Asked by Andrew
How many milliliters of water at 25.0°C with a density of 0.997 g/mL must be mixed with 165 mL of coffee at 91.0°C so that the resulting combination will have a temperature of 62.1°C? Assume that coffee and water have the same density and the same specific heat (4.18 J/g·°C) across the temperature range.
Answers
Answered by
DrBob222
heat gained by cold water + heat lost by hot coffee = 0
[mass cold H2O x specific heat H2O x (Tfinal-Tinitial)] + [mass coffee x specific heat coffee x (Tfinal-Tinitial) = 0
Substitute and solve for mass cold H2O, then convert to mL.
mass = volume x density.
You know density and mass, solve for volume in mL.
[mass cold H2O x specific heat H2O x (Tfinal-Tinitial)] + [mass coffee x specific heat coffee x (Tfinal-Tinitial) = 0
Substitute and solve for mass cold H2O, then convert to mL.
mass = volume x density.
You know density and mass, solve for volume in mL.
Answered by
Anonymous
55.6
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.