(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

A student runs two experiments with a constant-volume "bomb" calorimeter containing 1300.g of water (see sketch at right). First, a 6.000g tablet of benzoic acid C6H5CO2H is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of /26.454kJg .) The temperature of the water is observed to rise from 14.00°C to 39.98°C over a time of 14.9 minutes. Next, 5.570g of acetylene C2H2 are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 14.00°C to 60.18°C . Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. →+2C2H2g 5O2g + 4CO2g 2H2Og Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced students:…
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.
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
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).
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.
10. The following molar enthalpies of formation are given in kJ/mol: AHP[C;Hs(g)] = -104; AHP[CO2(g)] = -394; AHP[H;O(g)] = -242. (a) Calculate the molar heat of combustion of propane (C;Hs) according to the following equation: C;Hs(g) + 5 O2(g) → 3CO2(g) + 4H2O(g); (b) How many grams of propane gas must be combusted to provide enough thermal energy to heat 1.00 kg water from 22.0°C to 100.0°C? (Specific heat of water = 4.184 J/mol.K)
(b) The standard enthalpy change for the following reaction is -697 kJ at 298 K.2 Zn(s) + O2(g)2 ZnO(s)What is the standard heat of formation of ZnO(s)
use the standard reaction enthalpies given below to determine ▲H°rxn for the following reaction (see image)
（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?
The reaction between hydrogen and oxygen to yield water vapor has AH" = -1843 2H₂(g) + O₂(g) 2H₂O(g)AH <=-484kJ Part A What is the enthalpy change in kilojoules when 0.70 mol of H₂ reacts with 0.35 mol of O, to produce 0.70 mol of H₂ at constant pressure of 1.00 atm? Express your answer as a whole number. AH = Submit Part B W= Submit 1957 ΑΣΦ How much PV work is done in kilojoules for this reaction at constant pressure of 1.00 atm if the volume change is-9-2 L? Express your answer using two significant figures. 100 ΑΣΦΑ Part C Request Answer Request Answer kJ What is the value of AE for this reaction in kilojoules?
Consider the combustion of propane: C3H (9) + 50, (9)→ 3CO, (9) + 4H2 O(1) AH = -2221 kJ A balloon is being inflated to its full extent by heating the air inside it. In the final stages of this process, the volume of the balloon changes from 4.00 x 10° L to 4.50 x 10° L by the addition of 1.4 x 10 J energy as heat. Assume that all the heat comes from the combustion of propane. What mass of propane must be burned to furnish this amount of energy assuming the heat transfer process is 50.% efficient? Mass =