Question

help check my answers for my chem lab?

Answer 1

this is my lab assignment:

Part I:

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

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.
Part II:

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

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.

Answer 2

Part 1 is for Al, here is the data for Al

Answer 3

1. qwater = m × c × ΔT.

Plug in the numbers for the equation, q=(1)(26)(4.18)(41.6-25). After multiplying, you end up with q water = 1804.088 Joules.

2. Since q water = -q unknown metal, I found the specific heat of the metal by doing q/mT. Once I plugged the values in, I got 1804.088/(37.720)(41.6-100.5). After simplifying, I got 0.8120275. This is the specific heat of Al.

This is my answer for Part 1, can someone check it?

Answer 4

looks fine to me!!! keep going
(you haven't posted the problem but all the logic looks OK)

Answer 5

i have a part 2 where i have to do the same thing i just did but for an unknown metal, can you help with that?