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Practice ProblemATTEMPT
The reaction of carbon dioxide and calcium hydroxide to produce calcium carbonate and water is represented by the equation
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Chemistry
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- What is ΔH, ΔS and ΔG° at 1000 °C for the following reaction? CaCO3 (s) = CaO (s) + CO2 (g) ΔHf° (KJ) S° (J/K CaCO3 -1206.9 92.9 CaO -635.1 38.2 CO2 -393.5 213.7 ΔHAnswerKJ ΔSAnswerJ/K ΔGoAnswerKJ (b) Is the reaction spontaneous at 1000 °C and 1 atm? Answer (c) What is the value of Kp at 1000 °C for this reaction given that (R = 8.314 J/K mol) KpAnswer (d) What is the partial pressure of CO2 (g)?Answeratmarrow_forwardCalculate T in Kelvin given:K= 7.61×10^−6ΔG^0cell=206kJ/molR= 8.314 J/mol KΔG^0cell=−RTlnK a) 526 b) 2,100 c) 701 d) 1,050 e) 420arrow_forward4,At constant pressure, the sign of q for the process C3H8(g) => C3H8(l) is____, because______ Group of answer choices A, positive, the process is exothermic B, no correct answer C, negative, the process is endothermic D, negative, the process is exothermic E, positive, the process is endothermic 5,If 9.00 mol of hydrogen gas completely reacted with 3.000 mol of nitrogen gas at constant pressure, releasing 277 kJ of heat, which of the following thermochemical equations is correct? Group of answer choices A, 3H2(g) + N2(g) => 2NH3(g); ΔH° = +92.33 kJ B, 3H2(g) + N2(g) => 2NH3(g); ΔH° = +831kJ C, 3H2(g) + N2(g) => 2NH3(g); ΔH° = +277 kJ D, 3H2(g) + N2(g) => 2NH3(g); ΔH° = –92.3 kJ E, 3H2(g) + N2(g) => 2NH3(g); ΔH° = –277 kJarrow_forward
- Predict the sign of ΔS°, if possible, for the following reaction. A. N2(g) + O2(g) ----> 2NO(g) B. C2H2(g) + 2H2(g) ----> C2H6(g) Question 3 options: positive negative not predictablearrow_forwardWith hypothetical equation Calculate the value of ΔH (in kJ) for the reaction: Q2 (g) + ½ X2 (g) → Q2X (g) 2QJ3 (g) + 3Q2X (g) → 4Q2 (g) + 3J2X (l) ΔH = -1,058.1 kJ 4QJ3 (g) + 3X2 (g) → 2Q2 (g) + 6J2X (l) ΔH = -1,594.2 kJarrow_forwardConsider 8 the following reaction: 2NH3(g) + CO2(g) → NH2CONH2(aq) + H2O(l) ∆G° = -13.6 kJ at 25°C What is the value of ∆G at 25°C for this reaction under the following set of conditions? 25.0 atm NH3 (g) 0.500 atm CO2 (g) 1.00 M NH2CONH2 (aq) Group of answer choices -18.1 kJ 0.63 kJ -27.8 kJ 14.2 kJ -20.0 kJarrow_forward
- For the following reaction, Kp = 4.768 at 700o K. NOCl(g) ⇄ NO(g) + 1/2 Cl2(g) What is Kp for the reaction below at this same temperature? Cl2(g) + 2 NO(g) ⇄ 2 NOCl (g) Express your answer using at least two significant figures. Do not use scientific notation.arrow_forwardFor the reaction CaCO3(s) → CaO(s) + CO2(g) which is spontaneous only at high temperatures Group of answer choices ∆H is positive and ∆S is positive ∆H is negative and ∆S is positive ∆H is positive and ∆S is negative ∆H is negative and ∆S is negativearrow_forwardWhat are the signs of ΔH,ΔS,ΔG when CO2 (dry ice) sublimes to a gas at room temperature and 1 atm pressure. The temperature of sublimation of dry ice is −78 C at 1 atm pressure.arrow_forward
- Which of the following processes are endothermic? Check all that apply. H2O(l) ⟶⟶ H2O(s) H2O(g) ⟶⟶ H2O(l) 2 C8H18(l) + 25 O2(g) ⟶⟶ 16 CO2(g) + 18 H2O(l) CO2(s) ⟶⟶ CO2(g) 2 H2(g) + O2(g) ⟶⟶ 2 H2O(g) Δ?=−241.83??ΔH=−241.83kJ 2 Al(s) + 1.5 O2 ⟶⟶ Al2O3 Δ?=−1675.7??ΔH=−1675.7kJ Br2(g) ⟶⟶ 2Br(g) 1/2 N2(g) + O2(g) ⟶⟶ NO2(g) Δ?=33.1??ΔH=33.1kJarrow_forwardFor the following reaction at 25°C, DH0 = -26.88 kJ and DS0 = 11.2 J/K. Calculate DG0 for the reaction at 25°C in kilojoules. I2(g) + Cl2(g) ® 2ICl(g) Choices: a. +77.0 kJ b. -50.6 kJ c. -102 kJ d. -30.2 kJ e. +50.6 kJarrow_forwardPredict the sign of S for each of the following and explain. a. the evaporation of alcohol b. the freezing of water c. compressing an ideal gas at constant temperature d. dissolving NaCl in waterarrow_forward
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