Melted methane was ignited and used to heat water in a thin metal container. After a short period of time, the methane was extinguished and final measurements were made. = 7.52 g = 7.20 g Mass of methane before burning Mass of methane after burning Mass of water in container Initial temperature of water = 140.0 g = 10.0°C Final temperature of water = 32.0°C a) Using this data, calculate the heat of combustion of methane in kJ/mol. Assume that all the heat from the methane was absorbed by the water b) Write the thermochemical equation for the complete combustion of methane.

Use the References to access important values if needed for this question Ethanol, C2H0, is most often blended with gasoline - usually as a 10 percent mix - to create a fuel called gasohol. Ethanol is a renewable resource and ethanol-blended fuels, like gasohol, appear to bum more efficiently in internal combustion engines. The combustion enthalpy of ethanol is 1366.9 kJ/mol The combustion enthalpy of 2-methylpentane, C6H14 is 4.157x103 kJ/mol. Calculate the energy released during the complete combustion of 382 g 2-methylpentane kJ Assuming the same efficiency, would 382 g ethanol provide more, less, or the same quantity of energy as 382 g 2-methylpentane? | Submit Answer Retry Entire Group 8 more group attempts remaining

Calculate the energy required to heat 403.0 mg of water from 36.8 °C to 57.0 °C. Assume the specific heat capacity of water under these conditions is 4.18 J-g .K . Be sure your answer has the correct number of significant digits. 0 0x10 ロ・ロ X μ 00 4 S

A chemist carefully measures the amount of heat needed to raise the temperature of a 399.0 g sample of a pure substance from 4.1 °C to 19.7°C. The experiment shows that 865. J of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 3 significant digits. -1 -1 J.g •K x10 Submit Assignme Continue 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center | Accessibili I IMG-6111.jpg IMG-6110.jpg IMG-6109.jpg IMG-6108.jpg IMG-6107.jpg MacBook Air 80 DII DD F2 F3 F4 F5 F6 F7 F8 F9 F10 F11 @ # $ % & 2 3 4 5 6 7 8 9

Review | Constants | Periodic Table To determine whether a shiny gold-colored rock is actually gold, a chemistry student decides to measure its heat çapacity. She first weighs the rock and finds it has a mass of 4.7 g. She then finds that upon absorption of 52.7 J of heat, the temperature of the rock rises from 25 °C to 57 °C. Find the specific heat capacity of the substance composing the rock. gh Expréss the specific heat capacity in joules per gram-Celsius to two decimal places. ? J Cs = g.°C Submit Request Answer Part B Complete previous part(s) Part C A 55.0 g aluminum block initially at 27.5 °C absorbs 725 J of heat. What is the final temperature of the aluminum? Express your answer in degrees Celsius to one decimal place. VO AEO T = P Pearson °C . All rights reserved. Terms of Use | Privacy Policy Permissions Contact Us |

Calculate the energy required to heat 718.0 mg of water from 46.0 °C to 56.7 °C. Assume the specific heat capacity of water under these conditions is -1 -1 4.18 J∙g¯¹·K-¹ Be sure your answer has the correct number of significant digits. 0 x10 X μ 010 ? 00. 18 Ar

A 28.5 g piece of gold is heated and then allowed to cool. What is the change in temperature (°C) if the gold releases 0.226 kJ of heat as it cools? The molar heat capacity of gold is 25.4 J/mol･°C.

A chemist carefully measures the amount of heat needed to raise the temperature of a 0.57 kg sample of a pure substance from 18.0 °C to 35.9 °C. The experiment shows that 19. kJ of heat are needed. What can the chemist report for the specific heat capacity of the substance? Round your answer to 2 significant digits. - 1 - 1 •K J. g x10

Can you explain where did I go wrong, I keep getting the same answer.