Diborane-6 (B₂H6) is a colorless, highly reactive gas that will burst into flames when exposed to oxygen. The reaction is B₂H(g) + 30₂(g) - - B₂O3(s) + 3 H₂O (1) Calculate the kilojoules of heat released per gram of the compound reacted with oxygen. The standard enthalpy of formations of B₂H, (g), B₂O₂ (s), O₂ (g) , and H₂O (1) are 36.4 1273.5 kJ kJ 0 mol mol and-285.8 kJ mol , respectively. Round your answer to 1 decimal place. kJ mol'

Diborane-6 (B₂H6) is a colorless, highly reactive gas that will burst into flames when exposed to oxygen. The reaction is B₂H(g) + 30₂(g) - - B₂O3(s) + 3 H₂O (1) Calculate the kilojoules of heat released per gram of the compound reacted with oxygen. The standard enthalpy of formations of B₂H, (g), B₂O₂ (s), O₂ (g) , and H₂O (1) are 36.4 1273.5 kJ kJ 0 mol mol and-285.8 kJ mol , respectively. Round your answer to 1 decimal place. kJ mol'

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? exothermic endothermic (b) Calculate the amount of heat transferred when 55.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced? g(d) How many kilojoules of heat are released when 12.0 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = kJ(e) Calculate E when 450.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K
2. (a) 36 mL of 1.0M hydrochloric acid is react with a solution of sodium hydroxide of the concentration 1.6M and volume 15 mL in a coffee cup calorimeter. It is noted that the temperature of both solutions before the reaction is 27.5 °C. After the reaction, the temperature of the solution raise to 35.0 °C. Calculate heat of neutralization for the reaction.(cw = 4.18 Jgl°C', Density of solution: 1gmL').
Consider the following reaction. CH3OH(g) CO(g) + 2 H2(g) H = +90.7 kJ (a) Is the reaction exothermic or endothermic? endothermicexothermic (b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H = kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced? g(d) How many kilojoules of heat are released when 13.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H = kJ(e) Calculate E when 360.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K kJ HopHelpCh5N1
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300. g of water (see sketch at right). thermometer stirrer First, a 6.000 g tablet of benzoic acid (C,H,C0,H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is insulation observed to rise from 13.00 °C to 40.13 °C over a time of 10.0 minutes. Next, 5.200 g of ethane (C,H) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 13.00 °C to 53.96 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H,(g) + 70,(g) 4CO,(g) + 6 H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced…
The heat of formation at 25oC of liquid acetone, CH3C(O)CH3(l) is -247.5 kJ/mol. Which of the following is the correct heat of formation reaction for CH3C(O)CH3(l) )? 3C(s,graphite)+3H2(g)+12O2(g)→CH3C(O)CH3(l)△Hof=−247.5kJmol 3C(s,graphite)+6H(g)+O(g)→CH3C(O)CH3(l)△Hof=−247.5kJmol CH3C(O)CH3(l)+4O2(g)→3CO2(g)+3H2O(g)△Hof=−247.5kJmol C3(s,graphite)+3H2(g)+12O2(g)→CH3C(O)CH3(l)△Hof=−247.5kJmol 6C(s,graphite)+6H2(g)+O2(g)→2CH3C(O)CH3(l)△Hof=−247.5kJmol
O THERMOCHEMISTRY Using Hess's Law to calculate net reaction enthalpy Lindsay Dimethyl ether, a useful organic solvent, is prepared in two steps. In the first step, carbon dioxide and hydrogen react to form methanol and water: CO,(g) + 3 H,(g) → CH;OH(1) + H,0(1) AH=-131. kJ In the second step, methanol reacts to form dimethyl ether and water: 2 CH,OH(1) → CH;OCH,(g) + H,0(1) AH=8. kJ Calculate the net change in enthalpy for the formation of one mole of dimethyl ether from carbon dioxide and hydrogen from these reactions. Round your answer to the nearest kJ. II
Decaborane-14 (B₁H₁4) is a white, highly reactive solid that will burst into flames when exposed to oxygen. The reaction is B₁H₁(g) + 110₂(g) SB₂0,(s) + 7H₂0 (1) Calculate the kilojoules of heat released per gram of the compound reacted with oxygen. The standard enthalpy of formations of B, H₁ (s), B₂O, (s), 0, (g) , and H₂O (/) are 82.8 kJ mol -1273.5 kJ kJ 0 mol' mol' 4 kJ 1- released 8 B. H.. 10 14 and-285.8 2 kJ mol respectively. Round your answer to 1 decimal place.
Incorrect. What is the heat of formation of elements in their standard states? Did you use the correct equation of products minus reactants? The amino acid glycine, C2H5NO2, is one of the compounds used by the body to make proteins. The equation for its combustion is 4C2H5NO2(s) + 902(g) → 8CO2(g) +10H20(1) +2N2(g) For each mole of glycine that burns, 973.49 kJ of heat is liberated. Use this information, plus values of AHº for the products of combustion, to calculate AH° for glycine. AH = kJ/mol eTextbook and Media Hint Solution 935 pm A 27°C Haze O G 10 ENG Type here to search 15/03/2022 1080 acer Insert Delete F11 F12 Prt Sc Pause Br F8 F9 F10 F7 NumLk F5 F3 Esc Coca) Backsp * 8 8 # 2$ % & 9 @ € 7 1 2 3 !!
Use Hess’s law to calculate the enthalpy change for the reaction WO3(s) + 3H2(g) —> W(s) +3H2O(g) from the following data: 2W(s) + 3O2(g) —> 2 WO3(s) H=-1685.4 2H2(g) + O2(g) —> 2H2O(g) H=-477.84
Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g), by the reaction 2 SO2(g) + O2(g) → 2 SO3(g) The standard enthalpies of formation for SO2(g) and SO3(g) are AH; [SO2(g)] = -296.8 kJ/mol AH; [SO3(g)] = -395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 2.25 L of SO2(g) is converted to 2.25 L gas behavior. of SO3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C. Assume ideal AH= kJ
A generic solid, X, has a molar mass of 78.678.6 g/mol. In a constant‑pressure calorimeter, 30.730.7 g of X is dissolved in 327327 g of water at 23.00 °CX(s)⟶X(aq)X(s)⟶X(aq) The temperature of the resulting solution rises to 28.5028.50 °C. Assume the solution has the same specific heat as water, 4.184 J/(g·°C), and that there is negligible heat loss to the surroundings. How much heat was absorbed by the solution?
When methanol, CH3OH,CH3OH, is burned in the presence of oxygen gas, O2,O2, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation CH3OH(g)+32O2(g)⟶CO2(g)+2H2O(l)ΔH=−764 kJCH3OH(g)+32O2(g)⟶CO2(g)+2H2O(l)ΔH=−764 kJ How much methanol, in grams, must be burned to produce 639 kJ639 kJ of heat?