Can some on please check me work for me? :( I feel like i'm doing it wrong.

Data and Observations:
Part I:
Insert a complete data table, including appropriate significant figures and units, in the space below. Also include any observations you made over the course of Part I.
Metal: Iron
Mass of metal: 34.720 g
Volume of water in the calorimeter: 26.0 mL
Initial temperature of water in calorimeter: 25.3 °C
Temperature of hot water and metal in hot water bath: 100.5 °C
Final temperature reached in the calorimeter: 33.1 °C

Part II:
Insert a complete data table, including appropriate significant figures and units, in the space below. Also include any observations you made over the course of Part II.
Metal: Metal A
Mass of metal: 15.262 g
Volume of water in the calorimeter: 24.0 mL
Initial temperature of water in calorimeter: 25.2 °C
Temperature of hot water and metal in hot water bath: 100.3 °C
Final temperature reached in the calorimeter: 27.5 °C

Calculations:
Show your work and write a short explanation with each calculation.
Part I:
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.

The water has absorbed the heat of the metal. So, qwater = qmetal\
1) Qwater= 34.720 times 4.18j\(oCtimes g) times (330C-25.4OC)
2) Then I multiply 34.720 by 4.18 then I subtract 25.4 by 33
3) So now I have qwater equals 145.1296j \(Co times g) times (7.6oC)
4) THEN I MULTIPLY 145.1296 TIMES 7.6
5) NOW MY QWATER EQULAS 1102.9849 \ CO TIMES G :)

2. Using the formula qmetal = m × c × ΔT, calculate the specific heat of the metal. Use the data from your experiment for the metal in your calculation.
The mass is still 34.720 and the triangle T is 1102.9848 because it is the answer to the first part of the question we have then and q water equals q metal q=q so the answer now would be c= 1102.98496\ 34.720 times 7.6 which is 241.4368 

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.

Question

Can some on please check me work for me? :( I feel like i'm doing it wrong.

Data and Observations: 
Part I:
Insert a complete data table, including appropriate significant figures and units, in the space below. Also include any observations you made over the course of Part I. 
Metal:	Iron
Mass of metal:	34.720 g
Volume of water in the calorimeter:	26.0 mL
Initial temperature of water in calorimeter:	25.3 °C
Temperature of hot water and metal in hot water bath:	100.5 °C
Final temperature reached in the calorimeter:	33.1 °C

Part II:
Insert a complete data table, including appropriate significant figures and units, in the space below. Also include any observations you made over the course of Part II. 
Metal:	Metal A
Mass of metal:	15.262 g
Volume of water in the calorimeter:	24.0 mL
Initial temperature of water in calorimeter:	25.2 °C
Temperature of hot water and metal in hot water bath:	100.3 °C
Final temperature reached in the calorimeter:	27.5 °C

Calculations:
Show your work and write a short explanation with each calculation.
Part I:
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.

The water has absorbed the heat of the metal. So, qwater = qmetal\
1)	 Qwater= 34.720 times 4.18j\(oCtimes g) times (330C-25.4OC) 
2)	Then I multiply 34.720 by 4.18 then I subtract 25.4 by 33
3)	So now I have qwater equals 145.1296j \(Co  times g) times (7.6oC) 
4)	THEN I MULTIPLY 145.1296 TIMES 7.6
5)	NOW MY QWATER EQULAS 1102.9849 \ CO TIMES G :)

2.	Using the formula qmetal = m × c × ΔT, calculate the specific heat of the metal. Use the data from your experiment for the metal in your calculation.
The mass is still 34.720 and the triangle T is 1102.9848 because it is the answer to the first part of the question we have then and q water equals q metal q=q so the answer now would be c= 1102.98496\ 34.720 times 7.6 which is 241.4368 

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.

anonymous · Answer

my friend...look up "how to ask questions" on the web. i want to help, but could you single out a thing or two instead of asking people to look at the entire thing?