) molar mass (g/mol) No. of Moles = Molarity (mol/L) volume (L) Molarity (M) = Amount of solute (Mol) Volume of solution (L) • 1 mole contains 1 Avogadro’s number (6.022 x 1023) 3 Example: Saline Water Concentration Typical seawaters contain
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element to the equivalent number of moles of that element. To find the simplest formula of a compound‚ we will combine the elements in the compound under conditions that allow us to determine the mass of each element. From these data‚ the moles of atoms of each element may be calculated. By dividing the numbers to the smallest number of moles‚ you obtain quotients that are in a simple ratio of integers or are readily converted to such a ratio. The ratio of moles of atoms of the elements in a compound
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below. 1. Calculate the number of moles of CaCl2·2H2O from the mass you weighed out and record in the table below. Have Factor (molar mass) Want _____ g CaCl2·2H2O ___ moles CaCl2·2H2O Note: CaCl2·2H2O is an example of a hydrate‚ the 2 water molecules are attached to the crystal structure of the compound. When determining the molar mass‚ add the mass of 2 water molecules to the mass of the CaCl2. 2. From the balanced equation calculate the number of moles of Na2CO3 required to react completely
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in a solution to its pure vapour pressure p∗ by its mole fraction in solution χa . a pa = χa p∗ a This allows us to calculate the mole fraction of 2-propanol χp (in the solution with the dissolved unknown) to the solutions vapour pressure pp and the vapour pressure of pure 2-propanol p∗ . p χp = pp /p∗ p 1 CHEM 3411‚ Fall 2010 Solution Set 5 Additionally‚ we know the solution only contains 2-propanol and the unknown with moles fraction of χp and χu respectively‚ and therefore χp
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allowed three trials‚ and will be graded on accuracy. Lab Questions: 1. HA(aq) + NaOH(aq) NaA(aq) + H2O 2. Trial 1: .1010 M of NaOH = moles of NaOH / 0.0299 L = 0.0030199 mols of NaOH Trial 2: .1010 M of NaOH = moles of NaOH / 0.0227 L = 0.0022927 mols of NaOH Trial 3: .1010 M of NaOH = moles of NaOH / 0.0158 L = 0.0015958 mols of NaOH After we find the moles of NaOH‚ we can use that to find the molar mass of each acid. Trial 1: 0.261g / 0.0030199 = 86.43 mm of acid Trial 2: 0.233g / 0.0022927
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Determine the g-moles of methanol in 200.0kg of the mixture. b) The flow rate of methyl acetate in the mixture is to be 100.0 Ib-mole/h. What must the mixture flow rate be in Ibm/h 6. The feed to an ammonia synthesis reactor contains 25 mole% nitrogen and the balance hydrogen. The flow rate of the stream is 3000kg/h. Calculate the rate of flow nitrogen into the reactor in kg/h. 7. A mixture is 10.0 mole% ethyl alcohol‚ 75.0 mole % ethyl acetate (C4H8O2) and 15.0 mole% acetic acid. Calculate
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Regents Chemistry Quarter 1 Midterm Review 1. The percent by mass of oxygen in Na2SO4 (formula mass = 142) is closest to 1) 11% 3) 45% 2) 22% 4) 64% 2. Given the unbalanced equation: __Al(s) + __O2(g) → __Al2O3(s) 3. 4. 5. 6. 7. balance the equation using smallest whole number coefficients. The percent by mass of aluminum in Al2O3 is approximately 1) 18.9 3) 47.1 2) 35.4 4) 52.9 What is the approximate percent composition by mass of CaBr2 (formula mass = 200)
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Student: Glavin Wiechert Group Member: Victoria Coe Due Date: May 2‚ 2011 Teacher: Louth‚ Ellen Mary Class: Chemistry 11 Ad Introduction: An empirical formula of a chemical compound is the ratio of atoms in simplest wholenumber terms of each present element in the compound. For example‚ Glucose is C H O ; it’s empirical formula is CH O. 6 12 6 2 A hydrate is a compound that is chemically combined with water molecules. In contrast‚ an anhydrate does not contain water
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