21. The enthalpy changes of these reactions can be measured:AH° = -1411.1 kJC,H,(g) +30,(g)C,H,OH(C) + 3 0,(g)2 CO,(g) +2 H,O(€)2 CO,(g) + 3 H,0(e)1)AH° =-1367.5 kJ-Use these values and Hess's law to determine the enthalpy change for the reactionCH,(g) + H,0(()CH,OH(€)

Given C2H4(g) + 3O2(g) → 2CO2(g) + 2H2O(l) ∆H° = -1411.1 KJ (…

Answered: 21. The enthalpy changes of these…

Chemistry

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Chapter1: Chemical Foundations

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

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Consider the two reactions. 2 NH, (g) + 3 N,0(g) → 4N,(g) + 3 H,0(1) 4 NH, (g) + 3 0,(g) 2 N,(g) + 6 H,0(1) AH° = -1010 kJ AH° = 1531 kJ Using these two reactions, calculate and enter the enthalpy change for the reaction below. N, (g) + 0,(g) → N,0(g)
a) Calculate the enthalpy variation produced in the butane combustion reaction under standard conditions.b) what amount of heat will be released in the complete combustion of the 12kg of butane contained in a cylinder dH standard CO2 (g) = -393kJ / mol, H2O (l) = -286kJ / mol, C4H10 (g) = -125kJ / mol
Task 3.2. Calculate the standard enthalpy of reaction of some thermochemical equations governed by Hess Law. Direction: Solve the following items. Show complete solution. Express all standard enthalpy to kilojoules.
Calculate the enthalpy change in kJ for the following reaction given the data below. Answer: -610.1 kJ P4O10(g) + 6 PCl5(g) --> 10 Cl3PO(g) A 1/4 P4(s) + 3/2 Cl2(g) --> PCl3(g) Ho/kJ = -306.4 B P4(s) + 5 O2(g) --> P4O10(g) Ho/kJ = -2967.3 C PCl3(g) + Cl2(g) --> PCl5(g) Ho/kJ = -84.2 D PCl3(g) + 1/2 O2(g) --> Cl3PO(g) Ho/kJ = -285.7
*You may need your knowledge in balancing equations which you had learned in your Chem. 1 1. Calculate AH for the reaction from the given thermochemical equations. Tell whether the reaction is exothermic or endothermic C:H« (9) + Ha(g) CaHo(g) CO-(g) CO2(g) H;O(1) H20() H20() AH = -1411 kJ * CHalg) * CaHelg) + O2(g) * Hz(g) + Oz(g) O2(9) AH = -1569 kJ + AH = -285.8 kJ
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THERMODYNAMICS: Given the following hypothetical thermochemical equations: 20J3 (g) + 302x (g) – 402 (g) + 3J2X () AH = -1,017.3 kJ 4QJ3 (e) + 3X2 (@) – 202 (g) + 6J2X (1) AH = -1,548.8 kJ Calculate the value of AH (in kJ) for the reaction: a2 (g) + % X2 (a) - Q2X (g) (Round off the final answer to ONE decimal place. Do not include unit.)
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PCI5(s) can be prepared by the reaction PCI3(1) + Cl2(g) - PCI5(s). Calculate the enthalpy change (in kJ) that accompanies the production of 100.0 g of PCI5(s) by the above reaction, given the following data. P4(s) + 6 Cl2(g) - 4 PC|3(1) AH° = -1280 kJ per mole of P4(s) %3D P4(s) + 10 Cl2(g) – 4 PCI5(s) ΔΗ AH° = -1774 kJ per mole of P4(s) +59.3 -59.3 +124 -124 -258
Use the thermochemical equations shown below to determine the enthalpy for the reaction: C3H8(g) + 502(g) +3CO 2 + 4H2O(1) CO2 C(graphite) + 02 HE = 221.6KJ H2(g) + 1/2O2(g) H2O(1) HE= -160.3KJ 3 C(graphite) + 4 H2(g) C3H8(g) HE= -58.5KJ
The standard molar enthalpy change AH°= -3135 kJ for the combustion of benzene. CH,(1)+15/2 0,(9) → 6 Co,(g)+3 H,0(g) AH°= -3135 k) Calculate the standard molar enthalpy of formation for benzene AH°F[C,H,(1)] based on the following standard enthalpies of formation: AH°F[CO,(g)] = -393.5 kl/mol and AH°F[H,O(g)] =-241.8 kJ/mol. Select one: a. -783 kJ/mol b. -3230 kJ/mol c. +49 kJ/mol d. -7670 k)/mol
Q5 (i) Draw an energy cycle and use the Standard Enthalpies of combustion values in the table below to calculate the 10(g)* enthalpy of formation of butane, C4H₁09). Explain how the value obtained here might be different from the value obtained using calorimetry. (Show working as this question will be assessed using grade descriptors 1, 3 & 7) Substance Enthalpy of Combustion/kJ mol-¹ -394 -286 -2876 C(s) H2(g) CH10(9)

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21. The enthalpy changes of these reactions can be measured: AH° = -1411.1 kJ - 2 CO,(g) +2 H,0(() 2 CO,(g) +3 H,0() %3D C,H,(g) + 30,(g) C,H,OH(C) + 3 0,(g) AH° =-1367.5 kJ Use these values and Hess's law to determine the enthalpy change for the reaction C,H.(g) + H,O(() C,H,OH(€)