Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entr AS. Vote: if you have not been given enough information to decide a sign, select the "unknown" option. reaction observations conclusions This reaction is always spontaneous, but proceeds faster at temperatures below AH is (pick one) v 132. °C. AS is (pick one) v AH is (pick one) ♥ This reaction is spontaneous except below 3. °C. B AS is (pick one) v This reaction is spontaneous only below AH is L(pick one) v 44. °C. AS is (pick one) ♥

Use the observations about each chemical reaction in the table below to decide the sign (positive or negative) of the reaction enthalpy AH and reaction entr AS. Vote: if you have not been given enough information to decide a sign, select the "unknown" option. reaction observations conclusions This reaction is always spontaneous, but proceeds faster at temperatures below AH is (pick one) v 132. °C. AS is (pick one) v AH is (pick one) ♥ This reaction is spontaneous except below 3. °C. B AS is (pick one) v This reaction is spontaneous only below AH is L(pick one) v 44. °C. AS is (pick one) ♥

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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MISSED THIS? Watch IWE: Standard Enthalpies of Formation; Read Section 7.9. You can click on the Review link to access the section in your eText. Consider the table of Standard Thermodynamic Quantities for Selected Substances at 25 °C. Substance AH; (kJ/mol) Substance AH; (kJ/mol) Substance AH; (kJ/mol) Al(g) HCl(aq) NF₂ (g) Al₂O₂ (s) Cr(g) NH:(E) F(g) C(g) CH₂(g) C₂H₂(g) C₂H₂(g) C₂H6(g) CO(g) CO₂ (g) Cl(g) HCl(g) 330.0 -1675.7 716.7 -74.6 227.4 52.4 -84.68 -110.5 -393.5 121.3 -92.3 HF(g) HF (aq) H(g) Fe(g) FeO(s) Fe₂O₂ (s) Fe₂O4(s) N(g) -167.2 396.6 79.38 -273.3 -335.0 218.0 416.3 -272.0 -824.2 -1118.4 472.7 NH3(aq) O(g) O₂(g) S(g) SO₂(g) SO3(g) Sn(g) SnO(s) SnO₂ (s) -132.1 -45.9 -80.29 249.2 142.7 277.2 -296.8 -395.7 301.2 -280.7 -577.6 Part A Enter an equation for the formation of HF(g) from its elements in their standard states. Express your answer as a chemical equation including phases. Part C ΑΣΦ 6 A chemical reaction does not occur for this question. Part B Complete previous…
5. The above reaction was performed again, but this time in a constant-pressure calorimeter attached to a frictionless piston. Over the course of the process, the total volume of the gaseous contents of the calorimeter decreased by 100.4 mL. If the pressure outside of the piston was 1.000 atm, determine AHoa for this process in kJ. Recall that 101.325 J=1 L atm.
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)
estion 30 of 41 <. Consider an ideal gas enclosed in a 1.00 L container at an internal pressure of 10.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 10.0 L. J w = Now calculate the work done if this process is carried out in two steps. 1. First, let the gas expand against a constant external pressure of 5.00 atm to a volume of 2.00 L. 2. From the end point of step 1, let the gas expand to 10.0 L against a constant external pressure of 1.00 atm. J w = とTOOLS x10 Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry| Publisher: University Science Books A étv Aa w MacBook Air DD
A mole of sodium met is added to water How much work is done on the atmosphere by the subsequent reaction if the temperature is 25 C°
1,2,3 please
Calculate AH°rxn_in kJ/mol for the reaction below. Look up the values for AHF° below. 4 NH3 (g) + 5 02 (g) → 4 NO (g) + 6 H20 (g) Table 6.3 Standard Enthalpies of Formation of Some Inorganic Substances at 25°C Substance AH; (kJ/mol) Substance AH? (kJ/mol) Ag(s) AgCl(s) Al(s) H,O;(/) - 187.6 Hg(/) 2(s) HI(g) Mg(s) MgO(s) M9CO (s) N2(g) NH3(G) NO(g) - 127.04 Al;03(s) - 1669.8 25.94 Br2(1) HBr(g) -36.2 -601.8 C(graphite) C(diamond) -1112.9 1.90 Co(g) -110.5 -46.3 CO2(g) Ca(s) - 393.5 90.4 NO,(g) N204(g) N20(g) O(g) 0,(g) 33.85 CaO(s) -635.6 9.66 CaCO;(s) Cl2G) - 1206.9 81.56 249.4 -92.3 HCIG) Cu(s) 03(g) S(rhombic) 142.2 CuO(s) - 155.2 F2(g) HF(g) H(g) S(monoclinic) 0.30 SO-(g) So:(g) H,S(g) -268.61 -296.1 218.2 - 395.2 H2(g) H2O(g) -20.15 -241.8 Zno(s) -347.98 H2O(I) -285.8
18. Calculate the heat of reaction at constant volume for 5.00 g C3H8 ,considering the following chemical reaction: C3H8 (g) + O2(g) --------------------> CO2 (g) + H2O (g) heat of standard formation: O2 = 0.00 kJ / mole, H2O (g) = -245 kJ / mole, CO2 = -318 kJ/mole and C3H8 = -438 kJ / mole C3H8 = 44.09 g/mole Temperature is 33 oC a. -789 kJ b. -212 kJ c. 412 kJ d. -169 kJ
Calculate AH°rxn in kJ/mol for the reaction below. Look up the values for AHº below. SO2 (g) + ½ O2 (g) – SO3 (g) Table 6.3 Standard Enthalpies of Formation of Some Inorganic Substances at 25°C Substance AH; (kJ/mol) Substance AH; (kJ/mol) Ag(s) AgCl(s) H,O2(/) - 187.6 - 127.04 Hg(/) 1(5) Al(s) Al203(s) - 1669.8 HI(g) 25.94 Br2(/) HBr(g) C(graphite) Mg(s) - 36.2 MgO(s) MgCO3(s) N2(g) NH3(g) NO(g) NO,(g) N,O4(g) -601.8 -1112.9 C(diamond) 1.90 CO(g) CO2(g) -110.5 -46.3 -393.5 90.4 Ca(s) 33.85 CaO(s) -635.6 9.66 CacO;(s) - 1206.9 N20(g) 81.56 Cl2(g) HCI(g) Cu(s) CuO(s) O(g) O2(g) O3(g) 249.4 -92.3 142.2 - 155.2 S(rhombic) F2(g) HF(g) S(monoclinic) 0.30 -268.61 SO2(g) SO;(g) H2S(g) -296.1 H(g) H2(g) 218.2 -395.2 -20.15 -347.98 H,O(g) H2O(I) -241.8 ZnO(s) -285.8
25°C 32°C bum wohl 891 10 228 1. Two aqueous reactants are mixed in a flask with a balloon over the top and the following change is observed. What are the signs on q and w for the system? Enter >, <, or in each box below. W 0 2. You drop a piece of potassium metal into water and the following exothermic reaction occurs: 2 K(s) + 2 H₂O(l) → 2 KOH(aq) + H₂(g) What are the signs on q and w for this reaction, at constant temperature and pressure? A) q is positive and w is negative. B) q is negative and w is positive. C) q and w are both negative. D) q and w are both positive. E) There is not enough information given. 3. What is the change in internal energy when one mole of helium gas in a flexible-walled container at STP is heated to 100°C? (CHe(g) = 5.30 J/g°C) AU =
Calculate G for the reaction of iron (III) oxide with carbon monoxide to give elemental iron and carbon dioxide. í G₁ (kJ/mol) Fe(s) 0 CO₂(g) -394.4 Fe₂O3(s) -741.0 CO(g) -137.3