THERMODYNAMICS: Calculate the value of AH (in kJ) for the reaction, 2AR3 (g) + Q (s) – A2R4 (g) + QR2 (s) given the following hypothetical thermochemical equations: 2AR3 (g) + 2AX (g) → A2R4 (g) + 2XAR (g) AH = -80.2 kJ AX (g) + %R2 (g) - XAR (g) AH = -161.6 kJ Q (s) + R2 (g) – QR2 (s) AH = -504.2 kJ (Round off the final answer to ONE decimal place. Do not include the unit.)

THERMODYNAMICS: Calculate the value of AH (in kJ) for the reaction, 2AR3 (g) + Q (s) – A2R4 (g) + QR2 (s) given the following hypothetical thermochemical equations: 2AR3 (g) + 2AX (g) → A2R4 (g) + 2XAR (g) AH = -80.2 kJ AX (g) + %R2 (g) - XAR (g) AH = -161.6 kJ Q (s) + R2 (g) – QR2 (s) AH = -504.2 kJ (Round off the final answer to ONE decimal place. Do not include the unit.)

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. จงหาค่า AH ของปฏิกิริยานี้ จากข้อมูลที่กำหนดให้ 2C (s) + 2 H,0 (g) → CH, (g) + CO,(g) Determine the standard enthalpy change for this reaction from the following standard enthalpies of reaction: (1) C(s) + H,O (g) → CÓ (g) + H, (g) AH° = 131.3kJ (2) CO (g) + H2O (g) → CO2 (g) + H2 (g) ΔΗΟ = -41.2 kJ (3) CH, (g) + H,O (g) → 3H, (g) + CO (g) AH° = 206.1kJ ชื่อ-สกุล .วันที่ เลขที่ เรหัส.. (0202104) จงหาค่า AH และ As ของปฏิกิริยานี้ จากข้อมูลที่กำหนดให้ 3 ปฏิกิริยาการสังเคราะห์ด้วยแสงเกิดขึ้นดังสมการ 6 CO, (g) + 6 H,0 (1) CH2O6 (S) + 6 0, (g) กำหนดค่าที่สภาวะมาตรฐานของ AH และ S ของสารแต่ละตัว ดังนี้ AH°, (kJ mol-') s° (JK-1 mol-') สาร | CH,206 (s) -1,273 212 O, (g) 205 2/2 CO, (g) -393 214 H,0 (1) -285 70
Determine the enthalpy of the reaction: 3Fe,O; (s) + CO (g) → CO, (g) + 2Fe;O4 (s), given the following reactions. 38. Fe,O3 (s) + 3CO (g) → 2Fe (s) + 3CO, (g) AH= -28.0 kJ 3Fe (s) + 4CO2 (s) → 4CO (g) + Fe;O4 (s) AH =+12.5 kJ A) 40.5 +109 -59.0 -109
THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) – 4Q2 (9) + 3J2X (1) AH = -1,017.3 kJ 4QJ3 (g) + 3X2 (g) → 202 (9) + 6J2X (1) AH = -1,548.8 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (g) + % X2 (g) –→ Q2X (g) (Round off the final answer to ONE decimal place. Do not include unit.)
THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) → 4Q2 (g) + 3J2X (l) ΔH = -1,004 kJ 4QJ3 (g) + 3X2 (g) → 2Q2 (g) + 6J2X (l) ΔH = -1,520.1 kJ Calculate the value of ΔH (in kJ) for the reaction: Q2 (g) + ½ X2 (g) → Q2X (g)
THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) – 4Q2 (g) + 3J2X (1) AH = -1,096.4 kJ 4QJ3 (g) + 3X2 (g) → 202 (g) + 6J2X (1) AH = -1,548.8 kJ Calculate the value of AH (in kJ) for the reaction: Q2 (g) + % X2 (g) –→ Q2X (g) (Round off the final answer to ONE decimal place. Do not include unit,.)
THERMODYNAMICS: Calculate the value of AH (in kJ) for the reaction, 2AR3 (9) + Q (s) → A2R4 (g) + QR2 (s) given the following hypothetical thermochemical equations: 2AR3 (g) + 2AX (g) → A2R4 (9) + 2XAR (g) ΔΗ = -88.4 kJ AX (g) + ½R2 (g) → XAR (g) AH = -164.8 kJ Q (s) + R2 (g) –→ QR2 (s) AH = -520.4 kJ (Round off the final answer to ONE decimal place. Do not include the unit.)
Study the following thermochemical data very carefully: Clelg) lag) ICI(g) Ia(s) 2C(g) 21(g) I(g) + CI(g) la(g) AH = 242.3 kJ AH = 151.0 kJ AH = 211.3 kJ AH = 62.8 kJ I2(s) reacts with Clag) to produce ICI(g). Write the chemical equation to produce ONLY one mole of ICI(g)
Rearrange the thermochemical equations given to determine the AH value for the equation of interest. Determine: 2 Fe203(s) + 3 C(s) → 3 CO2(g) + 4 Fe(s) Given Enthalpy (K/mol) 3 -833.8 O2(g) Fe203(s) 2 1. 2 Fe(s) + ch 2. C(s) + - O2(8) → CO(g) -110.4 1 O2(g) → CO2(g) -264.8 3. CO(g) + K/mol
THERMODYNAMICS: Calculate the value of AH (in kJ) for the reaction, 2AR3 (g) + Q (s)→ A2R4 (g) + QR2 (s) given the following hypothetical thermochemical equations: 2AR3 (g) + 2AX (g) → A2R4 (g) + 2XAR (g) AH = -87.2 kJ AX (g) + ½R2 (g) → XAR (g) AH = -157.3 kJ Q (s) + R2 (g) – QR2 (s) AH = -510.2 kJ (Round off the final answer to ONE decimal place. Do not include the unit.)
to calculate the true enthalpies of these reactions by the Hess’ law, as: ΔH°(rxn) = Σ[ν × ΔHf°(product)] – Σ[ν × ΔHf°(reactant)] for: Mg(s) + ½O2(g) → MgO(s)
（1）Consider the reaction: 2A (g) + 3 B (g) → 2 C (g) ΔHrxn = +254.3 kJ What will be the enthalpy change (in kJ) if 0.471 mol B reacts in excess A? （2）Consider the reaction: C (s) + O2 (g) → CO2 (g) ΔHrxn = -393.5 kJ What mass of carbon (in g) must be reacted via this mechanism to release 581.2 kJ of heat?
THERMODYNAMICS Given the following hypothetical thermochemical equations: 2QJ3 (g) + 302X (g) 402 (9) + 3J2X (I) AH = -1,034 kJ 4QJ3 (g) + 3X2 (g) 202 (g) + 6J2X () AH = -1,577.7 kJ Calculate the value of AH (in kJ) for the reaction 02 (g) % X2 (g) Q2X (g) (Round off the final answer to ONE decimal place. Do not include unit)