It is sometimes appropriate to express the temperature dependence of the heat capacity by the empirical expression Cp,m =a+BT+yT² . Use this expression to estimate the standard enthalpy of combustion of methane at 350 K. Use the standard enthalpy tables in the back of your book in the "Resource Section" (you can also look this up on the internet) and the following data for the empirical constants: 2C.7 CH4 (g) CO₂ (g) O₂ (g) H₂O (1) al(J K-¹ mol-¹) 14.16 26.86 25.72 30.36 B/(mJ K¹ mol-¹) 75.5 6.97 12.98 9.61 Yl(@J K- mol) -17.99 -0.82 -3.868 1.184

It is sometimes appropriate to express the temperature dependence of the heat capacity by the empirical expression Cp,m =a+BT+yT² . Use this expression to estimate the standard enthalpy of combustion of methane at 350 K. Use the standard enthalpy tables in the back of your book in the "Resource Section" (you can also look this up on the internet) and the following data for the empirical constants: 2C.7 CH4 (g) CO₂ (g) O₂ (g) H₂O (1) al(J K-¹ mol-¹) 14.16 26.86 25.72 30.36 B/(mJ K¹ mol-¹) 75.5 6.97 12.98 9.61 Yl(@J K- mol) -17.99 -0.82 -3.868 1.184

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) What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by 0.68 oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) b) What is the standard enthalpy of reaction per mole of KOH when 50.00 cm3 of 1.0 moldm-3 of Nitric Acid (HNO3) and 50.00 cm3 of 1.0 moldm-3 of Potassium Hydroxide (KOH) are mixed? According to your simulation, the temperature rose by __6.81__ oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1)
Given, Salt: FeCl2 Mass of salt: 4.843 Mass of water: 45.1 Initial temp: 20.00 Final Temp: 32.663239 The sample of this salt is placed in water at a constant pressure calorimeter with a heat capacity of 35.5 J/℃. Determine the enthalpy change for the dissociation of this salt, ΔHdiss. 1. Σ qi = qreaction + qsolution + qcalorimeter = 0 Calculate the heat of the solution. 2. Calculate the heat of the calorimeter. 3. Calculate the heat of the reaction. 4. How many moles of your salt dissolved? 5. Calculate the value of ΔHdiss.
Consider 2.00 mol of an ideal gas with a constant-volume molar specific heat of 26.0 J/(mol K), an initial temperature of 26.3 °C, and an initial pressure of 5.810 x 104 Pa. The state of the gas is changed to a final temperature of 46.1 C and a final pressure of 3.090 × 104 Pa. The gas constant is 8.31 J/(mol-K). What is the change in the entropy AS of the gas during this process? AS = J/K
a) What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by 0.68 oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) Show your working below:
The table provides molar heat capacities (Cm) of selected metals with the units of joules per mole-kelvin. Heat capacity is also frequently given as specific heat capacity (C₂) with the units joules per gram-degree Celsius. Using the values provided in the table, convert the molar heat capacity (Cm) of zinc to the specific heat capacity (C₂) of zinc. C₁ = J/(g. °C) Molar heat capacity (Cm) of selected metals at 25 °C Element aluminum copper iron lead magnesium nickel titanium zinc Cm (J/(mol-K)) 24.20 24.44 25.10 26.84 24.87 26.07 25.06 25.39
In this experiment you will place a sample of your salt in water in a constant pressure calorimeter with a heat capacity of 29.4 J/℃. You will determine the enthalpy change for the dissociation of your salt, delta Hdiss or rxn. A sample of 4.368 grams of the salt SrCl2 was placed in 35.5 g water, the initial temperature was 20.00℃ and the final temperature was 27.086365℃. What is the total mass of the solution in sig figs? mass = 4.368 g + 35.5 g = 39.868 g a. 39.8 g b. 40 g c. 39 g d. 39.868 g e. 4.0 x 10^1 g f. 39.87 g g. 39.86 g h. 39.9 g i. none of these
PCI5(s) can be prepared by the reaction PCI3(1) + Cl2(g) - PCI5(s). Calculate the enthalpy change (in kJ) that accompanies the production of 100.0 g of PCI5(s) by the above reaction, given the following data. P4(s) + 6 Cl2(g) - 4 PC|3(1) AH° = -1280 kJ per mole of P4(s) %3D P4(s) + 10 Cl2(g) – 4 PCI5(s) ΔΗ AH° = -1774 kJ per mole of P4(s) +59.3 -59.3 +124 -124 -258
Measurements show that the enthalpy of a mixture of gaseous reactants decreases by 253. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 149. kJ of work is done on the mixture during the reaction. Calculate the change in energy of the gas mixture during the reaction. Round your answer to 3 |kJ х10 significant digits. exothermic Is the reaction exothermic or endothermic? endothermic
When 1786 J1786 J of heat energy is added to 45.9 g45.9 g of hexane, C6H14,C6H14, the temperature increases by 17.2 ∘C.17.2 ∘C. Calculate the molar heat capacity of C6H14.C6H14. ?P=CP= J/(mol⋅∘C)