1. Calculate the AHrxn for the reaction, Sn (s) + Cl2 (g) → SnCl2 (s) AHrxn = ? Sn (s) + Cl2 (g) → SnCl2 (s) Eq.1 Sn (s) + 2CI2 (g) → SnCl4 (1); AH = - 545.2 kJ Eq.2 SnC12 (s) + C12 (g) → SnCla (1); AH = – 195.4 kJ Eq.3 2. Calculate for the enthalpy of the following reaction between dinitrogen tetroxide, N204, and liquid hydrazine, N2H4, used to fuel small rockets. The balanced equation for the reaction is, N2O4(g) + 2 N2H4(1) → 3N2(g) + 4H2(g) AHf values: N2O4 (g) = +9.2 kJ/mol H20(g) = -238.9 kJ/mol N2H4(g) = 50.6 kJ/mol N2(g) = 0

1. Calculate the AHrxn for the reaction, Sn (s) + Cl2 (g) → SnCl2 (s) AHrxn = ? Sn (s) + Cl2 (g) → SnCl2 (s) Eq.1 Sn (s) + 2CI2 (g) → SnCl4 (1); AH = - 545.2 kJ Eq.2 SnC12 (s) + C12 (g) → SnCla (1); AH = – 195.4 kJ Eq.3 2. Calculate for the enthalpy of the following reaction between dinitrogen tetroxide, N204, and liquid hydrazine, N2H4, used to fuel small rockets. The balanced equation for the reaction is, N2O4(g) + 2 N2H4(1) → 3N2(g) + 4H2(g) AHf values: N2O4 (g) = +9.2 kJ/mol H20(g) = -238.9 kJ/mol N2H4(g) = 50.6 kJ/mol N2(g) = 0

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...

See similar textbooks

Similar questions

A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 72.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. AH = 76. kJ AS = 220. K 2NOCI(g) → 2NO (g) + Cl, (g) O kJ AG = Which is spontaneous? this reaction the reverse reaction neither
Example: At 25°C, calculate the AG° N₂+ 3H2 → 2NH3 • AG° N2(g) = 0 kJ/mol f • AG + H2(g) = 0 kJ/mol f • AG˚ NH 3(g) = -16.66 kJ/mol f a) 12.9 kJ b) -33.3 kJ c) -16.7 kJ d) -8.33 kJ e) Unsure sys for: AG sys =ΣnpG˚ products - Σn,G° reactants 60
From the AE given for 25 °C, calculate AH at the same temperature for the reaction: 2 NO2 (g) → 2 NO (g) + O2(g) -159.14 kJ O-166.58 kJ O-173.62 kJ O-164.10 kJ O-161.62 kJ AE-166.58 kJ
A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 142.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 2NO(g) → N₂(g) + O₂(g) AH = -181. kJ AS = -436. AG = | KJ J K Which is spontaneous? this reaction the reverse reaction neither X Ś
Write the net ionic equation for this neutralization reaction, including the states of matter (-e., H*(aq)) for the reactants and products. 4. Given the following data: 2C,H,(g) + 70,(g) → 4CO,(g) + 6H,0(1) AH = -3120 kJ %3D 2H,0(1) → 2H,(g) + O,(g) AH = +572 kJ %3D (8)'O C,H,(g) + 2H,(g) → C,H,(g) AH = -312 kJ Find the AH of the following reaction: 4CO,(g) + 2H,O(1) → 2C,H,(g) + 50,(g)
G.167.
Calculate the AH°, AS°, and AG° at 298 K for the following reaction: (Use the values found in Thermodynamic Properties to calculate your answers for questions a and b.) Al2O3(s) + 3 C(graphite) + 3 Cl₂(g) → 2 AICI3(s) + 3 CO(g) a) ΔΗο 400-64 kJ/mol b) AS° J/K.mol c) AGO 4.0 ✔ kJ/mol (Determine from the temperature, AH and AS) (d) Is the reaction extensive at standard conditions and 298 K? O Yes O NO 4.0 76.9 -89 (e) Write the expression for K. (Format example: Kp = pHC1² / pH₂. pCl2 would be entered as K_{p} = pHCI^{2}/pH_{2} . pCl_{2}.) Help chemPad X₁X (PCO)³ (pCl₂)3 Greek (PCO)^3/(pCl_2)^3 Your answer provides a different type of equation than was expected. (f) Calculate the value of K at 298 K 2.51e-16 X (Please answer to 3 significant figures.) (g) Estimate the value of K at 600 K. 1 79e-8 Ty (Please answer to 3 significant figures)
# H₂O(1) H*(aq) + OH(aq) Calculate the pOH of a 0.0100 M HCl solution at 50.0 °C. AH = -55.8 kJ; K=1.0 x 10-¹4 (at 25.0 °C)
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. Mg(OH), (s) + 2 HCI(g) → MgCl, (s) + 2 H,O(g) AHixn kJ
Determine ΔG°rxn for the following reaction: N2O (g) + NO2 (g) à 3 NO (g)ΔG° = ? Use the following reaction with known ΔG° values. Rxn 1:2 NO (g) + O2 (g) à 2 NO2 (g)ΔG1° = - 71.2 kJ Rxn 2:N2 (g) + O2 (g) à 2 NO (g)ΔG2° = + 175.2kJ Rxn 3:2 N2O (g) à 2 N2 (g) + O2 (g) ΔG3° = - 207.4kJ
Give detailed Solution with explanation needed
365 Calculate the standard free energy change for the following reaction: = Drive 2XO(s)+O2(g)→ 2XO2(s) AG 298(XO2) = -219.1 AG 298 (XO) = -150 Use 4 significant figures in your answer. Do not include the unit.