When a neutralization reaction was carried out using 100.0 mL of 0.7890M NH3 water and 100.0 mL of 0.7940M acetic acid, ΔT was found to be 4.76 °C. The specific heat of the reaction mixture was 4.104 J g-l K-1 and its density was 1.03 g mL-1. The calorimeter constant was 3.36 JK-1 a) Calculate ΔH neutralization for the reaction of NH3 and acetic acid.

a) Describe in your own words the relationship between standard change in Gibbs free energy associated with a chemical process (∆?o) and an equilibrium constant, Keq.    A ∆?o of –3.8 kJ/mol is associated with the equilibrium 2A+B⇌C+D. If A and B are initially present in 1M concentration, find the equilibrium concentrations of all species.   You know this reaction to be spontaneous at all temperatures, what can you deduce about the signs of the changes in enthalpy and entropy associated with this process? Why?

When a neutralization reaction was carried out using 100.0 mL of 0.7890M NH3 water and 100.0 mL of 0.7940M acetic acid, ΔT was found to be 4.76 °C. The specific heat of the reaction mixture was 4.104 J g-l K-1 and its density was 1.03 g mL-1. The calorimeter constant was 3.36 JK-1 a) Calculate ΔH neutralization for the reaction of NH3 and acetic acid. b) At the end of the experiment, it was discovered that the thermometer had not been calibrated. When it was calibrated, it was found that the thermometer read 0.50 °C low. What effect would this thermometer reading have on the reported DH neutralization calculated above? c) When the temperature-time data graph was reviewed, it was found that an error had been made in determining ΔT. Instead of 4.76 °C, ΔT was actually 4.70 °C. Based on this change only, calculate the correct ΔH neutralization for the reaction of NH3, and acetic acid. d) Calculate the percent error for the correct ΔH neutralization if aΔ DT of 4.76 °C had been used.…

Here are some relevant excerpts from the tables of standard thermodynamic data: Substance    ΔHfo(kJ/mol) H2O (l)     -286 NO (g)        90 NO2 (g)       34 HNO3 (aq)   -207 NH3 (g)       -46 Find ΔHo in kJ of 4NH3(g) + 5 O2 (g) --> 4 NO (g) + 6 H2O (l)   Question 15 options:   -1540 kJ   -1172 kJ   -1892 kJ   -150 kJ

Do not give handwriting solution. Calculate the entropy change, ΔS, for the following processes. If needed, Cp(O2)= 29.4 J mol-1 K-1 and Cp(CO2) = 37.1 J mol-1 K-1.(a) The pressure of one mole of O2(g) is increased from P to 2P at 298 K.(b) The temperature of one mole of CO2(g) is increased from 298 K to 355 K at aconstant volume of 20.0 L.

What is ΔHrxn if mixing 50.0 mL of 0.500 M HCl (aq) with 50.0 mL of 0.500 M NaOH (aq), both initially at 24.0 °C results in a Tmix of 27.3 °C?  Assume that the reaction goes 100%  HCl (aq) + NaOH (aq) → H2O (l) + NaCl(aq) **answer in kJ/mol of H2O produced

From the enthalpies of reaction 2C(s) + O2 (9) → 2C0(g) 2C(s) + O2 (9) + 4H2 (g) → 2CH3 OH(g) AH ΔΗ :-221.0kJ %3| :-402.4kJ calculate AH for the reaction CO(g) + 2H2 (g) → CH3 OH(g) Express your answer to three significant figures with the appropriate units.

MISSED THIS? Read Section 19.8 (Pages 871-877); Watch IWE 19.6. Liquid methanol burns in oxygen to form gaseous carbon dioxide and gaseous water. Substance H (kJ/mol) S° (J/(mol · K)) CH, OH (1) -238.6 126.8 O₂(g) 0 205.2 CO₂(g) -393.5 213.8 CO2(aq) -413.8 117.6 H₂O(g) -241.8 188.8 H₂O(1) -187.8 70.0 ▼ Part D where no represents the stoichiometric coefficients of the products, n, represents the st of the reactants, and Sº represents the standard entropies. AGxn= Calculate AG at 25°C. Express your answer in kilojoules to three significant figures. Submit = Provide Feedback 15] ΑΣΦ Request Answer Part E Complete previous part(s) [2(S° co₂(g)) + 4(S° H₂O(g))]- [2(S° CH₂OH()) + 3(S° 0₂(E [2(213.8 J/K)+4(188.8 J/K)] - [2(126.8 J/K) + 3(2 314 J/K MacBook Pro P Pearson ? kJ Copyright © 2023 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions Contac

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N, (g) + 3 H, (g) 2 NH,(g) the standard change in Gibbs free energy is AG° = -32.8 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN, = 0.500 atm, Pi, = 0.100 atm, and PNH, = 0.600 atm? AG = kJ/mol

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N₂(g) + 3 H₂(g) ⇒ 2NH₂(g) the standard change in Gibbs free energy is AG° = −32.8 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN₂ = 0.100 atm, PH₂ = 0.100 atm, and PNH₂ = 0.750 atm? AG = 737 kJ/mol