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Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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55. Does the standard enthalpy of formation of H2O(g) differ from ΔH° for the reaction 2H2(g)+O2(g)⟶2H2O(g)?
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- Calculate the enthalpy for the reaction, BaC₂ (s) + 2 H₂O (l) → Ba(OH)₂ (aq) + C₂H₂ (g) Using the appropriate data from the following reactions, Ba (s) + 2 C (graphite, s) → BaC₂ (g) ∆H° = +437 kJ/mol Ba (s) + 2 H₂O (l) → Ba(OH)₂ +H₂ (g) ∆H° = -374.7 kJ/mol Ba (s) + 1/2 O₂ (g) → BaO (s) ∆H° = -553.5 kJ/mol BaO (s) + H₂O (l) → Ba(OH)₂ (aq) ∆H° = -107 kJ/mol C₂H₂ (g) + 5/2 O₂ (g) → 2 CO₂ (g) + H₂O (l) ∆H° = -1300. kJ/mol C (graphite, s) + O₂ (g) → CO₂ (g) ∆H° = -393.5 kJ/mol H₂ (g) + 1/2 O₂ (g) → H₂O (l) ∆H° = -285.8 kJ/molarrow_forward(b) Calculate the enthalpy change for the reaction C(graphite) + 2 H2(g) → CH4(g) with the help of the enthalpy changes of the following reactions: C(graphite) + O2(g) → CO2(g) ∆H= -393.5 kJmol−1 H2(g) +1/2O2(g) → H2O(l) ∆H = -285.8 kJmol−1 CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) ∆H = -890.4 kJmol−1 The temperature is 25 ◦C in all instances.arrow_forwardA system does 516516 kJ of work and loses 236236 kJ of heat to the surroundings. What is the change in internal energy, Δ?Δ�, of the system? Note that internal energy is symbolized as Δ?Δ� in some sources.arrow_forward
- Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction (show all work): P4(g) + 10 Cl2(g) → 4PCl5(s) ΔH°rxn = ? Given: PCl5(s) → PCl3(g) + Cl2(g) ΔH°rxn = +157 kJ P4(g) + 6 Cl2(g) → 4 PCl3(g) ΔH°rxn = -1207 kJarrow_forwardWhat is the standard enthalpy change for the reaction: 2C5H10(1) + 15O2(g) → 10CO2(g) + 10H20(1); where C5H10(1) AH°f = –605.0 kJ/mol; CO2(g) AH°f = -393.5 kJ/mol; H2O(1) AH°F - 285.8 kJ/mol. O a. -5583 kJ O b. -5783 kJ O C. -5383 kJ O d. -5183 kJ e. -4983 kJarrow_forward1. Methanol CH3OH is a potential source of fuel. An experiment was conducted to determine the enthalpy of combustion of methanol. 2.00 g of methanol was used to heat 150 g of water. The temperature of the water increased from 25°C to 87 °C. (Given that the specific heat capacity of water is 4.18 J K-1 g-1) Define the term standard enthalpy of combustion with reference to methanol. Use the data above to determine the enthalpy of combustion of methanol (show solutions). 2. Calculate the e.m.f of the following cell in the image (show solutions).arrow_forward
- If a system has 5.00×102 kcal5.00×102 kcal of work done to it, and releases 5.00×102 kJ5.00×102 kJ of heat into its surroundings, what is the change in internal energy (Δ? or Δ?)(ΔE or ΔU) of the system?arrow_forward(fHydrogen cyanide, a useful intermediate in the production of other pharmaceuticals and other chemicals, can be be prepared according to the following reaction: CH4(g) + NH3(g) ⟶⟶ HCN(g) + 3 H2(g). ΔΔHrxn= ???? Use the information provided to calculate the change in enthalpy for this reaction N2(g) + 3 H2(g) ⟶⟶ 2 NH3(g). ΔΔHrxn= -91.8 kJ/mol C(s) + 2 H2(g) ⟶⟶ CH4(g). ΔΔHrxn= -74.9 kJ/mol H2(g) + 2 C(s) + N2(g) ⟶⟶ 2 HCN(g) ΔΔHrxn= +270.3 kJ/molarrow_forwardGiven the standard enthalpy changes for the following two reactions: (1) N2(g) + 202(g)N204(g) AH° = 9.2 kJ (2) 2N20(g)2N2(g) + O2(g) AH° = -164.2 kJ what is the standard enthalpy change for the reaction: (3) 2N½0(g) + 302(g)- →2N2O4(g) AH° = ? kJarrow_forward
- (1)Consider the reaction: 2A (g) + 3 B (g) → 2 C (g) ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A? (2)Consider the reaction: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?arrow_forwardGiven the standard enthalpy changes for the following two reactions: (1) N2(g) + O2(g) 2NO(g) AH° = 181.8 kJ (2) N2(g) + 202(g)2NO2(g) AH° = 66.4 kJ what is the standard enthalpy change for the reaction: (3) 2NO(g) + O2(g) 2NO2(g) AH° = ? kJarrow_forward
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