Question #95ca2

1 Answer
Sep 24, 2017

Answer:

#"9,900 J"#

Explanation:

Your goal here is to figure out how much heat is needed to increase the temperature of #"55 g"# of water by

#87^@"C" - 44^@"C" = 43^@"C"#

The key here is the specific heat of water, which tells you the amount of heat needed to increase the temperature of #"1 g"# of water by #1^@"C"#.

Use the specific heat of water to determine the energy needed to increase the temperature of #"55 g"# of water

#55 color(red)(cancel(color(black)("g"))) * overbrace("4.184 J"/(1color(red)(cancel(color(black)("g"))) * 1^@"C"))^(color(blue)("the specific heat of water")) = "230.12 J"""^@"C"^(-1)#

This tells you that in order to increase the temperature of #"55 g"# of water by #1^@"C"#, you need to provide #"230.12 J"#.

Consequently, you can say that in order to increase the temperature of the sample by #43^@"C"#, you need

#43 color(red)(cancel(color(black)(""^@"C"))) * overbrace("230.12 J"/(1color(red)(cancel(color(black)(""^@"C")))))^(color(blue)("for 55 g of water")) = color(darkgreen)(ul(color(black)("9,900 J")))#

of heat. The answer is rounded to two sig figs.