Interpretation:
To fill
Concept Introduction:
Entropy
Gibbs free energy (G): The thermodynamic quantity to the (
Forward Reaction: This type of reaction has involved irreversible, if obtained product cannot be converted back in to respective reactants under the same conditions. Backward Reaction: This type of reaction process involved a reversible, if the products can be converted into a back to reactants.
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Chemistry: Atoms First
- Define the standard enthalpy of formation. What are standard states for elements and for compounds? Using Hess's law, illustrate why the formula Hreaction=npHf(products)nfHf(reactants) works to calculate H for a reaction.arrow_forwardFor the reaction TiCl2(s) + Cl2(g) TiCl4(), rG = 272.8 kj/mol-txn. Using this value and other data available in Appendix L, calculate the value of fG for TiCl2(s).arrow_forwardFor the reaction BaCO3(s) BaO(s) + CO2(g), rG = +219.7 kJ/mol-rxn. Using this value and other data available in Appendix L, calculate the value of fG for BaCO3(s).arrow_forward
- When 7.11 g NH4NO3 is added to 100 mL water, the temperature of the calorimeter contents decreases from 22.1 C to 17.1 C. Assuming that the mixture has the same specific heat as water and a mass of 107 g, calculate the heat q. Is the dissolution of ammonium nitrate exothermic or endothermic?arrow_forwardThe bombardier beetle uses an explosive discharge as a defensive measure. The chemical reaction involved is the oxidation of hydroquinone by hydrogen peroxide to produce quinone and water: C6H4(OH)2(aq) + H2O2(aq) C6H4O2(aq) + 2H2O(l) Calculate H for this reaction from the following data: C6H4(OH)2(aq) C6H4O2(aq) + H2(g)H = 177.4 kJ H2(g) + O2(g) H2O2(aq)H = 191.2 kJ H2(g) + 12O2(g) H2O(g)H = 241.8 kJ H2O(g) H2O(l)H = 43.8 kJarrow_forwardGiven the following data 2O3(g) 3O2(g)H = 427 kJ O2(g) 2O(g)H = 495 kJ NO(g) + O3(g) NO2(g) + O2(g)H = 199 kJ Calculate H for the reaction NO(g) + O(g) NO2(g)arrow_forward
- Shown below is a diagram depicting the enthalpy change of a chemical reaction run at constant pressure. a Is the reaction exothermic or endothermic? b What is the sign of H? c What is the sign of q? d If the reaction does no work, what is the sign of E for this process?arrow_forwardWhen calculating rSfromSvalues, it is necessary to look up all substances, including elements in their standard state, such as O2(g), H2(g), and N2(g). When calculating rHfrom rHvalues, however, elements in theirstandard state can be ignored. Why is the situation different forSvalues?arrow_forwardA 20.0-g block of iron at 50.0C and a 20.0 g block of aluminum at 45C are placed in contact with each other. Assume that heat is only transferred between the two blocks. a Draw an arrow indicating the heat flow between the blocks. b What is the sign of qsys for the aluminum when the blocks first come into contact? c What will you observe when qsys for the iron is zero? d Estimate the temperature of the Al and Fe blocks when qsys of the iron equals qsys of the aluminum.arrow_forward
- Given the following information at 25C, calculate G at 25C for the reaction 2A(g)+B(g)3C(g) Substance Hf(kJ/mol) S(J/molK) A(g) 191 244 B(g) 70.8 300 C(g) 197 164 a 956 kJ b 956 kJ c 346 kJ d 346 kJ e 1.03 103 kJarrow_forward9.83 A student performing a calorimetry experiment combined 100.0 mL of 0.50 M HCl and 100.0 mL of 0.50 M NaOH in a coffee cup calorimeter. Both solutions were initially at 20.0°C, but when the two were mixed, the temperature rose to 23.2°C. (a) Suppose the experiment is repeated in the same calorimeter but this time using 200 mL of 0.50 M HCl and 200.0 mL of 0.50 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why? (b) Suppose that the experiment is repeated once again in the same calorimeter, this time using 100 mL of 1.00 M HCl and 100.0 mL of 1.00 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why?arrow_forward9.96 Most first aid "cold packs" are based on the endothermic dissolution of ammonium nitrate in water: NH4NO3(s)NH4+(aq)+NO3(aq) H= 25.69 kJ A particular cold pack contains 50.0 g of NH4NO3 and 125.0 g of water. When the pack is squeezed, the NH4NO3dissolves in the water. If the pack and its contents are initially at 24.0°C, what is the lowest temperature that this bag could reach? (Assume that the ammonium nitrate solution has a specific heat of 4.25J g-l K-l, and that the heat capacity of the bag itself is small enough to be neglected.)arrow_forward
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