(a) Write the balanced chemical equation that represents the standard heat of formation of HgClh(s) at 298 K. Be sure to specify states. Write fractions with a slash, such as 1/2 for one half. If a box is not needed leave it blank. (b) The standard enthalpy change for the following reaction is 859 kJ at 298 K. BaCl2(s)→ Ba(s) + Cl½(g) What is the standard heat of formation of BaCl2(s)? kJ/mol Check & Submit Answer Show Approach

(a) Write the balanced chemical equation that represents the standard heat of formation of HgClh(s) at 298 K. Be sure to specify states. Write fractions with a slash, such as 1/2 for one half. If a box is not needed leave it blank. (b) The standard enthalpy change for the following reaction is 859 kJ at 298 K. BaCl2(s)→ Ba(s) + Cl½(g) What is the standard heat of formation of BaCl2(s)? kJ/mol Check & Submit Answer Show Approach

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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Ethylene glycol, HOCH2CH2OH, is used as antifreeze. It is produced from ethylene oxide, C2 H40, by the reaction C2 H4O(g) + H,0(1) HOCH, CH,OH(!) Use Hess's law to obtain the enthalpy change for this reaction from the following enthalpy changes: 2C, HO(g) + 502(9) → 4CO2 (9) + 4H,0(1) AH =-2612.2 kJ HOCH, CH, OH(1) + O2 (9) → 2002 (9) + 3H,0(1) AH=-1189.8 kJ Enthalpy change = kJ %3D
Using the table of standard formation enthalpies that you'll find under the ALEKS Data tab, calculate the reaction enthalpy of this reaction under standard conditions: 2C2H6 (g) + 7O2 (g) → 4CO2 (g) + 6H2O (l)Round your answer to the nearest kJ .
The standard heat of formation, AH, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have AH = 0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g) + O2(g) = 2NO₂(g) with heat of formation values given by the following table: Substance ΔΗ (kJ/mol) 90.2 0 33.2 NO(g) O₂(g) NO₂(g) Then the standard heat of reaction for the overall reaction is AH AH (products) AH; (reactants) [2(90.2) +0] = 2(33.2) = -114 kJ Part A For which of the following reactions is AHn equal to AH; of the product(s)? You do not need to look up any values to answer this question. Check all that apply. ► View Available Hint(s) Li(s) + Cl₂(g) →LiCl(s) SO(g) + O₂(g) →SO2(g) S(s) + O₂(g) →SO₂ (g) SO3(g) → O₂(g) + SO2(g) Li(s) + Cl₂(1)→LiCl(s) 2Li(s) + Cl₂ (g)→2LiCl(s) Submit Constants I Periodic Table Part B
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The table provides molar heat capacities (Cm) of selected metals with the units of joules per mole-kelvin. Heat capacity is also frequently given as specific heat capacity (C₂) with the units joules per gram-degree Celsius. Using the values provided in the table, convert the molar heat capacity (Cm) of zinc to the specific heat capacity (C₂) of zinc. C₁ = J/(g. °C) Molar heat capacity (Cm) of selected metals at 25 °C Element aluminum copper iron lead magnesium nickel titanium zinc Cm (J/(mol-K)) 24.20 24.44 25.10 26.84 24.87 26.07 25.06 25.39
Find the molar enthalpy of combustion in kJ/mol of glucose at some temperature and pressure C6H12O6 (s) + 6 O2 (g) → 6 CO2 (g) + 6 H2O (l) given that in an experiment under the same conditions the combustion of 0.108 g of glucose raised the temperature of a calorimeter with total heat capacity C= 1.155 kJ/°C by 1.31 °C. The molar mass of glucose is 180.1 g/mol. Ignore the heat absorbed by the combustion products; assume this is negligible, and all heat went into the calorimeter itself. Give the answer with 5 or more significant figures.
4) Consider the thermochemical equation below. What mass of HgO must decompose to consume 400.0 kJ of heat? 2 HgO (s) → 2 Hg (1)+ O2(g) AH°rxn =+ 181.4 kJ (1) 5) Write the standard formation reaction for KAI(SO4)2(s). (1) 3 CO2 (g). (1) -393.5 kJ/mol 2 Cr (s) + 3 CO (ag) -110.5 kJ/mol Cr2O3 (s) 6) Consider the reaction 0.0 kJ/mol AH°f = -1139.7 kJ/mol Calculate AH°rxn.
Using the standard enthalpies of formation, what is the standard enthalpy of reaction? CO(g) + H,O(g) –→ CO,(g) + H,(g) AHân = kJ
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(b) The standard enthalpy change for the following reaction is -697 kJ at 298 K.2 Zn(s) + O2(g)2 ZnO(s)What is the standard heat of formation of ZnO(s)
5.000 g of Compound X with molecular formula C,H, are burned in a constant-pressure calorimeter containing 20.00 kg of water at 25 °C. The temperature of the water is observed to rise by 2.556 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. ? olo :
Find the enthalpy change for this reaction using the data below. Clearly show how you got the answer. 2 Al(s) + 3 Cl2 (g) → 2 AlCl3 (s) Data: (a) 2 Al(s) + 6 HCl(aq) → 2 AlCl3 (aq) + 3 H2 (g) H = −1049 kJ (b) AlCl3 (s) → AlCl3 (aq) H = −323 kJ (c) H2 (g) + Cl2 (g) → 2 HCl(g) H = −185 kJ (d) HCl(aq) → HCl(g) H = +74.8 kJ