Question #6ab87

1 Answer
zhirou
Feb 7, 2018

The correct choice is #"32.2°C"#.

Explanation:

For this question, we'll need to use the equation #q=mCDeltaT#, where #q# is heat gained or lost, #m# is mass, #C# is specific heat of the substance, and #DeltaT# is the change in temperature.

We have all of the variables except for #DeltaT#, which can be used to solve for final temperature. So, let's solve for #DeltaT# first by plugging the values in:

#q=mCDeltaT#
#"4110J" = "282g" * "4.184 J/g°C" * DeltaT#
#DeltaT = "4110J / 282g / 4.184 J/g°C"#
#DeltaT = "3.48 °C"#

#DeltaT# is #"final temperature - initial temperature"#, and we already know the initial temperature, so:

#DeltaT = "3.48 °C" = "final temperature - 28.7°C"#
#"3.48 °C = final temperature - 28.7°C"#
#"final temperature = 3.48 °C + 28.7°C"#
#"final temperature = 32.2°C"#

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