Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- The thermodynamic values from part A will be useful as you work through part B: ΔH∘rxn 243.5kJ/mol ΔS∘rxn 172.0J/(mol⋅K) Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C BaCO3(s)→BaO(s)+CO2(g)arrow_forwardA chemist measures the enthalpy change AH during the following reaction: 2 Al(OH),(s)→Al,03(s) + 3 H,0(1) ΔΗ-41. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol, reaction ΔΗ 4AI(OH), (3) → 2Al,0;(s) + 6H,0(1) 82 kJ Al,0, (;) + 3H,0(1) → 2A1(OH), (s) -41 kJ Al,0, () + H,0() -- AI(OH), (-)arrow_forwardGiven the reactions, X(s) + ¿0,(g) – XO(s) AH = -527.1 kJ XCO,(s) → XO(s) + CO,(g) ΔΗ +261.3 kJ what is AH for this reaction? X(s) + ¿0,(g) + CO,(g) XCO,(s) ΔΗ- kJarrow_forward
- Calculate AGºrxn for the reaction: BaCO3(s)→BaO(s)+CO₂(g) Use the following reactions and given AGºrxn values: Ba(s)+CO₂(g)+1/2O2(g) →BaCO3(s) AG°rxn=-1134.4kJ 2Ba(s)+O₂(g)→2BaO(s), AGºrxn=-520.3kJ BaCO3(s)→BaO(s)+CO₂(g). AGºrxn =arrow_forwardA student dissolves 11.0 g of ammonium chloride (NH, CI) in 200. g of water in a well-insulated open cup. He then observes the temperature of the water fall from 20.0 °C to 16.8 °C over the course of 6 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH,CI(s) NH (aq) + Cl (aq) db You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the known and published values for this reaction. O exothermic Is this reaction exothermic, endothermic, or neither? O endothermic O neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. kJ kJ…arrow_forwardCalculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation values can be found in this list of thermodynamic properties. C;H¿(g) + 50,(g) → 3 CO,(g) + 4 H,O(g) ΔΗ kJ rxnarrow_forward
- Consider the unbalanced equation for the neutralization of acetic acid: αHC2H3O2(aq)+βBa(OH)2(aq) →γH2O(l)+δBa(C2H3O2)2(aq) Balance the equation. Give your answer as an ordered set of numbers α, β, γ, δ. Your answers should reflect the lowest whole-number ratio of coefficients.arrow_forwardA chemist measures the enthalpy change AH during the following reaction: 4 Fe(s) + 3 02(g)→2 Fe,O3(s) AH =-320. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mol. reaction ΔΗ x10 Fe(s) + 0,6) - Fe,0,(1) O kJ 2Fe,0; (s) – 4Fe(s) + 30, (3) O kJ 4Fe,0, (s) - 8Fe(s) + 60, (3)arrow_forwardThe thermodynamic values from part A will be useful as you work through part B: ΔH∘rxn 243.5kJ/mol ΔS∘rxn 172.0J/(mol⋅K) Calculate the equilibrium constant for the following reaction at room temperature, 25 ∘C BaCO3(s)→BaO(s)+CO2(g)arrow_forward
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