Enthalpy calculations for alcohol Initial mass burner (g) Initial temperature H2O(°C) Final temperature H2O(°C) Final mass burner (g) mburned (g) AT(°C) reaction (KJ) Moles of fuel burned, burned (mol) Enthalpy change per mole, AHmol (kJ/mol) Enthalpy change per gram, Qg (kJ/g) Run 1 Run 2 134.874 21.3 27.3 133.373 1.501 133.373 21.3 27.0 131.949 1.424 6.0 5.7 .005
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- In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.16. Using the information below, determine the enthalpy change (in kJ) for the reaction of 50.0 g of oxy gas (MW 32.0) with excess diborane gas (B2H6; MW 27.6). B2H6(g) + 302(g) B2O3(s) + 3H20() AH--2147.5 kJ a. -3360 kJ b. -2150 kJ c. -1300 kJ d. -1120 kJWhat is the enthalpy change of combustion of urea, (NH2)2CO, in kJ mol-1? 2(NH2)2CO(s) + 302(g) → 2CO2(g) + 2N2(g) + 4H2O(I) AH, I kJ mol (NH,),CO (s) CO, (g) H,O (1) -333 -394 -286 A. 2 x (-333) –2 × (-394) –4 × (-286) В. [2 x (-394) + 4 × (-286) -2 x (-333)] C. 2 x (-394) + 4 × (-286) –2 × (-333) D. (2 x (-333) –2 × (-394) –4 × (-286)]
- The standard enthalpy of reaction, AH°, for the reaction: 3H2(g) + N2O3(g) = N2(g) + 3H20(1) (1) is - 941.1 kJ mol-1 What is the value for the reaction? H2(g) +1/3N2O3(g) = 1/3N2(g) + H2O(1) (2) i) -104.7 kJ mol-1. ii) - 313.7 kJ mol-1. iii) - 941.1 kJ mol-1.ellus_engine.html?ClassID=1087757335# Calculate the standard reaction enthalpy for the reaction between NO and O3. NO(g) + O3(g) NO2(g) + O2(g) Compound AH°; (kJ/mol) NO(g) 90. AHxn = [ ? ] kJ %3D 0,(8) NO,(g) 143 34 Enter either a + or - sign and the magnitude. Enterus engine.html?ClassID=1087757335 Calculate the standard enthalpy of formation for ethane, C2H6, using the enthalpy for the reaction and the formation data. 2C2H6(g) + 702(g) → 4CO2(g) + 6H2O(g) AHxn = -2858 kJ Compound AH°; (kJ/mol) C,Ho(g) Co,(g) H,O(g) AH; = [ ? ] kJ -394 -242 Enter either a + or - sign and the magnitude. Enter
- When 50.0 g of oxygen gas (MW = 32.0) react excess diborane gas (B2H6; MW =D27.6), the enthalpy change is -1120 kJ. What is the enthalpy change for the reaction B2H6lg) + 3 O2lg) → B2O3(s) + 3 H20(1) AH° = ? O-2150 kJ -239 kJ -1120 kJ -717kJ Next ► « Previousus engine.html?ClassID=1087757335# Calculate the enthalpy of vaporization for the phase change from gaseous methanol to liquid methanol. CH3OH(g) → CH3OH(I) Compound AH°, (kJ/mol) CH,OH(I) CH,OH(g) -239 -201 AHvap = [ ? ] kJ/mol Enter either a + or - sign and the magnitude. EnterConstruct enthalpy cycles; use Hess's law and the following data to calculate the enthalpy of formation of ethane (from carbon and hydrogen gas). Cis) + Ozig) + CO2(g) AHa = -394kJmol H2g) + %02(a) – H20 m AH°. = -286kJmol1 + 3%O2(g) → 2002(9) + 3H20 m AH = -1560kJmol1
- Use Table 6.3 or Appendix B to write balanced formation equations at standard conditions for each of the following compounds. (Type your answer using the format 03 for 03. Write all coefficients, even if they are fractions or 1.) (a) (Apply fractions as needed.) (s) + (g) AgCI(s) (b) (Use the lowest possible coefficients.) (s) + (g) → TIO2(s) (c) (Apply fractions as needed.) (g) O3(9) (d) (Apply fractions as needed.) H2(g) + (graphite) + (g) HCN(g)For-each of the-two-following-equations, write-the symbol (use-this-A), and-calculate the molar enthalpy-of-combustion ofthe-substance-that-reacts-with-oxygen-gas. Show your-work!-(3)1 a)→4NH3le++70zie)-4-NO2)++6H2)++1272.1-kl1 b)→2N2(e)++O2(e)++163.2-kJ> N201Esc ||| = OTHERMOCHEMISTRY A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water (see sketch at right). Calculating heat of reaction from bomb calorimetry data First, a 5.000 g tablet of benzoic acid (C6H,CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 16.00 °C to 38.96 °C over a time of 9.2 minutes. 2 4. Next, 5.730 g of acetaldehyde (C₂H₂O) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 16.00 °C to 42.19 °C. 84°F Sunny Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: FI Explanation Is this reaction exothermic, endothermic, or neither? 4- F₂ Check 2C₂H4O(g) + 50₂(g) 4CO₂(g) + 4H₂O(g) Be sure any of your answers that are…