In a chemical reaction old bonds are broken and new ones formed. Therefore reaction enthalpies can be predicted on the basis of the tabulated old and new bond strengths or estimated by using mean bond enthalpies. Account for the difference in the standard enthalpy of combustion of methane andmethanol vapour, -890 kJ mol-1 and -688 kJ mol-1 , respectively.

4. Number these in order of ease of hydrolysis. 1 = easiest to hydrolyze, 4 = hardest to hydrolyze. C.H.&CI C6H5CNHC(CH3)3 CH₂C=NCHCOCH

Classify the formation of methane from its elements in their reference states as exergonic or endergonic under standard conditions at 298 K.

Consider the following molecule. How many hydrogens are in this molecule? OH авдав -NH. NH 00000 H₂N. О 18 O 14 О 17 О 16 О 15 CH 3 OH

Measurements show that the energy of a mixture of gaseous reactants decreases by 175. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 79. kJ of work is done on the mixture during the reaction. Calculate the change in enthalpy of the gas mixture during the reaction. Be sure your answer has the correct number of significant digits. x10 exothermic Is the reaction exothermic or endothermic? endothermic

The hydrocarbons acetylene (C2H2) and benzene (C6H6)have the same empirical formula. Benzene is an “aromatic”hydrocarbon, one that is unusually stable because of its structure.(a) By using data in Appendix C, determine the standardenthalpy change for the reaction 3 C2H2(g)-----> C6H6(l).(b) Which has greater enthalpy, 3 mol of acetylene gas or1 mol of liquid benzene? (c) Determine the fuel value, inkJ/g, for acetylene and benzene.

A constant-volume calorimeter was calibrated by carrying out a reaction known to release 0.704 kJ of heat in 0.600 L of = -0.704 kJ), resulting in a temperature rise of 2.76 °C. In a subsequent experiment, 300.0 mL of 0.40 M HCI0, (aq) and 300.0 mL of 0.40 M NaOH(aq) were mixed in the same calorimeter and the temperature rose by solution in the calorimeter (q 5.90 °C. What is the change in the internal energy of the reaction mixture as a result of the neutralization reaction? AU= kJ TOOLS x10 Question Source: Atkins 7e - Chemical Principles| Publishe MacBook Pro +

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

Calculate 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 rxn

The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a value of zero to H* ions; that is, AH H* (aq)]=0. H₂O HC1 (g) →H (aq) + Cl¯ (aq) Note: Reference the Thermodynamic properties of pure substances table for additional information. Part 1 of 2 For the following reaction, calculate AH, for the CI ions. Round your answer to 4 significant digits. Part 2 of 2 □ 0x10 X □ 0.0 kJ ΔΗ% = -14.7 mol S Calculate the enthalpy of neutralization when 1 mole of a strong monoprotic acid (such as HCI) is titrated by 1 mole of a strong base (such as KOH) at 25 °C. Round your answer to 3 significant digits. 010