What does a negative ÄGròn tell you about the reaction? The reaction is absorbing heat from the surroundings The system is becoming more disordered. © The reaction is nonspontaneous at that temperature. The reaction is transferring heat to the surroundings The reaction is spontaneous at that temperature. The system is becoming less disordered.

What does a negative ÄGròn tell you about the reaction? The reaction is absorbing heat from the surroundings The system is becoming more disordered. © The reaction is nonspontaneous at that temperature. The reaction is transferring heat to the surroundings The reaction is spontaneous at that temperature. The system is becoming less disordered.

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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Use the reaction for the formation of NH3 from its elements N2(g) and H2(g) . This reaction has the following thermodynamic data: ΔfHo (NH3) = - 45.9 kJ/mol and ΔfSo (NH3) = - 99.1 J/mol*K at 298 K a) Write a balanced equation (whole number ratios) for this process and write out the expression for the reaction quotient Q using partial pressures. b) Without doing any calculations, explain how the progression of the reaction will change (more reactants or more products) with respect to 1) increasing temperature, and 2) increasing pressure. c) Calculate the equilibrium constant K at 298 K d) Assuming that : ΔfHo is independent of temperature, calculate K at - 78o C
Without doing any calculations, match the following thermodynamic properties with their appropriate numerical sign for the following exothermic reaction. C,H4(g) + H20(g) →CH3CH,OH(g) Clear All > 0 AHrxn 0 low T, 0 high T Previous Next
Consider the following reactions at 298 K. 2 03(g) → 3 O₂(g) O₂(g) → 2 0(g) NO(g) + O3(g) → NO₂(g) + O₂(g) ΔΗΘ Aat H ᎪᎻᎾ = -427.0 kJ/mol = 495.0 kJ/mol = -199.0 kJ/mol Apply Hess's law to calculate the standard reaction enthalpy for the reaction NO(g) + O(g) → NO₂(g)
One mole of an ideal gas is contained in a cylinder with a movable piston. The temperature is constant at 78°C. Weights are removed suddenly from the piston to give the following sequence of three pressures. a. P₁ b. P2 c. P3 = 5.20 atm (initial state) = 2.53 atm = 1.00 atm (final state) What is the total work (in joules) in going from the initial to the final state by way of the preceding two steps? J What would be the total work if the process were carried out reversibly? J
1.) Complete A and B to move on. a.) Write the complete, balanced chemical equation for the following reaction on a separate sheet of paper. Provide products where they are not given. Assume that the reaction is spontaneous. Propane (C3H8) + oxygen → carbon dioxide + water Type the sum of the coefficients in the equation into the answer blank. If there is no coefficient, count it as one. Include ( g, s, l, or aq) b.) Write the complete, balanced chemical equation for the following reaction on a separate sheet of paper. Provide products where they are not given. Assume that the reaction is spontaneous. Diphosphorus pentoxide + water → Type in the coefficient and formula for the product in the equation that contains phosphorus. Include ( g, s, l, or aq)
Using the following information, calculate the ΔH∘rsn Δ H r s n ° for the reaction between ammonia gas and oxygen. 4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (l). NH3 -45.9 kJ/mol O2 0.0 kJ/mol NO 90.3 kJ/mol H2O -285.8 kJ/mol
13. Energy is stored in the body in adenosine triphosphate, ATP, which is formed by reaction between adenosine diphosphate, ADP, and dihydrogen phosphate ions. ADP3-(aq) + H2PO42-(aq) -----> ATP4-(aq) + H2O (l) ΔH° = 38 kJ Is the reaction endothermic or exothermic?
Which one of the following reactions cannot proceed spontaneously as written at any temperature? Assume that ΔH°rxn does not depend on temperature. A. 2Cl2O(g) → 2Cl2(g) + O2(g) ΔH°rxn = –151 kJ B. 3O2(g) → 2O3(g) ΔH°rxn = +284 kJ C. COCl2(g) → CO(g) + Cl2(g) ΔH°rxn = +112 kJ D. 2C(s) + 2S(s) + O2(g) → 2COS(g) ΔH°rxn = –137 kJ E. N2O4(g) → 2NO2(g) ΔH°rxn = +171 kJ
Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Standard Gibbs free energy of formation values can be found in this table. 3 NO₂(g) + H₂O(1) – 2 HNO3 (1)+NO(g) -52.83 kJ/mol AGTxn Incorrect
Consider the reaction. 2Fe2O3⟶4Fe+3O2Δ?∘rxn=+824.2 kJ2Fe2O3⟶4Fe+3O2ΔHrxn°=+824.2 kJ The formation of 75.0 g75.0 g of O2 results in the absorption of 1930 kJ1930 kJ of heat. the absorption of 20600 kJ20600 kJ of heat. the release of 20600 kJ20600 kJ of heat. the release of 644 kJ644 kJ of heat. the release of 1930 kJ1930 kJ of heat. the absorption of 644 kJ644 kJ of heat.
Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change During an endothermic chemical reaction, four moles of gaseous reactants are turned into two moles of gaseous products. A solid precipitates from a solution, releasing heat as it does so. A solid absorbs heat and turns to a gas. Is this change spontaneous? Yes. O No. O Can't decide with information given. O Yes. O No. O Can't decide with information given. O Yes. O No. O Can't decide with information given.
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. 2CH3OH(g)+3O2(g)----> 2CO2(g)+4H2O(g)