The reaction between 0.052 g of magnesium with excess HBr was carried out in an ice calorimeter as used in this lab. The volume of water in the calorimeter was observed to decrease by 0.26 mL during the reaction. Calculate the enthalpy of reaction in kJ/mol. Answer to the nearest whole number, do not include units and use the appropriate sign! Your Answer: Answer

The reaction between 0.052 g of magnesium with excess HBr was carried out in an ice calorimeter as used in this lab. The volume of water in the calorimeter was observed to decrease by 0.26 mL during the reaction. Calculate the enthalpy of reaction in kJ/mol. Answer to the nearest whole number, do not include units and use the appropriate sign! Your Answer: Answer

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Calculate the energy of combustion per gram of Olive Oil (kJ/g) if 31.0 mL of water is placed in the test tube and the temperature changes from 22.9 °C to 44.6 °C. The initial mass of the spirit burner is 204.60 g and the final mass is 204.51g. State your answer with correct significant digits. Notes: • Include a negative sign if the reaction is exothermic • Do not include units in your answer.
Could you do question C please
Ignition wires heat sample Thermometer Stirrer A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.4059 g sample of 9,10-anthracenedione (C14H30,) is burned completely in a bomb calorimeter. The calorimeter is surounded by 1.116x10³ g of water. During the combustion the temperature increases from 22.76 to 25.09 °C. The heat capacity of water is 4.184 Jgl°c-!. Water The heat capacity of the calorimeter was determined in a previous experiment to be 965.5 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 9,10-anthracenedione based on these data. C14HgO2(s) - 1502(g) 4 H20(1) + 14 CO,(g) - Energy Molar Heat of Combustion = kJ/mol Sample dish Burning sample Steel Insulated outside chamber bomb Combustion (bomb) calorimeter.
Try Again Row 3: Your answer is wrong. In addition to checking your math, check that you used the right data and DID NOT round any intermediate calculations. A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). First, a 7.000 g tablet of benzoic acid (CH₂CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 15.00 °C to 53.26 °C over a time of 12.3 minutes. Next, 5.420 g of acetylene (C₂H₂) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 15.00 °C to 74.42 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or…
A certain chemical reaction releases 13.4/kJg of heat for each gram of reactant consumed. How can you calculate the heat produced by the consumption of 3.2kg of reactant? Set the math up. But don't do any of it. Just leave your answer as a math expression. Also, be sure your answer includes all the correct unit symbols.
+ 1 on CI- CI Q A Z @ 2 Click to edit molecule W S ●● command X Carbon tetrachloride, (CCI) is a solvent used in dry cleaning. Draw the Lewis structure of CCI and then determine the ideal bonding angle(s) for the CI-C-CI bond(s). www # 3 CJ Cl: . E D 8.0 F3 C $ 4 R JAN 25 A a FA FLO % 5 V T G Question 1 of 26 6 B FG Y H & 7 A) 90° B) 109.5° C) 120° D) 180° F7 לון U N 8 J DII FB I M ( 9 K F9 zoom O O H F10 L P command F11 { J F12 = ? option 1
When 3.8 g A are reacted with 8.5 g D, according to the balanced chemical equation below, 33 kJ of energy are released. Please calculate the enthalpy for this reaction when 3 moles of G are produced. 2A + 3D = 2Z + 3G given molar masses: A = 141.8 g/mole D = 63.996 g/ mole Z = 4.032 g/ mole G = 56.028 g/ mole
Calorimetry is a method used to measure enthalpy, or heat, changes that occur during chemical processes. Two common calorimeters are constant- pressure calorimeters and constant-volume (or "bomb") calorimeters. Part A A simple constant-pressure calorimeter can be made from a foam coffee cup and a thermometer; energy changes in a reaction are observed via a temperature change of the solution in the cup. Bomb calorimeters are used to measure combustion and A total of 2.00 mol of a compound is allowed to react with water in a foam coffee cup and the reaction produces 175 g of solution. The reaction caused the temperature of the solution to rise from 21.00 to 24.70 °C. What is the enthalpy of this reaction? Assume that no heat is lost to the surroundings or to the coffee cup itself and that the specific heat of the solution is the same as that of pure water. Enter your answer in kilojoules per mole of compound to three significant figures. other gas-producing reactions, where the reaction…