stion 5 The enthalpy of combustion under a pressure of one atmosphere of one mole of methane at 298K is -212.8 kJ. CH4 (g)+202 (g)>CO2(g) +2H2O(1) a. Calculate the average molecular speed of CO2 gas at 298 K (C=12, O–16) b. Calculate the standard enthalpy of formation of the methane at 298K ;AĦ°(methane(g),298K). Given: A CH,0(); 298K) =-68.33 kJ/mol); A(CO2 (3); 298K) = -94.25 kJ/mol) %3D

stion 5 The enthalpy of combustion under a pressure of one atmosphere of one mole of methane at 298K is -212.8 kJ. CH4 (g)+202 (g)>CO2(g) +2H2O(1) a. Calculate the average molecular speed of CO2 gas at 298 K (C=12, O–16) b. Calculate the standard enthalpy of formation of the methane at 298K ;AĦ°(methane(g),298K). Given: A CH,0(); 298K) =-68.33 kJ/mol); A(CO2 (3); 298K) = -94.25 kJ/mol) %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...

See similar textbooks

Similar questions

The gas cyclopropane, C3H6(g), can be used in welding. When cyclopropane is burned in oxygen, the reaction is: 2 C3H6(g) + 9 O₂(g)6 CO₂(g) + 6 H₂O(g) (a) Using the following data, calculate AH° for this reaction. AH kJ mol-¹: C3H6(g) = 53.3; CO₂(g) = -393.5; H₂O(g) = -241.8 4 AH° = kj (b) Calculate the total heat capacity of 6 mol of CO₂(g) and 6 mol of H₂O(g), using CcO₂(g) = 37.1 J K-1 mol-¹ and CH₂O(g) = 33.6 J K-¹ mol-¹. C = JK-1 (c) When this reaction is carried out in an open flame, almost all the heat produced in part (a) goes to raise the temperature of the products. Assuming that the reactants are at 25°C, calculate the maximum flame temperature that is attainable in an open flame burning cyclopropane in oxygen. The actual flame temperature would be lower than this because heat is lost to the surroundings. Maximum temperature °℃
Use Hess's law to Calculate the AH of the reaction C₂H₂(g) + H₂(g) → C₂H,(g) from the following data. Identify the "manipulation" for each reaction C₂H₂(g) + 3 O₂(g) → 2 CO₂(g) + 2 H₂O(1) C₂H₂(g) + 3% O₂(g) 2 CO₂(g) + 3 H₂O(1) H₂(g) + O₂(g) → H₂O(1) ΔΗ = -1411 kJ AH = -1560 kJ AH = -285.8 kJ
Consider the following reaction: CH4 (9) + 20, (g) → CO2(g) + 2H,0(1) AH=-891 kJ a. Calculate the enthalpy change if 2.59 g methane is burned in excess oxygen. Enthalpy change = kJ b. Calculate the enthalpy change if 3.04 × 10° L methane gas at 737 torr and 25°C is burned in excess oxygen. Enthalpy change = kJ
and 2 Enthalpy #1.30 enoindice pled TT 2010 2D49.bs 22) When 1 mole of Fe2O3(s) reacts with H₂(g) to form Fe(s) and H2O(g) according to the following equation, 98.8 kJ of energy are absorbed. (6 Fe2O3(s) + 3 H2(g) → 2 Fe(s) + 3 H₂O(g) (pp) (20/d4 (pm) $40 D Reaclanis 13:48 SH Products endothermic, A endothermic, B (2) exothermic, A exothermic, B nad W (21 Enthalpy MOMS. Reactants Products (A) (B) Is the reaction endothermic or exothermic, and which of the enthalpy diagrams above represents grow olor and to noin (01 this reaction? SH GH TH A HOMH X HILD 08.10 Page 6 of 8
For a particular isomer of Cg H₁g, the combustion reaction produces 5108.7 kJ of heat per mole of C, H₁g (g) consumed, under standard conditions. 25 Cg H18 (8) + O₂(g) →→→ 8 CO₂(g) + 9 H₂O(g) What is the standard enthalpy of formation of this isomer of Cg H₁g (g)? AH; = $ V T B MacBook Air Y H & 7 8 AH-5108.7 kJ/mol 18 N M K 1 38 kJ/mol
Question 6 Which of the following graph represents the change in the Potential Energy (PE) of the particles in the system when the substances undergoes the change corresponding to path I? PE с A D B Pressure (atm) A 10³ 10² 10¹ P 10-1 10-² 10-3 Т IV PE 20 ||| || 40 B C PE Т TREF 60 Temperature (K) 80 Т 100 PE D Т
What is the standard enthalpy change for the reaction: 2C5H10(1) + 15O2(g) → 10CO2(g) + 10H20(1); where C5H10(1) AH°f = –605.0 kJ/mol; CO2(g) AH°f = -393.5 kJ/mol; H2O(1) AH°F - 285.8 kJ/mol. O a. -5583 kJ O b. -5783 kJ O C. -5383 kJ O d. -5183 kJ e. -4983 kJ
Determine the enthalpy for the production of 5.0 g of H2 in the following target equation, making use of the known equations given below. CH4 (g) + NH3 (g) → HCN(g) + 3H2 (g) Using the following given equations: N2 (g)+3H2 (g) → 2NH3 (g) ΔH=− 91.8kJ C(s)+2H2 (g) → CH4 (g) ΔH=− 74.9kJ H2(g) + 2C(s) + N2 (g) → 2HCN(g) ΔH= + 270.3 kJ
Calculate the standard enthalpy of formation of NH, 13(g) + N2c9) 342(9) 2NH. '3(g) AH = -92.2kJ/mol 3H, Select one: а. -36.1 b. -92.2 C. -46.1 d. -31.1 e. -41.1
The internal pressure of a gas, π = au dv)T' is a measure of intermolecular forces, because it indicates a change in internal energy as the molecules get closer or further apart, without temperature changing. = a Calculate the change in internal 1 Vm T energy, AU, when 1.5 mols of acetone (a = 16 l² atm/mo1²), expands from 2 liters to 5 liters at a constant temperature. ii) Would this change in internal energy be greater or smaller for an ideal gas? Why? i) Using the van der Waals equation of state, T = au
HCl(g) Suppose we redefine the standard state as P = 4 atm . Find the new standard AG; values of the following substances. AG; = - 78.3 J/mol Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining Part B N20 (g) Express your answer using four significant figures. ΑΣΦ AG; = J/mol Submit Request Answer Part C H(g) Express your answer using four significant figures. ΑΣΦ AG; = J/mol Submit Request Answer
The chemical equation for photosynthesis is as follows: 6 CO2 + 6 H2O → CoH1206 ( + 6 02 Every year, the mass of carbon dioxide used by this reaction on a small island is 2.85 x 10 kg. What is the annual enthalpy change resulting from photosynthesis on the island? Compound AH° (kJ/mol) -1268 02 CO2 -393.5 HO -285.8 O 303 x 10 k Q 2.54 x 10 k O 254 x 10 k O 153x 10' k 0412x 10 k