Measuring qrxn Using a Bomb Calorimeter The combustion of methylhydrazine (CH&N2), a liquid rocket fuel, produces N2(g), CO2(g), and H2O(!): 2 CH&N2(1) + 5 O2(g) → 2 N2(g) + 2 CO2(g) + 6 H2O(1) When 4.00 g of methylhydrazine is combusted in a bomb calorimeter, the temperature of the calorimeter increases from 25.00 °C to 39.50 °C. In a separate experiment the heat capacity of the calorimeter is measured to be 7.794 kJ/ °C. Calculate the heat of reaction for the combustion of a mole of CH&N2.

Measuring qrxn Using a Bomb Calorimeter The combustion of methylhydrazine (CH&N2), a liquid rocket fuel, produces N2(g), CO2(g), and H2O(!): 2 CH&N2(1) + 5 O2(g) → 2 N2(g) + 2 CO2(g) + 6 H2O(1) When 4.00 g of methylhydrazine is combusted in a bomb calorimeter, the temperature of the calorimeter increases from 25.00 °C to 39.50 °C. In a separate experiment the heat capacity of the calorimeter is measured to be 7.794 kJ/ °C. Calculate the heat of reaction for the combustion of a mole of CH&N2.

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...

See similar textbooks

Similar questions

Using the following equation how many grams of pure oxygen do you need to consume 727 g of glucose: Your Answer: Answer C6H12O6 + 602 6CO2 + 6H₂O + energy -> units
Try Again Row 3: Your answer is wrong. In addition to checking your math, check that you used the right data and DID NOT round any intermediate calculations. A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). First, a 7.000 g tablet of benzoic acid (CH₂CO₂H) 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 15.00 °C to 53.26 °C over a time of 12.3 minutes. Next, 5.420 g of acetylene (C₂H₂) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 15.00 °C to 74.42 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or…
If the following three thermochemical equations are added together, what is the resulting equation:2 XO2 (g) +2 CO (g) →→ 2 XO (g) + 2 CO2 (g)2 XO (g) + 2/3 CO2(g) →→ 2/3 X3O4 (s) + 2/3 CO (g)2/3 X3O4 (s) + 1/3 CO2 (g) →→ X2O3 (g) + 1/3 CO (g) Question 17 options: 6 XO (g) + 2 CO2(g) →→ 2 X3O4 (s) + 2 CO (g) 2 XO2 (s) + CO (g) →→ X2O3 (s) + CO2 (g) C (s) + 3 XO2 (g) →→ X3O4 (g) + CO2 (g) 2 X3O4 (s) + CO2 (g) →→ 3 X2O3 (g) + CO (g) CO (g) + XO2 (g) →→ XO (g) + CO2 (g)
Calculate how much heat is released when 100. Grams of NO is mixed with 75 grams of O2.2NO(g) + O2(g)→ 2NO2(g) ?H= - 116kJ5. What is the limiting reagent
The enthalpy of combustion of isooctane (C8H18), one of the many hydrocarbons in gasoline is 5.45 × 103 kJ/mol. Calculate the enthalpy change per gram of isooctane and per liter of isooctane (d = 0.688 g/mL).
Use the References to access important values if needed for this question. The following thermochemical equation is for the reaction of methane(g) with water(g) to form hydrogen(g) and carbon monoxide(g). CH4(g) + H20(g)3H2(g) + CO(g) →3H2(g) + CO(g) AH = 206 kJ When 6.16 grams of methane(g) react with excess water(g), kJ of energy are Hint: An amount of energy is expressed as a positive number. The sign of AH in the thermochemical equation indicates whether the energy is absorbed or evolved.
What is the kinetic energy (in Joules) of a chlorine molecule moving at 167 m/sec?
Methanol (CH3OH) is also known as wood alcohol and can be used as a fuel. When one mole of methanol is burned, 1453 kJ of heat are evolved. When methanol is burned in a bomb calorimeter, 233 kJ of heat are evolved by the methanol. How many mL of methanol (d = 0.791 g/mL) were burned?
a Search this co Use the References to access important values if needed for this question. A 0.403-g sample of xanthone (C13H8O2) is burned in a bomb calorimeter and the temperature increases from 25.10 °C to 27.51 °C. The calorimeter contains 1.07x10 g of water and the bomb has a heat capacity of 802 J/°C. The heat capacity of water is 4.184 J g T°C. Based on this experiment, calculate AE for the combustion reaction per mole of xanthone burned. kJ/mol Submit Answer 5 question attempts remaining