A 62.6-gram piece of heated limestone is placed into 75.0 grams of water at 23.1°C. The limestone and the water come to a final temperature of 51.9°C. The specific heat capacity of water is 4.186 joules/gram degree Celsius, and the specific heat capacity of limestone is 0.921 joules/gram degree Celsius. What was the initial temperature of the limestone? Express your answer to three significant figures.

The initial temperature of the limestone was

208.7°C was the initial temperature of the limestone.

Explanation:

Heat lost by limestone will be equal to heat gained by the water

Mass of limestone =

Specific heat capacity of limestone =

Initial temperature of the limestone =

Final temperature = =T =  51.9°C

Mass of water=

Specific heat capacity of water=

Initial temperature of the water =

Final temperature of water = =T =  51.9°C

On substituting all values:

208.7°C was the initial temperature of the limestone.

i'm assuming that the correct answer is indeed the first one/ "a"..

substituting a hydrogen atom with a halogen in a hydrocarbon:

- the single bond remains single. a is wrong.

- the bond with hydrogen is as strong as with a halogen. c is wrong

- a hydrocarbon is saturated if there is no double bond. we do not know that so d is wrong.

- carbon will always have four valence electrons. e is wrong.

by elimination, the correct answer is b. the boiling point of the new compound increases.