Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Textbook Question
Chapter 4, Problem 4.27E
Example
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How do you find the S value, and delta H value of a product (in a reaction) With given S, delta H, of the reactants of the reaction, and with given delta Grxn. Please write a formula.
Calculate Δ Hrxn for
Ca(s) + 1/2 O2(g) + CO2(g) → CaCO3(s)
given the following set of reactions:
Ca(s) + 1/2 O2(g) →CaO(s)
ΔH = −635.1 kJ
CaCO3(s) →CaO(s) + CO2(g)
ΔH = 178.3 kJ
Calculate
Δ
Hrxn for
Ca(s) + 1/2 O2(g) + CO2(g) → CaCO3(s)
given the following set of reactions:
Ca(s) + 1/2 O2(g) → CaO(s)
Δ
H = −635.1 kJ
CaCO3(s) →CaO(s) + CO2(g)
Δ
H = 178.3 kJ
Chapter 4 Solutions
Physical Chemistry
Ch. 4 - List the sets of conditions that allow dS, dU, and...Ch. 4 - Explain why conditions for using S>0 as a strict...Ch. 4 - Explain how the equation dU+pdVTdS0 is consistent...Ch. 4 - Explain why the spontaneity conditions given in...Ch. 4 - Prove that the adiabatic free expansion of an...Ch. 4 - Derive equation 4.6 from equation 4.5.Ch. 4 - Derive equation 4.8 from equation 4.7.Ch. 4 - The third part of equation 4.9 mentions a...Ch. 4 - Calculate A for a process in which 0.160mole of an...Ch. 4 - What is the maximum amount of non-pV work that can...
Ch. 4 - Consider a piston whose compression ratio is 10:1;...Ch. 4 - When one dives, water pressure increases by 1atm...Ch. 4 - Calculate G(25C) for this chemical reaction, which...Ch. 4 - Thermodynamic properties can also be determined...Ch. 4 - Calculate G in two different ways for the...Ch. 4 - Calculate G in two different ways for the...Ch. 4 - For the reaction C(graphite)C(diamond) at 25C,...Ch. 4 - Determine G for the following reaction at 0C and...Ch. 4 - What is the maximum amount of electrical that is,...Ch. 4 - When a person performs work, it is non-pV work....Ch. 4 - Can non-pV work be obtained from a process for...Ch. 4 - Can pV work be obtained from a process for which...Ch. 4 - Batteries are chemical systems that can be used to...Ch. 4 - The value of G for any phase change at constant p...Ch. 4 - The value of G for any phase change at constant p...Ch. 4 - Under what conditions is A=0 for a phase change?...Ch. 4 - Example 4.2 calculated A for one step of a Carnot...Ch. 4 - Can CV and Cp be easily defined using the natural...Ch. 4 - Analogous to equation 4.26, what is the expression...Ch. 4 - Prob. 4.30ECh. 4 - Prob. 4.31ECh. 4 - Prob. 4.32ECh. 4 - Although ideally, U=H=0 for a gas-phase process at...Ch. 4 - Use equations 4.21 and 4.25 to explain why H and G...Ch. 4 - Prob. 4.35ECh. 4 - Which of the following functions are exact...Ch. 4 - Prob. 4.37ECh. 4 - Prob. 4.38ECh. 4 - Prob. 4.39ECh. 4 - Equation 4.19 says that (UV)S=p If we are...Ch. 4 - For an isentropic process, what is the approximate...Ch. 4 - Use the ideal gas law to demonstrate the cyclic...Ch. 4 - Prob. 4.43ECh. 4 - Prob. 4.44ECh. 4 - Evaluate (U/V)T for an ideal gas. Use the...Ch. 4 - Evaluate (U/V)T for a van der Waals gas. Use the...Ch. 4 - Repeat the previous exercise for a gas that...Ch. 4 - Determine an expression for (p/S)T for an ideal...Ch. 4 - Determine the value of the derivative {[(G)]/T}p...Ch. 4 - Prob. 4.50ECh. 4 - Prob. 4.51ECh. 4 - A 0.988-mole sample of argon expands from 25.0L to...Ch. 4 - A 3.66-mol sample of He contracts from 15.5L to...Ch. 4 - Prob. 4.54ECh. 4 - Prob. 4.55ECh. 4 - Use the Gibbs-Helmholtz equation to demonstrate...Ch. 4 - For the equation 2H2(g)+O2(g)2H2O(g)...Ch. 4 - Use equation 4.46 as an example and find an...Ch. 4 - What is the value of G when 1.00mol of water at...Ch. 4 - Prob. 4.60ECh. 4 - Prob. 4.61ECh. 4 - Prob. 4.62ECh. 4 - Prob. 4.63ECh. 4 - Prob. 4.64ECh. 4 - What is the change in the chemical potential of a...Ch. 4 - Prob. 4.66ECh. 4 - Prob. 4.67ECh. 4 - Prob. 4.68ECh. 4 - Prob. 4.69ECh. 4 - Can equation 4.62 be used to calculate for an...Ch. 4 - Prob. 4.71ECh. 4 - Of helium and oxygen gases, which one do you...Ch. 4 - Prob. 4.73ECh. 4 - Use equation 4.39 to determine a numerical value...Ch. 4 - Prob. 4.75ECh. 4 - Prob. 4.76E
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Determine delta H* for the following thermochemical equation.Pb(s) + PbO2(s) + 2SO3(g) -> 2PbSO4(s)Given:Pb(s) + PbO2(s) + 2H2SO4(l) -> 2PbSO4(s) + 2H2O(l) deltaH* = -509.2 kJSO3(g) + H2O(l) -> H2SO4(l) deltaH* = -130. kJarrow_forwardWould the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.arrow_forward9.42 Why is enthalpy generally more useful than internal energy in the thermodynamics of real world systems?arrow_forward
- From the following enthalpies of reaction: H2 (g) +F2 (g) → 2HF (g) ∆H = −537 kJ C (s) + 2F2 (g) →CF4 (g) ∆H = −680 kJ 2C (s) + 2H2 (g) → C2H4 (g) ∆H = +52.3 kJ calculate ∆H for the reaction of ethylene with F2: C2H4 (g) + 6F2 (g) → 2CF4 (g) + 4HF (g)arrow_forwardSodium carbonate can be made by heating sodium bicarbonate: 2NaHCO3(s) ® Na2CO3(s) + CO2(g) + H2O(g) Given that DH° = 128.9 kJ/mol and DG° = 33.1 kJ/mol at 25°C, Calculate ΔSoarrow_forwardCalculate the heat of reaction deltaH for the following reaction: CH4(g) + 2O2(g)——>CO2(g)+ 2H2O(g) Round your answer to the nearest kJ/mol.arrow_forward
- From the following enthalpies of reaction: H2(g)+F2(g)→2HF(g),ΔH=−537kJ C(s)+2F2(g)→CF4(g),ΔH=−680kJ 2C(s)+2H2(g)→C2H4(g),ΔH=+52.3kJ calculate ΔH for the reaction of ethylene with F2: C2H4(g)+6F2(g)→2CF4(g)+4HF(g)arrow_forwardCalculate ΔH°rxn for the following reaction. 3N2H4(l) → 4NH3(g) + N2(g)given that ΔH°f[N2H4(l)] = 50.4 kJ/mol and ΔH°f[NH3(g)] = –46.3 kJ/mol. Group of answer choices –96.7 kJ +336.4 kJ +34.0 kJ –34.0 kJ –336.4 kJarrow_forwardMatch the state function to its corresponding heat of reaction: A: delta E B: delta H A: qv or qp? B: qv or qp?arrow_forward
- Substance D has the following properties: ΔHvap = 30.5 kJ/mol ΔHfus = 5.9 kJ/mol Tb = 89.4 °C Tm = -31.6 °C Specific Heat (solid) = 4.6 J/g·°C Specific Heat (liquid) = 2.7 J/g·°C Specific Heat (gas) = 1.5 J/g·°C Calculate the energy that must be removed to convert 107.6 g of substance D from a gas at 136.1 °C to a solid at -68.0°C. The molar mass of Substance D is 75 g/mol.arrow_forwardDetermine the heat of formation for C2H2. CaC2(s) + 2H2O(l) ---> C2H2(g) + Ca(OH)2(s) Delta H(rxn)= -128.9kJ Substances: CaC2(s)= S(1/mol*K)= 70.0 Delta H(f) (kJ/mol)= -59.8 H20(l)= S= 69.9 Delta H= -285.8 C2H2(g)= S= 200.8 Delta H= ? Ca(OH)2= S= 83.4 Delta H= -986.1arrow_forwardConsider the hypothetical thermochemical equation: 3 A + B ----> 2 C for which delta H = 62.1 kJ/mol. What would delta H, in kJ/mol, be for the reaction 2 C --> 3A + B?arrow_forward
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