Chem 177 1st Edition Exam # 2 Study Guide Define these termsOxidation- reduction reaction-Concentration-Molarity (and formula)-Thermochemistry-1st law of thermodynamics-Internal energy-System types (systems and surroundings):- Open-- Closed-- Isolated-Enthalpy-State and path dependent functions-Hess’ law-Calorimetry-Excited and ground states of electrons-Wave nature (draw out)Wave nature of matter-Uncertainty principle-Quantum mechanics-Describe and draw out each of the following orbitals:- Principle quantum 1: n- Angular momentum quantum # (l)Example Problems1. Calculate the standard enthalpy change, ΔHo, for the formation of 1 mol of strontium carbonate (the material that gives the red color in fireworks) from its elements. Sr (s) + C(graphite ) + 32 O2 ( g ) → SrCO 3 (s ) The information available is(1) Sr (s ) + 12 O2 ( g) → SrO (s ) ΔH ° = -592 kJ(2) SrO ( s ) + CO 2( g ) → SrCO3 (s ) ΔH ° = -234 kJ(3) C(graphite ) + O 2( g ) → CO 2 (g ) ΔH ° = -394 kJ2. The combination of coke and steam produces a mixture called coal gas, which can be used as afuel or as a starting material for other reactions. If we assume coke can be represented by graphite, the equation for the production of coal gas is2 C (s ) + 2 H 2 O ( g ) → CH 4 (g ) + CO 2( g ) Determine the standard enthalpy change for this reaction from the following standard enthalpies of reaction:(1) C( s ) + H2 O (g ) → CO ( g ) + H2 (g ) ΔH ° = 131 .3 kJ(2) CO (g ) + H 2 O ( g ) → CO2( g) + H 2( g ) ΔH ° = - 41 . 2 kJ(3) CH4 ( g) + H 2 O (g ) → 3 H2 (g ) + CO ( g ) ΔH ° = 206 .1 kJAnswers: 1. – 1220 kJ 2. + 15.3 kJ3. Hydrogen peroxide decomposes according to the following thermochemical reaction:H2O2(l) → H2O(l) + 1/2 O2(g); ΔH = -98.2 kJCalculate the change in enthalpy, ΔH, when 1.00 g of hydrogen peroxide decomposes.Answer: The change in enthalpy, ΔH, when 1.00 g of hydrogen peroxide decomposes = -2.89 kJ4. Write the electron configurations for the following: (noble gas form)Ga:Fe:Na:Write the full electron configuration, short-hand electron configuration, and fill in the orbital diagrams, for the following elements. 5. Nitrogen ______________________________________________________________1s 2s 2p 3s6. Write the net ionic equation for the following reaction. For full credit, include the phase of all substances (s, l, g, or aq). 2 HClO3 (aq) + Ba(OH)2 (aq) Ba(ClO3)2 (aq) + 2 H2O(l)7. Calculate the molar concentration of potassium ions K+ in a solution formed from mixing 10.0mL of 0.10 Molar K3PO4(aq) with 10.0 mL of 0.10 Molar K2SO4(aq). Assume that the volumes are additive. 8. How many liters of 0.23 molar NaOH is needed to neutralize 2.63 liters of 0.49 molar EDTA. EDTA is a weak acid that can donate four protons H+ and is symbolized in the following equation as H4Y. 9. What are strong, weak, and non