b My Questions | bartleby 101 Chem101 app.101edu.co Submit Question 25 of 29 Using the equations N2 (g) + 3 H2 (g) → 2 NH3 (g) AH° = -91.8 kJ/mol C(s) + 2 H2 (g) → H2 (g) + 2 C(s) + N2 (g) → 2 HCN (g) AH° = 270.3 kJ/mol Determine the enthalpy for the reaction CH4 (g) + NH3 (g) → HCN (g) + 3 H2 (g). → CH4 (g) AH° = -74.9 kJ/mol %3D | kJ/mol 1 3 4 8 9. +/- x 100 1:22 PM O Type here to search 12/9/2019 LO

b My Questions | bartleby 101 Chem101 app.101edu.co Submit Question 25 of 29 Using the equations N2 (g) + 3 H2 (g) → 2 NH3 (g) AH° = -91.8 kJ/mol C(s) + 2 H2 (g) → H2 (g) + 2 C(s) + N2 (g) → 2 HCN (g) AH° = 270.3 kJ/mol Determine the enthalpy for the reaction CH4 (g) + NH3 (g) → HCN (g) + 3 H2 (g). → CH4 (g) AH° = -74.9 kJ/mol %3D | kJ/mol 1 3 4 8 9. +/- x 100 1:22 PM O Type here to search 12/9/2019 LO

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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0.5Ν2 (NH3 (g) H2 (g) + 1.5H2 (g) +1.2502 (g) (g) +0.502 (g) → NH3 (g) NO 2NO H2O (1) (g) (g) ΔΗ1° Use the data from the table above to determine AH° for the reaction below, expressed in terms of ΔΗ1°, ΔΗ2°, and ΔΗ3°. N2 (g) + O2 (g) + 1.5H2O (I)|ΔΗ2° ΔΗ3°
Classify as exothermic or endothermic CH4(g) + 2 O2(g) + → 2 H2O(g) + CO2(g) + 889 kJ How do you know?
Are the reactions endothermic or exothermic? What observation supports this?
Using the equations H₂ (g) + Cl₂ (g) → 2 HCI (g) AH° = -184.6 kJ/mol C (s) + 2 Cl₂ (g) →→ CCI (g) AH° = -95.7 kJ/mol Determine the molar enthalpy (in kJ/mol) for the reaction C (s) + 4 HCI (g) → CCI (g) + 2 H₂ (g). 4 2
CH, (g) 20, (g) → CO, (g) + 2 H,O (g) + Exothermic or endothermic
What is the enthalpy change when 8.20 moles ammonium chloride form in the following equation? N2 (g) + 4 H2 (g) + Cl2 (g) --> 2 NH4Cl (s) Delta H = – 628.8 kJ a. – 2.58 x 103 kJ b. – 1.29 x 103 kJ c. + 314.4 kJ d. – 314.4 kJ e. – 628.8 kJ f. – 5.16 x 103 kJ g. none of these d. – 314.4 kJ
Determine AH for the following reaction, N₂(g) + 3 H₂(g) → 2 NH3(g) given the thermochemical equations below. N₂(g) + O₂(g) → 2 NO(g) 4 NH3(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g) 2 H₂(g) + O₂(g) → 2 H₂O(g) A. -1209.0 kj B.-1189.0 kJ OO OC. 150.3 k OD.-241.8 kJ E. -91.5 kJ Reset Selection o Ei C 6 AH = +180.8 kJ AH = -906.2 kJ ΔΗ = -483.6 k S IA
1/2 O2(g) + H2(g) → H2O(l) ΔHrxn = ?
The specific heat of substance C is 0.93 J/(g K) and that of substance D is 1.8 J/(g K). You are given an unknown that could be pure substance C, pure substance D, or a homogeneous mixture of C and D. In the lab you determine that it requires 23.3 J of heat energy to raise the temperature of a 25.0 g sample of the unknown by 1.0 K. What conclusions can you make about the identity of your unknown, from this data?
Question 9 of 24 Determine the enthalpy of reaction for HCI(g) + NaNO2(s) → HNO2(1) + NaCI(s) 2NACI(s) + H2O(1) → 2HCI(g) + Na20(s) AH° = -507.1 kJ/mol NO(g) + NO2(g) + Na,0(s) → 2NANO2(s) AH° = -427.0 kJ/mol NO(g) + NO2(g) → N20(g) + O2(g) AH° = -43.01 kJ/mol 2HNO2(1) → N,0(g) + O2(g) + H2O(1) AH° = +34.02 kJ/mol %3D %3D %3D Tap here or pull up for additional resources @ #3 24 & 2 8.