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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used in mothballs‚ produced 8.80g CO2 and 1.44 H2O. Calculate the empirical formula for naphthalene. 8.80g CO2 (find moles of Carbon by dividing the molar mass and doing the molar ratio of C and CO2 = 0.200mol C. 1.44H2O (find moles of Hydrogen by dividing the molar mass of water and doing the ratio of 2moil H/1molH2O) 0.160mol H divide them by the smallest number of moles C = 1.25 H= 1 Multiply 4= 5‚ H=4 1) If the molar mass of naphthalene is 128.18g/mol what is the molecular formula
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vinegar. The second part of the experiment was to see if by titrating a solution of NaOH and an unnamed mystery acid‚ you could find the molar mass of the unknown acid (solving the mystery). It must be understood that the number of moles of the reacting NaOH and the number of moles of the product NaX acid‚ must both equal (in this case 1:1) in order for the calculation to find the molar mass to work. Procedure: Begin the procedure by first making sure all glassware has been cleaned. Next set up the
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figures; • convert physical quantities from one system of units to another; • explain various laws of chemical combination; • appreciate significance of atomic mass‚ average atomic mass‚ molecular mass and formula mass; • describe the terms – mole and molar mass; • calculate the mass per cent of different elements constituting a compound; • determine empirical formula and molecular formula for a compound from the given experimental data; • perform the stoichiometric calculations.
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lab) 1. Use the equations given on the front page to determine the number of moles of sodium thiosulfate that are equivalent to one mole of sodium hypochlorite. 2. From your three trials‚ calculate the average volume of Na2S2O3 needed for the titration of 25.00mL of diluted bleach. 3. Use the average volume and the molarity of Na2S2O3 to determine the molarity of the diluted bleach. (Find moles of Na2S2O3‚ convert to moles of NaClO‚ and divide by volume of dilute bleach that was titrated in each trial
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white crystalline powder with no odor and a bitter taste. It is a derivative of morphine in that the –OH (hydroxyl group) is replaced by an acetyl group‚ -OCOCH3 and has a molecular formula is C21H23NO5 with a molecular weight of 369.42 grams per mole and a melting point of 173°C. Heroin is a schedule I controlled substance meaning it has no medical uses and has a high potential for abuse. Abuse is classified as illegal usage of a drug or excessive use above recommended dosage. Some health effects
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______________________________________________________________________ Combustion Reaction: ______________________________________________________________________ Mole Ratio: ______________________________________________________________________ Diatomic Molecule: ______________________________________________________________________ Mole: ______________________________________________________________________ Hydrocarbon: ______________________________________________________________________
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moles-stoichiometry-practice-problems Now you’re ready to use what you know about conversion factors to solve some stoichiometric problems in chemistry. Almost all stoichiometric problems can be solved in just four simple steps: 1.Balance the equation. 2.Convert units of a given substance to moles. 3.Using the mole ratio‚ calculate the moles of substance yielded by the reaction. 4.Convert moles of wanted substance to desired units. These "simple" steps probably look complicated at first
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