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: AH = -81.9 k) AH = -159.1 kj 2AR3 (g) + 2AX (g) A2R4 (g) + 2XAR (g) AX (g) + ½R2 (g) - XAR (g) Q (s) + R2 (g) → QR2 (s) (Round off final answer to ONE decimal place) AH = -510.4 kJ Round your answer to 1 decimal place.

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: AH = -81.9 k) AH = -159.1 kj 2AR3 (g) + 2AX (g) A2R4 (g) + 2XAR (g) AX (g) + ½R2 (g) - XAR (g) Q (s) + R2 (g) → QR2 (s) (Round off final answer to ONE decimal place) AH = -510.4 kJ Round your answer to 1 decimal place.

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

THERMODYNAMICS: Given the following hypothetical thermochemical equations: 2QJ3 (g) + 3Q2X (g) – 4Q2 (g) + 3J2X (1) AH = -1,070 kJ 4QJ3 (g) + 3X2 (g) → 202 (g) + 6J2X (1) AH = -1,580.2 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.)
Determine the heat of reaction for the decomposition of calcium carbonate CaCO3(g) → CaO(s) + CO2(g) given the following thermochemical equations: Ca(OH)2(s) --> CaO(s) + H20() Ca(OH)2(s) + CO2(g) --> CaCO3(s) + H20() C(s) + 02(g) -> CO2(g) 2Ca(s) + 02(g) --> 2CaO(s) O a. 345.5 kJ O b.441.0 kJ c. 178.4 kJ O d. 48.0 kJ ÄH = 65.2 kJ ÄH = -113.2 kJ ÄH = -393.5 kJ ÄH = -1270.2 kJ
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.)
The thermite reaction, used for welding iron, is the reaction of FegO4 with Al. 8 Al (s) + 3 Fe3O4 (s) > 4 Al203 (s) + 9 Fe (s) AH° = -3350 kJ Because this large amount of heat cannot be rapidly dissipated to the surroundings, the reacting mass may reach temperatures near 3000°C. How much heat (in kJ) is released by the reaction of 16.5 g of Al with 76.7 g of Fe304? Enter your numerical answer in units of kJ.
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.)
12.00 g of Compound with molecular formula C4h8 are burned in a constant-pressure calorimeter containing 15.00 kg of water at 25 °C. The temperature of the water is observed to rise by 8.603 °C. (You may assume all the heat released by the reaction is absorbed by the water, and none by the 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 the correct number of significant digits. calorimeter itself.)
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)
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
4. What mass of propane must be burned to supply 700. kJ as heat? The thermochemical equation for the combustion of propane is: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4H₂O(1) AH°-2220. kJ