A scientist measures the standard enthalpy change for the following reaction to be -876.5 kJ: 2NH3(g) + 3 N₂O(g) 4N₂(g) + 3 H₂O(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of NH3(g) is Submit Answer Use the References to access important values if needed for this question. 1 question attempt remaining kJ/mol.

A scientist measures the standard enthalpy change for the following reaction to be -876.5 kJ: 2NH3(g) + 3 N₂O(g) 4N₂(g) + 3 H₂O(g) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of NH3(g) is Submit Answer Use the References to access important values if needed for this question. 1 question attempt remaining kJ/mol.

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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A scientist measures the standard enthalpy change for the following reaction to be - 778.8 kJ: 2NO(g) + 2H₂ (g) → N₂(g) + 2H₂O (1) Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of H₂O(l) is kJ/mol. Substance AH (kJ/mol) NO(g) H₂(g) N₂ (9) Submit Answer 90.3 0.0 0.0 Retry Entire Group 9 more group attempts remaining
QUESTION 32 Using the table of enthalpies of formation below, calculate AHrxn (in kJ) for the following reaction. 2 C6H1206 (s) C12H22011 (s) + H20 () Report your answer to one decimal place. Do not input a unit. If your value is negative, please insert a (-) sign. ΔΗΡη-ΣΠΔΗ fproducts )-ΣηΔΗfreactants) %3D Compound AHf (kJ/mol) C12H22011 (s) -2226.1 H20 (1) -285.8 C6H1206 (s) -1273.3
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Suppose that the molar enthalpy of a reaction is -240 kJ/mol and 44.0 grams of X (MW = 14) reacted. How many joules of heat are released by the reaction? Report your answer to the appropriate number of significant figures in the first blank below and the correct units in the second blank below.
Using the standard enthalpies of formation, calculate the standard enthalpy change for the overall reaction that occurs when ammonia is burned in air to form nitrogen dioxide and water. 4NH,(g) +70,,g) 4NO,(g) 6H.O(1) AH of NH₂(g) = -46 kJ/mol AH of NO(g) = 34 kJ/mol, AH of H₂O() = -286 kJ mol f f 5 O-360 kJ -1396 kJ O-1496 kJ O -1496 kJ Question 9 - 1 Not yet answered - Flag question
目 Re [References] Use the References to access important values if needed for this question. Using standard heats of formation, calculate the standard enthalpy change for the following reaction. 2H202(1)2H20(1) + O2(g) ANSWER: kJ Submit Answer Try Another Version 1 item attempt remaining
Simple Algorithm: Solve the following problems. Write your answer on the space provided. Show your complete solutions. For your final answer, report correct significant figures and rounding off (Follow the conventional). 2. The value of ΔH0 for the reaction CH3OH(l) → CO(g) + 2H2(g) is +128.1 kJ. Determine the heat consumed when 5.75 g of CO(g) is formed.
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mation [References] INTERACTIVE EXAMPLE Using Enthalpies of Formation Nitroglycerin is a powerful explosive that forms four different gases when detonated: 2 C3H;(NO3)3(t) → 3 N2(g) + ½ O2(g) + 6 CO,(g) + 5 H20(g) -> Calculate the enthalpy change that occurs when 18.0 g of nitroglycerin is detonated. The standard enthalpies of formation are shown below. AHF (kJ/mol) C3H5(NO3)3(t) -364 CO2(g) -393.5 H,O(g) -241.8 kJ Submit Show Approach Show Tutor Steps