www-awu.aleks.com/alekscgi/x/Isl.exe/1o_u-IgNslkr7j8P3jH-IvUrTNdLZh5A8CnG03PBGuXr8ICPa7ZMmym9dTU3qxST1ZucrVpgTPcmJZmFF8YfXJcU_ZaDcV...AppsSprouts Academy:..6 Online TutoringC 400 Request Heade...Weather & Soil CH...O THERMOCHEMISTRY=Solving combustion thermochemistry problemsAlec15.00 g of Compound X with molecular formula C,H,, are burned in a constant-pressure calorimeter containing 10.00 kg of water at 25 °C. The temperature10of the water is observed to rise by 16.34 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the calorimeteritself.) 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.x10ArExplanationCheckO 2020 McGraw-Hill Education. All Rights Reserved. Terms of Use | Privacy AccessibilitySEUETPEebe10:37 PM2 Type here to search7)W10/12/2020DELL

The number of moles of compound can be calculated as, No. of moles = Given MassMolecular…

15.00 g of Compound X with molecular formula C,H10 are burned in a constant-pressure calorimeter containing 10.00 kg of water at 25 °C. The temperature of the water is observed to rise by 16.34 °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.

15.00 g of Compound X with molecular formula C,H10 are burned in a constant-pressure calorimeter containing 10.00 kg of water at 25 °C. The temperature of the water is observed to rise by 16.34 °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.

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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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 of the 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.
a group of chem students was asked to determine the heat of reaction for the neutralization of a newly synthesized monoprotic acid HX and NaOH. they first calibrated the styro ball calorimeter using the reaction of 15.0mL of 0.100M HCl and 20.0mL of 0.0500M KOH. this recorded a change in temperature from 26.5 °C to 31.8 °C. afterwards, they determined the heat of reaction for a mixture of 5.00mL, 1.00M NaOH and 10.0mL, 1.00M HX. this showed an increase in temperature of 3.6 °C C. What is the experimental enthalpy (in kJ/mol) for the neutralization reaction between HX and NaOH?D. Is the reaction between NaOH and HX endothermic or exothermic?
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When 60.0 mL of a 0.400 M solution of HNO3(aq) is combined with 60.0 mL of a 0.400 M solution of NaOH(aq) in a coffee-cup calorimeter, the final temperature of the solution is measured to be 26.6 °C. The initial temperature of the solutions is 24.0 °C. Calculate qrxn in joules, assuming the specific heat capacity of the final solution is 3.90 J.g-¹.°C-¹, the density of the final solution is 1.04 g/mL, and the calorimeter constant is 45 J/°C. (Hint: start with 9rxn+qsoln+qcal = 0.) The balanced chemical equation for this reaction is: HNO3(aq) + NaOH(aq) → H₂O(1) + NaNO3 (aq)
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
The molar heat of solution of a substance is found to be +21.38 kJ/mol. The addition of 0.100 mol of this substance to 1.000L of water initially at 40.0 degrees celsius results in a temperature decrease. Assume the specific heat of the resulting solution to be equal to that of pure water. Find the final temperature of the solution (Also assume that the heat capacity of the calorimeter is negligible).
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
A student is attempting to determine the heat capacity of a Styrofoam cup calorimeter by pouring hot water into a Styrofoam cup containing cold water. The student determined the mass of the cold water to be 21.2455 g and its initial temperature to be 20.36 °C. The mass of the hot water was 24.2646 g and its initial temperature as 34.54 °C. The final temperature of the water after mixing was determined to be 24.57°C. The specific heat capacity of the water is 4.184 J/(g•°C). What is the heat capacity of the Styrofoam cup calorimeter? Assume the temperature of the calorimeter is the same temperature as the cold water. 4.184 J/°C 132.5 J/°C
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