Given the following data2 CIF (g) + O2 (9) → Cl2 O(g) + F20(g)2 CIF3 (g) + 202(9) → Cl2 0(9) + 3F20(g)2F2 (9) + O2(9) - 2F20(g)AH = 167.4 kJAH= 341.4 kJAH = -43.4 kJcalculate A H for the reactionCIF(g)+ F2(g) CIF3 (g)AH =kJ

Given the following data 2 CIF (g) + O2 (9) → Cl2 O(g) + F20(g) 2 CIF3 (g) + 202(9) → Cl2 O(g) + 3F20(g) 2F2 (9) + O2 (9) –→ 2F20(g) AH = 167.4 kJ AH = 341.4 k) AH = -43.4 k) calculate A H for the reaction CIF(g) + F2 (g) → CIF3 (g) ΔΗ= kJ %3D

Given the following data 2 CIF (g) + O2 (9) → Cl2 O(g) + F20(g) 2 CIF3 (g) + 202(9) → Cl2 O(g) + 3F20(g) 2F2 (9) + O2 (9) –→ 2F20(g) AH = 167.4 kJ AH = 341.4 k) AH = -43.4 k) calculate A H for the reaction CIF(g) + F2 (g) → CIF3 (g) ΔΗ= kJ %3D

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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Using Appendix II from your book, determine the heats of reaction (DHrxn) based on the equation below: 2502(g) + O2(g) + 2H2O(1) → 2H2SO4(aq) DHrxn
Consider these reactions: Reaction 1: H2(g)+Cl2(g)⟶2HCl(g)ΔH=−184.6 kJ Reaction 2: 2OF2(g)⟶O2(g)+2 F2(g)ΔH=−49.4 kJ Reaction 3: N2(g)+2O2(g)⟶2NO2(g)ΔH=+66.4 kJ Use Reaction 1. Determine the mass, in grams, of chlorine gas consumed (with excess H2) when 1,530.0 kJ of energy is released from the system.
Using the equations N₂ (g) + 3 H₂ (g) → 2 NH₂ (9) AH° = -91.8 kJ/mol C(s) + 2 H₂(g) →→ CH₂ (g) AH° = -74.9 kJ/mol H₂(g) + 2 C(s) + N₂ (g) → 2 HCN (g) AH° = 270.3 kJ/mol - Determine the enthalpy (in kJ/mol) for the reaction CH₂(g) + NH₂(g) → HCN (g) + 3 H₂ (g).
3) How many liters of combusted propane (C3H8; 44 g/mol) are required to heat a 100 kg steel pipe (specific heat of steel is 0.420 J/g°C), from room temperature (20°C) to its melting point of 1300°C? The density of propane is 0.493 g/mL.C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l) ΔH=–2220 kJ /mol 4) How much energy is required to produce 1.9 grams of glucose (C6H12O6; 180 g/mol) from CO2 and H2O. Use the following combustion equation to help you answer the question?6CO2(g) + 6H2O(l) → C6H12O6(s) + 6O2(g) ΔH= 2900kJ 19) What volume of 0.12 M Na2SO4 will be required to react with 35 mL of 0.05 M CrCl6? 24) In an experiment when 100 g of C3H8 is combusted, 30 g of carbon dioxide resulted. What was the percent yield for the reaction?
Calculate AH for the following reaction, given the data in the table below: H2SO4() → So:(g) + H2O(g) AH = ??? kJ/mol H2S(g) +202(g)→ H2SO4(1) AH = -749.7 kJ H,S(g) + 202(g) → SO3(g) + H2O(1) AH = -355.0 kJ H20(1) H20(g) AH = +53.95 kJ
Which reaction would it be possible to calculate (Triangle H)?
#3
Consider these reactions: Reaction 1: H2(g) + Cl2(g) 2HCl(9) AH = -184.6 kJ Reaction 2: 20F2(g) → O2(g) +2F2(g) AH=-49.4 kJ Reaction 3: Na (g) +202 (9) 2NO2(g) AH = +66.4 kJ Use Reaction 1. Determine the mass, in grams, of chlorine gas consumed (with excess H₂) when 1,409.0 kJ of energy is released from the system. Round to the nearest whole number .
Consider the problem below: (Equation 1) CaCO3(s) → CaO(s) + CO2(g) AH = 178 kJ/mol (Equation 2) CO(g) + O3(g) → CO2(9) + 20(g) AH = -425.7 kJ/mol %3D (Equation 3) 2 O(a) → O2(a) AH = -498 kJ/mol (Equation 4) CaCO3(s) + O2(9) → CaO(s) + CO(g) + O3(9) AH = ??????? The AH for equation 4 is: (express in kJ) Screen reader version Consider the problem below: (Equation 1) C a CO3(s) arrow Ca Ols) + CO22) AH = 178 kJ/mol (Equation 2) CO(g) + O3(g) arrow CO2(g) + 20(2) AH = minus 425.7 kJ/mol (Equation 3) 2 O(2) arrow O2(e) AH = minus 498 kJ/mol (Equation 4) C a CO3(s) + O2(g) arrow C a O(s) + C Og) + O3(2) AH = ??????? %3D The AH for equation 4 is: _(express in kJ)
Calculate AH for the following reaction, given the data in the table below: 4N204 (2) →2N20g) + 4NO2 (g) + 302 AH = ??? kJ/mol 2NO2 (e) + 2NO() +O2 (g)→2N2O4 (g) AH = -396.81 kJ 4NO+ 2N2Og) + 502 (g)→4N2O4 (g) AH = -398.88 kJ 2NO + O2 ()→N2O4 (3) AH = -173.09 kJ