Question

I NEED SERIOUS HELP, I HAVE PART OF THE ANSWERS THOUGH!!!

Answer 1

Part II:
1. Calculate the energy change (q) of the surroundings (water) using the enthalpy equation

qwater = m × c × ΔT.

We can assume that the specific heat capacity of water is 4.18 J / (g × °C) and the density of water is 1.00 g/mL. Show ALL your work.

The water has absorbed the heat of the metal. So, qwater = qunknown metal
So we use the same process as we did for part I.
So
1) Qwater= 15.262 times 4.18 J / (g × °C) times (27.5oC – 25.2 oC)
2) We then multiply our mass of 15.262 times 4.18
3) To get qwater 63.79516j\ (g × °C) times (2.3oC)
4) WE THEN MULTIPLY THOSE TWO NUMBERS TO GET
5) 63.79516 TIMES 2.3 TO GET OUT
6) QWATER= 146.728868J\ (g × °C) 

2. Using the formula qunknown metal = m × c × ΔT, calculate the specific heat of the metal. Use the data from your experiment for the unknown metal in your calculation. Show ALL your work.
The mass is still 15.262 and the triangle T is 146.728868 because it is the answer to the first part of the question we have then and q water equals q unknownmetal q=q so the answer now would be c= 146.728868\ 15.262 times 2.3 which is 22.1122 


Conclusion:
1. 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
I got stuck here


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 Specific Heat Capacity
Nickel 0.440
Tin 0.210
Silver 0.237
Magnesium 0.140
Calcium 0.650
Mercury 0.140
o Metal you examined:
o Experimental specific heat capacity:
o Metal identity:
o Known specific heat capacity value:
o Percent error (Show ALL work):

4. In complete sentences, describe three sources of experimental error that could occur with this type of calorimetry lab. Explain, in detail, the effect that each specific error would have on the calculated specific heat capacity values.
9 months ago

Answer 2

Wow, I understand why you need help now! lol :D

Answer 3

Is the mass of 15.262 the mass of the water or the metal, and is it in grams?

Answer 4

q of the water = mass of the water * specific heat of water * change in temp of the water

Answer 5

For a calorimeter, you assume that all of the heat gained by the water was lost by the metal, so
-q of the water = mass of the metal * specific heat of the metal * change in the temperature of the metal

Answer 6

My best guess from what you have here is that you used the mass of the metal for the mass of the water. Do you know the actual mass of the water? The mass of the water should be more than the mass of the metal.

Answer 7

ThaNK YOU

Answer 8

You're welcome. :)