Question

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

Givens:
Mass of metal (AI) = 27.776g
Distilled water measurement = 26mL
Distilled water temperature = 25.4 C
Temperature of metal = 100.8 C
Temperature of mixture (after metal is placed in calorimeter with distilled water) = 28.9 C

Please and thank you!!

Answer 1

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.

Answer 2

@BloomLocke367

Answer 3

@Daniellelovee

Answer 4

My answer for question 1 is: Qwater = 27.776 * 4.18 J / (g * °C) * (25.4 * 38.9) = 6562.388 calories or 27475.410 Joules

and for question 2 it's: Qmetal = 27.776 * c * (100.8 * 38.9) = -3.816 cal / g * C or -15.980 j / g * C

Answer 5

hmm, I'm not to good at chemistry. But @JFraser might be able to help.

Answer 6

Ok, thanks :)

Answer 7

or @thomaster or @nincompoop.. try sending them a message and asking for help.

Answer 8

Will do :P

Answer 9

Can someone please check my work? @nincompoop @thomaster @Callisto @rvc

Answer 10

gimme a sec I'll help you this was my favorite

Answer 11

Yep you got it right :)

Answer 12

Good job
both of you :)
All The Best

Answer 13

\(\Delta T\) is the \(change\) in temperature, not the \(product\) of the two temperatures.

You need to find the difference in temperature from the metal before and after, and the water before and after