MCEOCkeyII - MasteringChemistry: Assignment Print View

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MasteringChemistry: Assignment Print View http://session.masteringchemistry.com/myct/assignmentPrint?assignmen. .. 1 of 11 9/2/2008 10:16 AM Assignment Display Mode: Chemistry 1212 Gas Laws Hmwk II Due at 5:00pm on Friday, August 29, 2008 View Grading Details Stoichiometric Relationships with Gases Description: Calculate the mass of reactant needed to yield a given volume of gaseous product and calculate the volume of gas produced from the given mass of reactant. The ideal gas law relates pressure , volume , temperature , and number of moles of a gas, . The gas constant equals 0.08206 or 8.3145 . The equation can be rearranged as follows to solve for : This equation is useful when dealing with gaseous reactions because stoichiometric calculations involve mole ratios. Part A When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction How many grams of calcium carbonate are needed to produce 83.0 of carbon dioxide at STP? Hint A.1 How to approach the problem First, use the ideal gas law to calculate the number of moles. Recall that standard temperature and pressure (STP) is 273 and 1.00 . Next, use the mole ratio (given by the coefficients in the balanced equation) to determine the moles of calcium carbonate needed. Finally, convert to grams of calcium carbonate by using its molar mass. Part A.2 Calculate the moles of CO 2 How many moles of carbon dioxide occupy a volume of 83.0 at STP? Hint A.2.a How to approach the problem Recall that standard temperature and pressure (STP) are 0 (273 ) and 1.00 . When the volume, temperature, and pressure are known, the number of moles of gas can be calculated by using the ideal gas law ( ). Make sure to use the appropriate value (look at the units). Express your answer numerically in moles. ANSWER: moles of = Part A.3 Calculate the moles of CaO needed How many moles of calcium carbonate are needed to produce 3.70 of carbon dioxide? Hint A.3.a How to approach the problem According to the balanced reaction equation, 1 of produces 1 of . Therefore, the mole ratio is 1:1. Express your answer numerically in moles. [ Print
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MasteringChemistry: Assignment Print View http://session.masteringchemistry.com/myct/assignmentPrint?assignmen. .. 2 of 11 9/2/2008 10:16 AM ANSWER: moles of =
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MasteringChemistry: Assignment Print View http://session.masteringchemistry.com/myct/assignmentPrint?assignmen. .. 3 of 11 9/2/2008 10:16 AM Problem 9.63: Section Problem Description: The average oxygen content of arterial blood is approximately conc_O2 of O_2 per liter. (a) Assuming a body temperature of T, how many moles of oxygen are transported by each liter of arterial blood? (b) How many milliliters of oxygen are. .. The average oxygen content of arterial blood is approximately 0.26 of per liter. Part A Assuming a body temperature of 37 , how many moles of oxygen are transported by each liter of arterial blood?
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This note was uploaded on 03/08/2010 for the course CHEMISTRY CHE111 taught by Professor Pat during the Spring '10 term at Northampton Community College.

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MCEOCkeyII - MasteringChemistry: Assignment Print View

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