Standard enthalpy of reactions can be calculated from standard enthalpies of formation of reactants. A True B. False Calculate AH for the combustion reaction of CH shown below given the following: AHf CH(g) -74.8 kJ/mol; AHt CO,(g) 393.5 kJ/mol; AHf H,O() -285.5 kJ/mol CH(g) + 2 0,(g) -> co,(g) + 2 H,0(1) Find the standard enthalpy of formation of ethylene, C2H4(g), given the following data: C2H4(g) 3 02(g) ---> 2 co2(g) + 2 H20(1) AHrn=-1411 kJ; C(s) + 02(g) co2(g) AH, -393.5 kJ; H2(g) + %02(g) -> H2O(1) AH, = 285.8 kJ A 604.2 kJ B. 889.7 kJ C. -997.7 kJ D. -889.7 kJ E. None of the above A 731 kJ B. 2.77 x 103 kJ C. 1.41x 103 kJ D. 87 kJ E. 52 kJ

Standard enthalpy of reactions can be calculated from standard enthalpies of formation of reactants. A True B. False Calculate AH for the combustion reaction of CH shown below given the following: AHf CH(g) -74.8 kJ/mol; AHt CO,(g) 393.5 kJ/mol; AHf H,O() -285.5 kJ/mol CH(g) + 2 0,(g) -> co,(g) + 2 H,0(1) Find the standard enthalpy of formation of ethylene, C2H4(g), given the following data: C2H4(g) 3 02(g) ---> 2 co2(g) + 2 H20(1) AHrn=-1411 kJ; C(s) + 02(g) co2(g) AH, -393.5 kJ; H2(g) + %02(g) -> H2O(1) AH, = 285.8 kJ A 604.2 kJ B. 889.7 kJ C. -997.7 kJ D. -889.7 kJ E. None of the above A 731 kJ B. 2.77 x 103 kJ C. 1.41x 103 kJ D. 87 kJ E. 52 kJ

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

A scientist measures the standard enthalpy change for the following reaction to be 154.8 kJ : CaCO3(s)Cao(s) + CO2(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CaO(s) is kJ/mol.
Using the standard enthalpies of formation provided, calculate the energy change for the combustion of methanol: 2 CH3OH(l) + 3 O2(g) ⟶⟶ 2 CO2(g) + 4 H2O(g) Standard Enthalpies of Formation (kJ/mol)CH3OH(l) = -238.4 CO2(g) = -393.5 H2O(g) = -241.8
A scientist measures the standard enthalpy change for the following reaction to be -1057.0 kJ: 2H2S(g) + 3 02(g) 2H20(g) + 2 S02(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H20(g) is kJ/mol.
A scientist measures the standard enthalpy change for the following reaction to be 36.8 kJ: CO₂(g) + H₂(g) → CO(g) + H₂O(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CO(g) is kJ/mol. Substance AH (kJ/mol) f CO₂(g) -393.5 H₂(g) 0.0 H₂O(g) -241.8
A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water (see sketch at right). First, a 7.000 g tablet of benzoic acid (C6H₂CO₂H) 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 19.00 °C to 54.07 °C over a time of 14.3 minutes. Next, 4.940 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 19.00 °C to 63.23 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: + 502 (8) Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. Calculate the reaction enthalpy AHxn…
[References] 1 pt b. Balanced formula equation: 1 pt HCHO2(aq) + KOH(aq) 1 pt 1 pt Complete ionic equation: 1 pt 1 pt 1pt 1 pt Net ionic equation: 1 pt 1 pt 1 pt c Balanced formula eqmation: 92) e element +. +.
9. A 40.0 kg industrial calorimeter has an overall specific heat capacity of 1.00 J/ (g°C). Complete combustion of 1.00 g of hydrogen in this calorimeter causes a temperature increase of 3.54°C. Calculate the molar enthalpy of combustion for hydrogen from this evidence. (-286 kJ/mol)
A scientist measures the standard enthalpy change for the following reaction to be 208.5 kJ :CH4(g) + H2O(g)3H2(g) + CO(g)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of CH4(g) is kJ/mol.
A scientist measures the standard enthalpy change for the following reaction to be -572.6 kJ:H2CO(g) + O2(g)CO2(g) + H2O(l)Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H2O(l) is?
For questions 4-7 Calculate ?Hrxn for the given reaction using the enthalpy of formation values provided at the end of the assignment.4) CaO(s) + SO3(g) → CaSO4(s) Substance Heat of Formation (?Hf) in kJ/mol CaO(s) -635.5 SO₃(g) -395.2 CaSO₄(s) -1432.7 Al(s) 0 Fe₂O₃(s) -822.2 Al₂O₃(s) -1669.8 C₄H₁₀(l) -147.6 O₂(g) 0 CO₂(g) -393.5 H₂O(g) -241.8 H₂O(l) -285.8 H₂O₂(l) -187.6
The combustion of heptane, C,H16, occurs via the reaction C;H16 (g) + 1102(g)→7CO2(g) + 8H,O(g) with heat of formation values given by the following table: Substance (kJ/mol) C;H16 (g) -187.9 CO2 (g) 393.5 H2O(g) -241.8 Calculate the enthalpy for the combustion of 1 mole of heptane. Express your answer to four significant figures and Include the appropriate units. > View Available Hint(s) HA 6 * O E ? Value Units
Use the standard molar enthalpies of formation and calculate the change in enthalpy for the reaction : 2CH3OH (l) + 3O2 (g) --> 2CO2 (g) + 4H2O (l) Given: CH3OH(l): -238.4 kJ/mol O2(g): 0 kJ/mol CO2(g): -393.5 kJ/mol H2O(l): -285.83 kJ/mol