Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Transcribed Image Text:1. What quantity is conserved in the reaction shown below? (circle all that apply)
2 HCI + Ca(OH)₂ 2 H₂O + CaCl₂
molecules
moles
atoms
mass (grams)
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- When chemists work with solid materials, we simply weigh out amounts of solid reagents and calculate mole amounts when thinking about stoichiometry. However, when we dissolve a solid (also known as a solute) in a solvent to form a solution, the solute becomes evenly distributed throughout the solution and we need to know how many moles of solute are present in a particular volume of solution. A solution is created by dissolving 12.5 grams of ammonium chloride in enough water to make 295 mL of solution. How many moles of ammonium chloride are present in the resulting solution? When thinking about the amount of solute present in a solution, chemists report the concentration or molarity of the solution. Molarity is calculated as moles of solute per liter of solution. What is the molarity of the solution described above? To carry out a particular reaction, you determine that you need 0.0500 moles of ammonium chloride. What volume of the solution described above will you need to…arrow_forward1arrow_forwardTrue or False? A molar ratio is a ratio between the number of moles of any two components involved in a chemical reaction.arrow_forward
- < [Review Topics] [References) Use the References to access important values if needed for this question. For the following reaction, 0.577 moles of methane (CH4) are mixed with 0.399 moles of carbon tet methane (CH4) (g) + carbon tetrachloride (g) → dichloromethane (CH₂ Cl₂) (g) What is the formula for the limiting reactant? What is the maximum amount of dichloromethane (CH₂ Cl₂) that can be produced? Amount = mol Submit Answer Retry Entire Group 4 more group attempts remainingarrow_forwardWhich of the following is NOT true about "yield"? * The percent yield is the ratio of the actual yield to the theoretical yield. The value of the actual yield must be given in order for the percent yield to be calculated. The actual yield may be different from the theoretical yield because insufficient limiting reagent was used. The actual yield may be different from the theoretical yield because reactions do not always go to completion.arrow_forwardA chemist will use a sample of 30 g of ethanol (CH3CH2OH) in an experiment. In one to two sentences, make and justify a claim about the number of moles of ethanol the chemist will usearrow_forward
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