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 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-1¹. 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 = °℃

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 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-1¹. 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 = °℃

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

THERMODYNAMICS: Calculate the value of AH (in kJ) for the reaction, 2AR3 (g) + Q (s) → A2R4 (g) + QR2 (s) given the following hypothetical thermochemical equations: AH = -84 kJ AH = -151.3 kJ AH = -537.5 kJ 2AR3 (g) + 2AX (g) → A2R4 (g) + 2XAR (g) AX (g) + ½R2 (g) → XAR (g) Q (s) + R2 (g) → QR2 (s) (Round off final answer to ONE decimal place) Round your answer to 1 decimal place.
9) The following thermochemical equation is for the reaction of ammonia(g) with oxygen(g) to form nitrogen monoxide(g) and water(g): 4 NH3(g) + 5 O₂(g) → 4 NO(g) + 6 H₂O(g) 8100.0 25228 AH = -905 kJ 2730.0 How many grams of NH3(g) would have to react with excess O₂(g) to produce 58.6 kJ of energy?
What quantity of heat (in kJ) will be released if 0.2921 mol of NH3 are mixed with 0.200 mol of O₂ in the following chemical reaction? 4 NH3(g) + O₂ (g) → 2 N₂H4 (g) + 2 H₂O (g) AH° = -286 kJ/mol
Given the following thermochemical data at 25°C and 1 atm pressure, 3/2 O2(g) + 2B(s) → B2O3(s); AH° =-1264 kJ; O3(g) + 2B(s) –→ B2O3(s); AH° = - 1406 kJ; determine AH° for the following reaction at 25°C and 1 atm pressure. 302(g) → 203(g) a. +284 kJ/mol b. -2670 kJ/mol C. -980 kJ/mol d. +980 kJ/mol O e. -284 kJ/mol
When 56.8 g of lead reacts with 3.50 L of oxygen gas, measured at 1.00 atm and 25.0°C, 60.1 kJ of heat is released at constant pressure. What is AH° for this reaction? (R = 0.0821 L. atm/(K• mol)) %3D 2Pb(s) + O2(g) → 2PBO(s) O a. -8.7 x 101 kJ b. -6.01 x 101 kJ O C. -4.39 x 102 kJ O d. -2.19 x 102 kJ O e. -5.2 x 102 kJ
Calcium carbonate can be decomposed upon applying heat with the following equation CaCO3(s) → CaO(s) + CO2(g) ΔH = +179.5kJ How much heat will be needed to decompose 30 g of calcium carbonate? AND What size container will be required (in L) to contain the carbon dioxide generated at 25ºC and 1.2 atm?
If a 136.51 g Al rod (c = 0.900 J/g ° C) is at 100.0 ° C and placed into 250.0 g of water at 21.8 ° C, what is the temperature of the system (rod + water) at equilibrium assuming no losses to the surroundings? Assume the specific heat of water to be 4.18 J/g ° C.
Zinc metal reacts with hydrochloric acid according to the following balanced equation.Zn(s)+2HCl(aq)→ZnCl2(aq)+H2(g)When 0.111 g of Zn(s) is combined with enough HCl to make 53.8 mL of solution in a coffee-cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 22.0 ∘C to 24.0 ∘C.Find ΔHrxn for this reaction as written. (Use 1.0 g/mL for the density of the solution and 4.18 J/g⋅∘C as the specific heat capacity.)
Liquid trinitroglycerin (C3H5N3O9) has been widely used as an explosive and as a medication to relieve angina. The enthalpy of decomposition (ΔHdec) for C3H5N3O9 to form N2(g), CO2(g), H2O(l), and O2(g) is -1541.4 kJ/mol. 1. Write the thermochemical equation for the decomposition of 1 mole of trinitroglycerin. 2. Calculate the standard heat of formation (ΔHf) for C3H5N3O9. 3. A standard does of C3H5N3O9 for relief of angina is 0.60 mg. If a sample is eventually oxidized completely, how many calories are released?
Zinc metal reacts with hydrochloric acid according to the following balanced equation: Zn(s) + 2HCl(aq)-> ZnCl2(aq) + H2(g) When 0.115g of Zn(s) is combined with enough HCI to make 52.6mL of solution in a coffee - cup calorimeter, all of the zinc reacts, raising the temperature of the solution from 21.5 °C to 24.7 °C. Part A Find \Delta Hrxn for this reaction as written. (Use 1.00 g/mL for the density of the solution and 4.18 J/(g°C) as the specific heat capacity.)
A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 72.8 mL water (where X is a hypothetical metal): X + 2 HCI → XCI2 + H2 In this process, the water temperature rose from 25.0 °C to 31.5 °C. If 0.00585 mol of "X" was consumed during the reaction, what is A,H of this reaction in kJ mol-1 with respect to "X"? The specific heat of water is 4.184 J g-1 °C-1
In a coffee cup calorimeter, 3.00 g of NaOH (molar mass 40.00g/mol) was mixed with 75.0 mL of 1.00M HNO3. If the initial temperature of the HNO3 was 31.3°C and the final temperature of the solution was 22.3°C, determine AH for the reaction in kJ/mol. NaOH(s) + HNO3(aq) ===> NaNO3(aq) + H2O) The density and the specific heat capacity of the resulting solution are 1.00 g/ml and 4.18 J/°C.g, respectively. Units do not need to be typed, simply enter the correct number. If the sign of AH is negative put a negative sign (-) in the answer. Answer: