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From the given information in the table, calculate: 1)qcontent(J) for part A and B 2) qrxn (J) for part A and B 3) standard enthalpy for part A and B 4) enthalpy of decomposition of NH4CL 5) literature enthalpy of decomposition of NH4Cl

From the given information in the table, calculate: 1)qcontent(J) for part A and B 2) qrxn (J) for part A and B 3) standard enthalpy for part A and B 4) enthalpy of decomposition of NH4CL 5) literature enthalpy of decomposition of NH4Cl

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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From the given information in the table, calculate: 1)qcontent(J) for part A and B 2) qrxn (J) for part A and B 3) standard enthalpy for part A and B 4) enthalpy of decomposition of NH4CL 5) literature enthalpy of decomposition of NH4Cl
O Search (Alt+Q) erences Mailings Review View Help Table Design Layout Aa v A EE AL T O Fin Emphasis Heading 1 Heading 2 三。 E Rep A Sle Paragraph Styles Editi Table 1Report): Determination of the enthalpy of decomposition of ammonium chloride Reactions Part A Part B reagents HCl NH3(a9) NH,Cl) water volume (mL) 25 25 50ml molarity (M) 0.9776 1.30 mass of beaker + NH,CI (g) 31.622 mass of emptied beaker (g) 29.720 mass of NH,CI (g) 1.902 n (mmols) 0.0244 0.0325 0.036 volume (mL) 50 ml 50ml total calorimeter Density (g mL1) 1.00 1.00 Mass = density * volume = 50*1 = 50 g content Mass = density * volume = 50*1= 50g mass (g) specific heat, c, (J gl °C!) 4.184 4.184 limiting reagent (yes/no) yes no initial temperature (°C) 22 c 21.3 c final temperature (°C) 28.1 c 19 c Acootent (J) Ion (J) calculated enthalpy of reaction AH1° AH, standard enthalpy J mmol-1 estigate
Transcribed Image Text:O Search (Alt+Q) erences Mailings Review View Help Table Design Layout Aa v A EE AL T O Fin Emphasis Heading 1 Heading 2 三。 E Rep A Sle Paragraph Styles Editi Table 1Report): Determination of the enthalpy of decomposition of ammonium chloride Reactions Part A Part B reagents HCl NH3(a9) NH,Cl) water volume (mL) 25 25 50ml molarity (M) 0.9776 1.30 mass of beaker + NH,CI (g) 31.622 mass of emptied beaker (g) 29.720 mass of NH,CI (g) 1.902 n (mmols) 0.0244 0.0325 0.036 volume (mL) 50 ml 50ml total calorimeter Density (g mL1) 1.00 1.00 Mass = density * volume = 50*1 = 50 g content Mass = density * volume = 50*1= 50g mass (g) specific heat, c, (J gl °C!) 4.184 4.184 limiting reagent (yes/no) yes no initial temperature (°C) 22 c 21.3 c final temperature (°C) 28.1 c 19 c Acootent (J) Ion (J) calculated enthalpy of reaction AH1° AH, standard enthalpy J mmol-1 estigate
O Search (Alt+Q) ces Mailings Review View Help Table Design Layout O Find - a v Emphasis Heading 1 Heading 2 E Replace A. 三。 A Select Paragraph Styles Editing calculated enthalpy of decomposition of NH.Cle), AH5, (kJ mol-)(as determined using the equation/answer to Q1 below) literature enthalpy of decomposition of NH.Clo), AHs, (kJ mol-1)(as determined in Q2 below) CHEM 1017 & CHEM 1987 Hess's Law Additional Questions 1. Express the enthalpy of decomposition of ammonium chloride, AH,, in terms of the four other enthalpies (AH1, AH2, AH3, AH4) described in the Introduction to this experiment. Use the examples in your textbook for help with Hess's Law. (Ex. AH, = AHỊ + 2AH2 - AH3 + AH4; this is NOT the answer; use this format). AH, = 2. List the enthalpies of formation for ammonium chloride (solid), ammonia (gas) and hydrogen chloride (gas) by referring to the appropriate appendix of your textbook. Compound Enthalpy of Formation (AH:) / kJ mol NH.Cl -314.4 NH3(2) -80.2 tigate
Transcribed Image Text:O Search (Alt+Q) ces Mailings Review View Help Table Design Layout O Find - a v Emphasis Heading 1 Heading 2 E Replace A. 三。 A Select Paragraph Styles Editing calculated enthalpy of decomposition of NH.Cle), AH5, (kJ mol-)(as determined using the equation/answer to Q1 below) literature enthalpy of decomposition of NH.Clo), AHs, (kJ mol-1)(as determined in Q2 below) CHEM 1017 & CHEM 1987 Hess's Law Additional Questions 1. Express the enthalpy of decomposition of ammonium chloride, AH,, in terms of the four other enthalpies (AH1, AH2, AH3, AH4) described in the Introduction to this experiment. Use the examples in your textbook for help with Hess's Law. (Ex. AH, = AHỊ + 2AH2 - AH3 + AH4; this is NOT the answer; use this format). AH, = 2. List the enthalpies of formation for ammonium chloride (solid), ammonia (gas) and hydrogen chloride (gas) by referring to the appropriate appendix of your textbook. Compound Enthalpy of Formation (AH:) / kJ mol NH.Cl -314.4 NH3(2) -80.2 tigate
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