THERMODYNAMICS: Calculate the value of AH (in kJ) for the reaction, 2AR3 (g) + Q (s) → A2R4 (g) + QR2 (s) given thefollowing hypothetical thermochemical equations:AH = -82.9 kJAH = -156.8 kJ2AR3 (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 = -505.6 kJRound your answer to 1 decimal place.

Answered: Image /qna-images/answer/08b8d3f8-df7f-4e4d-a6cc-ffd9423ede31.jpg

ICS: Calculate the value oT (in kJ) Tor the Peaction, ZAR3 (g) + Q (s) → A2R4 (g) + QR2 (S) given thne ollowing hypothetical thermochemical equations: AH = -82.9 kJ AR3 (g) + 2AX (g) → A¿R4 (g) + 2XAR (g) AH = -156.8 kJ X (g) + ½R2 (g) → XAR (g) 2 (s) + R2 (g) → QR2 (s) Round off final answer to ONE decimal place) AH = -505.6 kJ

ICS: Calculate the value oT (in kJ) Tor the Peaction, ZAR3 (g) + Q (s) → A2R4 (g) + QR2 (S) given thne ollowing hypothetical thermochemical equations: AH = -82.9 kJ AR3 (g) + 2AX (g) → A¿R4 (g) + 2XAR (g) AH = -156.8 kJ X (g) + ½R2 (g) → XAR (g) 2 (s) + R2 (g) → QR2 (s) Round off final answer to ONE decimal place) AH = -505.6 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

When 1.16E-1 g of Zn(s) combines with 5.21E1 mL of HCl(aq) in a coffee cup calorimeter, all of the zinc reacts, which increases the temperature of the HCl solution from 2.34E1 °C to 2.46E1 °C:Zn(s) + 2HCl(aq) → ZnCl(aq) + H(g) Calculate the enthalpy change of the reaction ΔH in J/mol. (Assume the volume of the solution doesn't change, density of the solution is 1.00 g/mL and the specific heat capacity of solution is 4.184 J/g°C.)
Using Hess law, compute the thermochemical equation to know the total heat of RXN. C,H. (g) + H2 (g) → C,H« (g) AH = ? C2H4 (g) + 3 O2 (g) → 2 CO2 (g) + 2 H¿O (I) C>Ho (g) + 3 ½ 0; (g) → 2 CO2 (g) + 3 H;O (1I) H2 (g) + ½ O> (g) → H;O (1). AH-- 1411.0 kJ AH = -1560.0 kJ AH = -285,8 kJ a. -3216.8 kJ b. -136.8 kJ c. 3216 kJ d. -136.8 J
O THERMOCHEMISTRY 15 Using Hess's Law to calculate net reaction enthalpy Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. In the first step, nitrogen and hydrogen react to form ammonia: N,(9) + 3 H,(g) → 2 NH;(9) AH=-92. kJ In the second step, ammonia and oxygen react to form nitric acid and water: NH,(g) + 20,(g) → HNO3(g) + H,0(g) AH=-330. kJ Calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ.
Given the two thermochemical equations below, find the enthalpy change for the reaction: N2H4 (l) + H2 (g) → 2 NH3 (g) delta H = ? Given: N2O4 (g) + 3 H2 (g) → 2 NH3 (g) + 2 O2 (g) delta H = – 100.96 kJ N2O4 (g) + 2 H2 (g) → N2H4 (l) + 2 O2 (g) delta H = + 41.47 kJ Select one: a. – 142.43 kJ b. – 59.49 kJ c. + 41.47 kJ d. + 59.49 kJ e. + 142.43 kJ f. none of these g. – 100.96 kJ
Given: 4AICI3(s) + 302(g) → 2Al,O3(s) + 6C12(g); AH=-529.0 kJ determine AH for the following thermochemical equation. Cl,(3) + Al,O;(s) → AICI,(9) + 02(g) O +88.2 kJ O +264.5 kJ O +176.3 kJ O -176.3 kJ O +529.0 kJ
O THERMOCHEMISTRY Using Hess's Law to calculate net reaction enthalpy Lindsay Dimethyl ether, a useful organic solvent, is prepared in two steps. In the first step, carbon dioxide and hydrogen react to form methanol and water: CO,(g) + 3 H,(g) → CH;OH(1) + H,0(1) AH=-131. kJ In the second step, methanol reacts to form dimethyl ether and water: 2 CH,OH(1) → CH;OCH,(g) + H,0(1) AH=8. kJ Calculate the net change in enthalpy for the formation of one mole of dimethyl ether from carbon dioxide and hydrogen from these reactions. Round your answer to the nearest kJ. II
Calculate the heat of neutralization for limewater, Ca(OH):(aq), and hydrochloric acid, HCl: Ca(OH):(aq) + 2 HCl(aq) → CaCl:(aq) + 2 H¿O(1) AH° = ? using Hess's Law and the three thermochemical equations below. Show work. (1) СаО(s) + 2 HС(аq) > СаСl,(аq) + H.О(1) (2) СаО(s) + H:0(1) > Са(ОН):(s) (3) Са(ОН):(s) watery Ca(ОH):(аq) AH° = - 186 kJ AH° = - 62 kJ AH° = - 13 kJ
A series of hypothetical thermochemical reactions with their corresponding enthalpies are given below. As) + X2(9) → AX2(9) A;Q8(g) + 5X2(9) → 3AX2(9) Q2(9) AH = - 394 KJ/mole + 4Q2X) AH = - 2,222 KJ/mole + ½ X2lg) → QzX AH = - 286 KJ/mole (A). Using the thermochemical equations above, the heat for the given overall reaction is Kilojoules per mole. Express answer in the NEAREST WHOLE NUMBER + 4Q2(9) > A,Q3(9) 3A(s) (B). If the overall thermochemical reaction given above has an entropy value of -270 Joules/Kelvin, its free energy (AG) at 100 degrees Celsius is in the NEAREST WHOLE NUMBER (C). If the overall thermochemical reaction given above has an entropy value of -270 Joules/Kelvin, then it will become spontaneous at temperatures above KiloJoules. Express answer Kelvin. Express answer in the NEAREST WHOLE NUMBER
The heat of combustion of undecane is – 7430.9 kJ/mol. Use this value to find the heat of formation of undecane. (You may also need to use the following tabulated thermochemical data. Enter an unrounded value.) Substance AH° (kJ - mol) 02 (9) Co, (9) -393.5 H,O(1) -285.8 C;H12(1) -173.5 C,H16 (1) -224.2 C3H20 (1) -274.7 C1H24 (1) -327.2 kJ/mol
Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g), by the reaction 2 SO2(g) + O2(g) → 2 SO3(g) The standard enthalpies of formation for SO2(g) and SO3(g) are AH; [SO2(g)] = -296.8 kJ/mol AH; [SO3(g)] = -395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 2.25 L of SO2(g) is converted to 2.25 L gas behavior. of SO3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C. Assume ideal AH= kJ
5(a)
Please answer the question in the image with details.