I Review I Constants I Periodic Table Instant cold packs, often used to ice athletic injuries on the field, contain ammonium nitrate and water separated by a thin plastic divider. When the divider is broken, the ammonium nitrate dissolves according to the following endothermic reaction: NHẠNO3 (s) → NH;(aq) + NO3 (ag) Part A Calculate the change in enthalpy for the reaction. (Use 1.0 g/mL as the density of the solution and 4.18 J/(g.°C) as the specific heat capacity.) Express the enthalpy change in kilojoules per mole to two significant figures. In order to measure the enthalpy change for this reaction, 1.25 g of NH4NO3 is dissolved in enough water to make 25.0 mL of solution. The initial temperature is 25.8 ° C and the final temperature (after the solid dissolves) is 21.9 ° C. Bνα ΑΣΦ You may want to reference (Pages 385 - 387) Section 9.7 while completing this problem. ΔΗΚn kJ/mol Request Answer Submit

I Review I Constants I Periodic Table Instant cold packs, often used to ice athletic injuries on the field, contain ammonium nitrate and water separated by a thin plastic divider. When the divider is broken, the ammonium nitrate dissolves according to the following endothermic reaction: NHẠNO3 (s) → NH;(aq) + NO3 (ag) Part A Calculate the change in enthalpy for the reaction. (Use 1.0 g/mL as the density of the solution and 4.18 J/(g.°C) as the specific heat capacity.) Express the enthalpy change in kilojoules per mole to two significant figures. In order to measure the enthalpy change for this reaction, 1.25 g of NH4NO3 is dissolved in enough water to make 25.0 mL of solution. The initial temperature is 25.8 ° C and the final temperature (after the solid dissolves) is 21.9 ° C. Bνα ΑΣΦ You may want to reference (Pages 385 - 387) Section 9.7 while completing this problem. ΔΗΚn kJ/mol Request Answer Submit

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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A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with 22.4 mL of 6.45 M hydrochloric acid. The temperature of the mixture rises 17.2 ° C. The density of the resulting solution is 1.00 g mL and has a specific heat capacity of 4.184 J g · ° C . The heat capacity of the calorimeter is 16.97 J ° C . Part 1: (a) Identify the limiting reagent for the reaction. Part 2: (b) Calculate the heat of reaction (in J). qrxn = × 10 JEnter your answer in scientific notation. Part 3 out of 3 (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization = ____ kj/mol
Consider the following reaction. (a) Is the reaction exothermic or endothermic? exothermic endothermic CH3OH(g) → CO(g) + 2 H₂(g) AH +90.7 kJ (b) Calculate the amount of heat transferred when 35.0 g of CH3OH(g) are decomposed by this reaction at constant pressure. ΔΗ= 100.8 (c) If the enthalpy change is 19.0 kJ, how many grams of hydrogen gas are produced? 0.42 x g (d) How many kilojoules of heat are released when 13.0 g of CO(g) reacts completely with H₂(g) to form CH₂OH(g) at constant pressure? AH = -90.7 X kJ (e) Calculate AE when 400.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol K-41.7 XkJ HopHelpCh5N1
1. 25 g of sodium (Na) is put into 200 mL of water. The reaction between the two produces sodium hydroxide (NaOH) and hydrogen gas, and increases the temperature by 14 °C. (a) Calculate the enthalpy change, AH, of the reaction. (C; = 4.18 JºC•3; d= 1 g/mL) (b) Is this reaction endothermic or exothermic? (c) Based on your calculation, determine what is considered as the surrounding in this experiment.
The Haber process is used to manufacture ammonia from nitrogen and hydrogen in the presence of an iron catalyst. The reaction, shown in this equation, is exothermic: N 2 (g)+3H 2 (g) rightleftharpoons 2N*H_{3}(g) + Heat Which statement correctly describes the chemical reaction? The energy needed to break the chemical bonds of 1 mole of nitrogen and 3 moles of hydrogen is greater than the energy released by the formation of 3 moles of ammonia. The energy needed to break the chemical bonds of 1 mole of nitrogen and 3 moles of hydrogen is less than the energy released by the formation of 3 moles of ammonia. The energy released by breaking the chemical bonds of 1 mole of nitrogen and 3 moles of hydrogen is greater than the energy needed to form 3 moles of ammonia. The energy released by breaking the chemical bonds of 1 mole of nitrogen and 3 moles of hydrogen is less than the energy needed to form 3 moles of ammonia.
The reaction between HCl and NaOH is represented below. When equal volumes of 1.00 M NaOH and 1.00 M HCl are mixed, 57.1 kJ of heat is released. What would A H be if 2.00 M HCI and 2.00 M NaOH is used instead of 1.00 M? HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l) AH = -57.1 kJ/mol... (A) - 28.6 kJ B-85.7 kJ (c) -57.1 kJ D - 114 kJ
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Determine the mass of water that is produced when 673 kJ of heat is absorbed in the following reaction? H₂A (s) + 2 XOH (ag) --> X₂A (aq) + 2 H₂O (g) AH = 448.4 kJ You may or may not need the following molar mass information: H₂O molar mass = 18.01 g/mol X₂A molar mass = 113.24 g/mol Report with the correct number of significant figures. Include the correct unit. Your Answer: Answer units
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