HELP ME PLEASE!!!! REFER TO IMAGE ATTACHED SHOW ALL WORK PLEASE MUST SHOW ALL WORK AND UNITS1. The temperature of a 98.7 g piece of metal increases from 17.0 °Cto 31.0 °C when the metal absorbs 705 J of heat. What is the specificheat of the metal?2. The initial temperature of the water in a constant-pressurecalorimeter is 25.0 °C. A reaction takes place in the calorimeter, andthe temperature rises to 79.0 °C. The calorimeter contains 858 g ofwater, which has a specific heat of 4.18 J/g °C. Calculate the enthalpychange during this reaction.3. C3H3 (g) + O2 (g) --> CO2 (g) + H20 (1) + 2220 KJ/molCalculate the amount of heat required to burn 0.56 moles of C3H3.(must balance the equation first)4. Calculate the amount of heat absorbed to liquefy 42.8 g ofmethanol (CH,0) at its melting point. The molar heat of fusion formethanol is 3.16 KJ/mol.5. How much heat (in KJ) is absorbed when 75.7 g of methanol(CH,O) is converted to gas? Heat of vaporization for methanol is 35.2KJ/mol.

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1. The temperature of a 98.7 g piece of metal increases from 17.0 °C to 31.0 °C when the metal absorbs 705 J of heat. What is the specific heat of the metal?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.101PAE

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Question

HELP ME PLEASE!!!! REFER TO IMAGE ATTACHED SHOW ALL WORK PLEASE

MUST SHOW ALL WORK AND UNITS
1. The temperature of a 98.7 g piece of metal increases from 17.0 °C
to 31.0 °C when the metal absorbs 705 J of heat. What is the specific
heat of the metal?
2. The initial temperature of the water in a constant-pressure
calorimeter is 25.0 °C. A reaction takes place in the calorimeter, and
the temperature rises to 79.0 °C. The calorimeter contains 858 g of
water, which has a specific heat of 4.18 J/g °C. Calculate the enthalpy
change during this reaction.
3. C3H3 (g) + O2 (g) --> CO2 (g) + H20 (1) + 2220 KJ/mol
Calculate the amount of heat required to burn 0.56 moles of C3H3.
(must balance the equation first)
4. Calculate the amount of heat absorbed to liquefy 42.8 g of
methanol (CH,0) at its melting point. The molar heat of fusion for
methanol is 3.16 KJ/mol.
5. How much heat (in KJ) is absorbed when 75.7 g of methanol
(CH,O) is converted to gas? Heat of vaporization for methanol is 35.2
KJ/mol.

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