Question

Calorimetry help for chemistry?
cant figure these questions out:

heres my data:
Part II:
Measured mass of metal 25.605g
Distilled water measurement 24mL
Distilled water temp. 25 °C
Temp. of metal 100.5 °C
Temp. of mixture 29.1 °C

calculations for part 2: the metal lost is 411 J. Then you divide this by its mass and its temperature change to get the specific heat capacity: (411 J) / ((25.605 g)(71.4 °C)) = 0.225 J / (g × °C).

questions:
2)Using the specific heat capacity value that you determined in Part II of the lab, what is the most probable identity of the unknown metal that you examined? Please explain your reasoning in complete sentences.

3)Based on your answer in question 2, determine the percent error of your calculated specific heat capacity value of your unknown metal using the specific heat capacities of known metals below.

Metal - Heat Capacity
Nickel - 0.440
Tin - 0.210
Silver - 0.237
Magnesium - 0.140
Calcium - 0.650
Mercury - 0.140

Answer 1

What is it that you need help with? The calculations?

Answer 2

Looks like it'll be a

-q = q calculation.

Answer 3

the questions I was able to get the calculations but not the questions I think they wanted me to use percent error bacause it also said this:
Use the given specific heat capacity values below to calculate the percent error of the experimental specific heat capacity that you determined in Part I of the lab.

Known specific heat values — Iron: 0.444 J/g°C; Zinc: 0.390 J/g°C; Copper: 0.385 J/g°C, Aluminum: 0.900 J/g°C
| experimental - actual value | x 100 % actual value

Answer 4

What was the "c" you calculated?

Answer 5

That'd be your experimental value.

Answer 6

I don't remember I just got the measurements and the specific heat capacity

Answer 7

Well you're asked to calculate the specific heat capacity and compare it to the values given to you there--whichever is the closest to your value is the theoretical value.

Answer 8

oh ok I get it thank you:)

Answer 9

You're welcome :))