(a) The preparation of NO,(g) from N2(g) and O2(g) is an endothermic reaction: N2(8) + O2(g) –→ NO>(8) (unbalanced) The enthalpy change of reaction for the balanced equation (with lowest whole-number coefficients) is AH = 67.7 kJ. If 250 mL of N,(g) at 100°C and 3.50 atm and 450 mL of O,(g) at 100°C and 3.50 atm are mixed, what amount of heat is necessary to synthesize NO,(g)?

(a) The preparation of NO,(g) from N2(g) and O2(g) is an endothermic reaction: N2(8) + O2(g) –→ NO>(8) (unbalanced) The enthalpy change of reaction for the balanced equation (with lowest whole-number coefficients) is AH = 67.7 kJ. If 250 mL of N,(g) at 100°C and 3.50 atm and 450 mL of O,(g) at 100°C and 3.50 atm are mixed, what amount of heat is necessary to synthesize NO,(g)?

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

1a only
ulate het reaction enthalpy O O D Dwayne V 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,O(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 olb 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. Explanation Check O 2021 McGraw Hill LLC. All Rights Reserved. Terms of UseI Privacy Center Accessibility 4:25 AM ENG 12/14/2021 35°F Clear O Type here to search
When chemical A and chemical B are mixed together, and endothermic reaction below occurs:4A(aq) + 3B(s) --> 2C(aq)To find the enthalpy of this reaction, a scientist pours 155 mL of a 0.33 M solution A into abeaker and measures the temperature to be 20.1 ̊C. To this same beaker the scientist thenadds 3.75 g of substance B with stirring (molar mass of B is 33 g/mol), and finds thetemperature to now be 16.3 ̊C. Calculate the molar enthalpy of this reaction for every mole ofC produced.
Butane, C4H10, is widely used as a fuel for disposable lighters When one mole of butane is burned in oxygen, carbon dioxide and steam are formed and 2654.3382 kJ of heat are evolved.. C4H10 (9) + O₂(g) → 4CO₂(g) +5H₂O(1) The standard enthalpies of formation of CO₂ and H₂O are: CO2(g)=-394.87 kJ/mol H₂O(1)=-285.59 kJ/mol Calculate the standard heat of formation of butane. (Round answer to the second decimal place)
In the recovery of iron from iron ore, the reduction of the ore is actually accomplished by reactions involving carbon monoxide. Use the following thermochemical equations, Fe,O3(s) + 3CO(g) 2Fe(s) + 3CO,(g) AH° = - 28 kJ 3Fc,O3() + CO(g) 2Fe3O4() + CO,(g) AH = -59 kJ FezO4(s) + CO(g) 3FcO(s) + CO,(g) AH° = +38 kJ to calculate AH° for the reaction FeO() + CO(g) Fe(s) + CO2(g) AH° = i kJ
Thermochemistry and Stoichiometry
2. (a) 36 mL of 1.0M hydrochloric acid is react with a solution of sodium hydroxide of the concentration 1.6M and volume 15 mL in a coffee cup calorimeter. It is noted that the temperature of both solutions before the reaction is 27.5 °C. After the reaction, the temperature of the solution raise to 35.0 °C. Calculate heat of neutralization for the reaction.(cw = 4.18 Jgl°C', Density of solution: 1gmL').
Calculate the standard enthalpy of formation for C3H6O (l) from its combustion using the following data: Enthalpy of this combustion is -1793 kJ ( you must write a balanced reaction first).
Phenol undergoes combustion in oxygen to produce carbon dioxide gas and The standard heat of combustion of phenol, CgH,OH(s), is -3054 kJ/mol. AH?[CO,(g)] = -393.5 kJ/mol and AHÇ [H,O(1)] = -285.8 kJ/mol, what is t %3D enthalpy of formation of phenol? +164.4 kj/mol +328.8 kj/mol -164.4 kj/mol -328.8 kj/mol
4) Consider the thermochemical equation below. What mass of HgO must decompose to consume 400.0 kJ of heat? 2 HgO (s) → 2 Hg (1)+ O2(g) AH°rxn =+ 181.4 kJ (1) 5) Write the standard formation reaction for KAI(SO4)2(s). (1) 3 CO2 (g). (1) -393.5 kJ/mol 2 Cr (s) + 3 CO (ag) -110.5 kJ/mol Cr2O3 (s) 6) Consider the reaction 0.0 kJ/mol AH°f = -1139.7 kJ/mol Calculate AH°rxn.
Incorrect. What is the heat of formation of elements in their standard states? Did you use the correct equation of products minus reactants? The amino acid glycine, C2H5NO2, is one of the compounds used by the body to make proteins. The equation for its combustion is 4C2H5NO2(s) + 902(g) → 8CO2(g) +10H20(1) +2N2(g) For each mole of glycine that burns, 973.49 kJ of heat is liberated. Use this information, plus values of AHº for the products of combustion, to calculate AH° for glycine. AH = kJ/mol eTextbook and Media Hint Solution 935 pm A 27°C Haze O G 10 ENG Type here to search 15/03/2022 1080 acer Insert Delete F11 F12 Prt Sc Pause Br F8 F9 F10 F7 NumLk F5 F3 Esc Coca) Backsp * 8 8 # 2$ % & 9 @ € 7 1 2 3 !!
use the standard reaction enthalpies given below to determine ▲H°rxn for the following reaction (see image)