10.00 g of Compound X with molecular formula C4H8 are burned in a constant-pressure calorimeter containing 50.00 kg of water at 25 °C. The temperature ofthe water is observed to rise by 2.151 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.)Calculate the standard heat of formation of Compound X at 25 °C.Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.

Answered: 10.00 g of Compound X with molecular…

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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2.000 g of Compound X with molecular formula C5H₁0 are burned in a constant-pressure calorimeter containing 45.00 kg of water at 25 °C. The temperature 10 of the water is observed to rise by 0.4696 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeter itself.) Calculate the standard heat of formation of Compound X at 25 °C. Be sure your answer has a unit symbol, if necessary, and round it to 3 significant digits. 0 00 X Ś x10
To a test tube containing 10.0 ml of 0.50 M HCl solution in a calorimeter, 0.05482 g of solid MgO (MW = 40.30 g/mol) at the same temperature was added. A change in temperature of 6.2°C was recorded. In a separate experiment, the heat capacity of the calorimeter was determined to be 0.293 kJ/°C. 1. Write the balanced equation for the reaction between HCl and MgO.2. Which is the limiting reactant? Show your solution.3. Calculate heat released by the reaction, qrxn, in the calibration step (in kJ).
A quantity of 85.0 mL of 0.600 M HCl is mixed with 85.0 mL of 0.600 M KOH in a constant-pressure calorimeter. The initial temperature of both solutions is the same at 17.35°C, and the final temperature of the mixed solution is 19.02°C. What is the heat capacity of the calorimeter? Assume that the specific heat of the solutions is the same as that of water and the molar heat of neutralization is −56.2 kJ/mol.
A 2.30 g sample of ethanol, CH3CH2OH, is combusted in a bomb calorimeter. The temperature of the calorimeter increases by 4.89 K. If the heat capacity of the bomb is 663 J/K and it contains 2.57 kg of water, what is the enthalpy change per mole of ethanol combusted? The specific heat capacity of water is 4.18 J/g×K and the molar mass of ethanol is 46.07 g/mol.
The first step in the production of nitric acid from ammonia involves the oxidation of NH3. 4 NH3(g) + 5 O₂ (g) → 4 NO(g) + 6 H₂O(g) 2 a Use standard enthalpies of formation from the table below to calculate the standard enthalpy change for this reaction. Species AfH (kJ/mol) NH3(g) -45.90 NO(g) +90.29 H₂O(g) -241.83 Standard enthalpy change Submit = kJ/mol-rxn
An electrical heater adds 25.3 kJ of heat to a constant-volume calorimeter. The temperature of the calorimeter rises by 4.55 °C. When 1.75 g of methanol is burned in the same calorimeter, the temperature increases by 7.14 °C. Calculate the molar energy of combustion of methanol. kJ/mol
When 6.10 g of urea,(NH2)2CO (g), burns to produce CO2 (g), N2 (g) and H2O (l) 67.8 kJ of heat energy are released in a bomb calorimeter. What is the energy released in the burning of one mole of urea? Using this, what is the enthalpy of formation of urea?
A scientist measures the standard enthalpy change for the following reaction to be -234.6 k) : 2502(g) + 02(g)→2s03(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of so3(g) is kJ/mol.
15. Use the following reactions for which the reaction enthalpies are given to determine the reaction enthalpy of: Given: N₂H40) + 2 H₂O2(1)→ N2(g) + 4H₂O N₂H4(1) + 3 O2(g) → 2 NO2(g) + 2 H₂O(g) H₂O(1) + 1/2O2(g) → H₂O2(1) 1/2 N2(g) + O2(g) → NO₂(g) H₂O → H₂O ΔΗ° = _466 kJ AH°= 98.0 kJ AH° = 34.0 kJ AH° = 44.0 kJ
5.00 × 10−2 mol KOH and an excess of hydrochloric acid are combined in 100.0 mL of water initially at 25.0 °C, leading to a final measured temperature of 31.1 °C. (a) What is the heat flow for the water in the calorimeter, qH2O, in Joules? (b) Assuming the calorimeter constant Ccal = 50.0 J °C , what is the heat flow for the calorimeter, qcal, in Joules? (c) What is the amount of heat given off by the reaction, qrxn, in Joules? (d) What is the molar enthalpy of the neutralization reaction (shown below) as measured in the calorimeter, ∆H◦ rxn in kilojoules per mole? H3O + (aq) + OH– (aq) → 2H2O (l)
Hydrobromic acid (HBr) is a commonly used acid for adding bromine to organic compounds. As bromine makes for an easily replaceable substituent, these bromine precursors are a necessary part of a vast amount of organic eynthesis, Calculate the reaction enthalpy for the synthesis of HBr according to H2(g) + Bra)2Br(g) Use the following information: NH3(g) +HBr(g) → NHABr(s) AH =-188.32 kJ Na(g) + 3H2(g) → 2NH3(g) AH = -92.22 kJ N2(g) + 4H2(g) + Br2(1) → 2NHABr(s) AH =-541.66 kJ a. AH =-728 kmol b. AH =-1010.52 KJjmol C. AH =-826.08 KJ/mol d. AH =728 kJ/mol e. AH = -257.24 kJ/mol Clear my choice
3. Write a balanced chemical reaction for the synthesis of methane (CH4) and liquid water from hydrogen and acetic acid (CH3COOH) and calculate the standard enthalpy of the reaction by using the appropriate enthalpies of formation on page 308 or Appendix 4 in the textbook.

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