Determine if the formation of acid rain is a spontaneous reaction at 50°C Chemical Equation: NO2 + H2O → HNO2 + HNO3 1. Compute for the AG of the equation: Compound NO₂ H₂O HNO2 HNO3 184.48 kJ/mol (round off to 2 decimal places) AH° (kJ/mol) 33.85 -285.8 -118.8 -173.2 AS° (J/K mol) 240.46 69.9 254.1 155.6

Determine if the formation of acid rain is a spontaneous reaction at 50°C Chemical Equation: NO2 + H2O → HNO2 + HNO3 1. Compute for the AG of the equation: Compound NO₂ H₂O HNO2 HNO3 184.48 kJ/mol (round off to 2 decimal places) AH° (kJ/mol) 33.85 -285.8 -118.8 -173.2 AS° (J/K mol) 240.46 69.9 254.1 155.6

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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Be sure to answer all parts. For the gaseous reaction of carbon monoxide and chlorine to form phosgene (COC1₂), perform the following calculations. (a) Calculate the ASº at 298 K (AH = -220. kJ/mol and AG =-206 kJ/mol). kJ/mol·K (b) Assuming that AS and AH change little with temperature, calculate AG at 450. K. kJ/mol
Consider the reaction 2NO2 (9) = N204(9) For each of the following mixtures of reactants and products at 25°C, predict the direction in which the reaction will shift to reach equilibrium. AG F(NO:(9)) = 52 kJ/mol AGN0.(0)) = 98 kJ/mol PNO, = PN,0, = 1.0 atm a. PNo, = 0.21 atm, PN,o, = 0.50 atm b. PNO2 0.21 atm, PN,04 0.84 atm с.
Use the information provided to determine AH°rxn for the following reaction: -> CH4(g) + 4 Cl2(g) → CCl4(g) + 4 HCl(g) AH°rxn = ? AHof (kJ/mol) CH4(g) -75 CCl4(g) -96 HCl(g) -92 O A.-71 kJ O B.-389 kJ OC. +79 kJ O D. +113 kJ O E.-113 kJ
For the reaction H,(g) + F2(g) →2 HF(g) AG°=-547.0 kJ and AS° = 14.1 J/K at 338 K and1 atm. This reaction is (reactant, product) favored under standard conditions at 338 K. The standard enthalpy change for the reaction of 2.33 moles of H2(g) at this temperature would be kJ.
The molar enthalpy change for the neutralization reaction: HCl(aq)+NaOH(aq)⟶NaCl(aq)+H2O(l) is ΔrH° = -57.3 kJ/mol. Imagine you mix 60.7 mL of 1.00 M HCl with 75.9 mL of 1.00 M NaOH in a beaker at 24.1 °C. Calculate the final temperature of the solution after the reaction has gone to completion. You will need to assume no heat is lost to the environment, the density of the reaction solution is the same as water, 1.00 g/mL, and the specific heat capacity of the reaction solution is the same as of water, 4.184 J/g°C. Final temperature (°C)?
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