19, Consider the following information about the combustion of octane (CaHis), the principle component of gasoline. 2C8HI8()+25O2(g) 16CO2(g) + 18H20() AH -1080 k If 1.14 g of octane are burned in a calorimeter surrounded by 1.0 kg of water, what is the temperature change of the water? The specific heat of water is 4.184 J/g°C. a. 1.3°C b. 2.6°C c. -1.3°C d. -2.6°C

19, Consider the following information about the combustion of octane (CaHis), the principle component of gasoline. 2C8HI8()+25O2(g) 16CO2(g) + 18H20() AH -1080 k If 1.14 g of octane are burned in a calorimeter surrounded by 1.0 kg of water, what is the temperature change of the water? The specific heat of water is 4.184 J/g°C. a. 1.3°C b. 2.6°C c. -1.3°C d. -2.6°C

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

please dont round along the way to solving
It is recommended that the average daily intake of glucose for humans is not to exceed 32.5 g of glucose (C6H12O6). The balanced chemical equation for the combustion of glucose is shown below. C6H12O6(aq) + 6 O₂(g) → 6 CO₂(g) + 6 H₂O (1) AH rxn= -1273.3 kJ/mol How much heat is released when 55.5 g of oxygen are combusted with glucose as shown in the reaction. above? Use the provided Periodic Table for any calculations involving elements. Report your answer to a single decimal place and report proper units with your answer.
The combustion of a sample of isoctane vapor at constant pressure raises the temperature of a calorimeter and its contents by 0.400 °C. The heat capacity of the calorimeter and water combined is 2.48 kJ/°C. How much heat was produced from the combustion? (variations of formula: c=q/mat)
Octane (C8H18) is a component of gasoline that burns according to the following equation: C8H18 (l) + 25/2 O2 (g) ------> 8 CO2 (g) + 9 H2O (g) ΔHorxn = - 5074.1 kJ What mass of octane (in g) is required to produce 5830 kJ of heat?
A 6.55 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. Wht is the change in teperature in celcios inside the calometer? was the dissolution process endothermic or exothermic? how much heat, in J, was hained b the solution? assume the specific heat of the solution is the same as water, 4.184 J/g. celcius
5(a)
What is the mas of natural gas (CH4) must you burn to emit 276 kJ of heat?