Question

Calculate ΔS°(system), ΔS°(surroundings), and ΔS°(universe) for the following process at 298 K: HNO3(g) → HNO3(aq) HNO3(g)...

Calculate ΔS°(system), ΔS°(surroundings), and ΔS°(universe) for the following process at 298 K:

HNO3(g) → HNO3(aq)

HNO3(g) HNO3(aq)
S°, J/K 266.38 146.4
ΔfH°, kJ/mol -135.06 -207.36

ΔS°(system) =  J/K∙mol

ΔS°(surroundings) =  J/K∙mol

ΔS°(universe) =  J/K∙mol

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Calculate ΔS°(universe) for the decomposition of 1 mol of liquid water to form gaseous hydrogen and...
Calculate ΔS°(universe) for the decomposition of 1 mol of liquid water to form gaseous hydrogen and oxygen at 25 °C. S° (J/K · mol) ΔfH° (kJ/mol) O2(g) 205.07 0 H2(g) 130.7 0 H2O(ℓ) 69.95 -285.83 P4(s, white) 41.1 0 PH3(g) 210.24 5.47 N2(g) 191.56 0 NH3(g) 192.77 -45.90 Cl2(g) 223.08 0 HCl(g) 186.2 -92.31 CO2(g) 213.74 -393.509 C(s, graphite) 0 5.6
A.Calculate ΔS°(universe) for the decomposition of 1 mol of gaseous phosphine (PH3) to form white phosphorus...
A.Calculate ΔS°(universe) for the decomposition of 1 mol of gaseous phosphine (PH3) to form white phosphorus and gaseous S° (J/K · mol .) . ΔfH° (kJ/mol) O2(g) 205.07 0 H2(g) 130.7 0 H2O(ℓ) 69.95    -285.83 P4(s, white) 41.1 0 PH3(g)210.24 5.47 N2(g)191.56 0 NH3(g)192.77 -45.90 Cl2(g)223.08 0 HCl(g)186.2 -92.31 CO2(g)213.74 -393.509 C(s, graphite)0 5.6 ΔS°(universe) = J/K B.Determine whether the decomposition of gaseous phosphine (PH3) to form white phosphorus and gaseous hydrogen is spontaneous at 25 °C.
If the temperature of the surroundings is -244.32 °C, calculate the entropy change (in J/K) for...
If the temperature of the surroundings is -244.32 °C, calculate the entropy change (in J/K) for the system (ΔSsys), surroundings (ΔSsur) and universe (ΔSuniverse) when 40.4 g of liquid oxygen (O2) freezes. Report your answers to two decimal places. Tfus(°C) -218.79 Tvap(°C) -182.96 ΔH°fus (kJ/mol) 0.44 ΔH°vap (kJ/mol) 6.82
If the temperature of the surroundings is 38.36 °C, calculate the entropy change (in J/K) for...
If the temperature of the surroundings is 38.36 °C, calculate the entropy change (in J/K) for the system (ΔSsys), surroundings (ΔSsur) and universe (ΔSuniverse) when 48.1 g of gaseous carbon tetrachloride (CCl4) condenses. Report your answers to two decimal places. Tfus(°C) -23.00 Tvap(°C) 76.80 ΔH°fus (kJ/mol) 3.28 ΔH°vap (kJ/mol) 29.82
Given the following data, calculate, ΔH rxn, ΔS rxn, and Δ rxn, at 25° C for...
Given the following data, calculate, ΔH rxn, ΔS rxn, and Δ rxn, at 25° C for the equilibrium describe by the chemical equation. What direction is the spontaneity of this system? Mg (s) +HCl (aq) <---> H2 (g) + MgCl2 (aq) Mg(s) HCl(aq) H2 (g) MgCl2(aq) ΔH°f (Kj/mol) 0 -167.2 0 -801.3 S°(J/(mol K) 130.7 56.5 32.7 -24.0
If the temperature of the surroundings is 5.45 °C, calculate the entropy change (in J/K) for...
If the temperature of the surroundings is 5.45 °C, calculate the entropy change (in J/K) for the system (ΔSsys), surroundings (ΔSsur) and universe (ΔSuniverse) when 33.6 g of gaseous diethyl ether (C4H10O) condenses. Report your answers to two decimal places. Tfus(°C) -116.30 Tvap(°C) 34.50 ΔH°fus (kJ/mol) 7.27 ΔH°vap (kJ/mol) 26.52 i need these : 1- ΔSsys = 2- ΔSsur = 3 -ΔSuniverse =
Consider the reaction: Ca(s) + 2 H2O(ℓ) → Ca(OH)2(aq) + 2H2(g) ΔfH°(kJ/mol) 0 -285.83 -1002.82 0...
Consider the reaction: Ca(s) + 2 H2O(ℓ) → Ca(OH)2(aq) + 2H2(g) ΔfH°(kJ/mol) 0 -285.83 -1002.82 0 S°(J/K·mol) 41.59 69.95 -74.5 130.7 What are the values of ΔH°, ΔS° and ΔG° ΔH° =   kJ/mol ΔS° =   J/mol·K ΔG° =   kJ/mol
Ammonia is formed by the Haber process according to the following reaction: N2(g) + 3H2(g) ⇌...
Ammonia is formed by the Haber process according to the following reaction: N2(g) + 3H2(g) ⇌ 2NH3(g) Use the following data table to answer the questions below: Substance: ΔHf (kJ/mol) So (J/(mol*K) N2(g) 0    187.4 H2(g) 0 127.1 NH3(g) -47.3 197.6 Part 1: Using the table in the introduction, calculate the value of ΔH in units of kJ/mol. After, calculate the value of ΔS in units of J/(mol*K). Finally, cCalculate the value of ΔG in units of kJ/mol for...
Diamond a. At 298 K, what is the Gibbs free energy change G for the following...
Diamond a. At 298 K, what is the Gibbs free energy change G for the following reaction? Cgraphite ->  Cdiamond b. Is the diamond thermodynamically stable relative to graphite at 298 K? c. What is the change of Gibbs free energy of diamond when it is compressed isothermally from 1 atm to 1000 atm at 298 K? d. Assuming that graphite and diamond are incompressible, calculate the pressure at which the two exist in equilibrium at 298 K. e....
Determine ΔS°rxn and ΔG°rxn at 298 K for each of the following reactions, and determine if...
Determine ΔS°rxn and ΔG°rxn at 298 K for each of the following reactions, and determine if it is spontaneous under these conditions. a. Ca( s ) + Cl2 ( g ) produces CaCl2 ( s ) b. 2C2H6 ( g ) + 7O2 ( g ) produces 4CO2 ( g ) + 6H2O( l ) c. SrCl2 ( s ) produces Sr (2+) ( aq ) + 2Cl (1–) ( aq )
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT