A 10.0 g cube of each of the following metals is heated to 100 °C

Question

A 10.0 g cube of each of the following metals is heated to 100 °C

and dropped (without loss of heat during transfer) into separate but identical beakers containing 100 mL of water at 25 °C. The temperature of the water in the beaker is measured at equilibrium. Which metal will cause the temperature of the water in the beaker to change the most?
Specific Heat (J/g!K)
A. Al(s) 0.903
B. Cu(s) 0.385
C. Au(s) 0.128
D. Fe(s) 0.449
E. They would all change the temperature by the same amount.

Answer 1

i just searched for this question too hahah chem 110 psu

Answer 2

Which holds the most heat?

q = mass metal x specific heat x delta T.
q = 10g x sp.h. x (100-25).

To make q large, specific heat must bae (large/small)?

Answer 3

To determine which metal will cause the temperature of the water in the beaker to change the most, we can use the formula:

Q = mcΔT

Where:
Q is the heat absorbed or released in Joules (J)
m is the mass of the substance in grams (g)
c is the specific heat capacity of the substance in J/g°C
ΔT is the change in temperature in degrees Celsius (°C)

In this case, the substances are the metals, and the water is the substance gaining or losing heat.

Since the mass of the metal cubes is given as 10.0 g, and the water volume is given as 100 mL, we need to convert the volume of water to grams. The density of water is 1 g/mL, so the mass of 100 mL of water is 100 g.

Now let's calculate the heat absorbed by each metal by using the formula and plugging in the given values:

For Al:
Q_al = (10.0 g)(0.903 J/g°C)(T_final - T_initial)

For Cu:
Q_cu = (10.0 g)(0.385 J/g°C)(T_final - T_initial)

For Au:
Q_au = (10.0 g)(0.128 J/g°C)(T_final - T_initial)

For Fe:
Q_fe = (10.0 g)(0.449 J/g°C)(T_final - T_initial)

Since the mass and specific heat capacity are the same for all metals, the change in temperature, ΔT, will determine which metal causes the greatest change in the water temperature.

So, to compare the values of Q for each metal and determine which one will cause the greatest temperature change in the water, we need to know the value of ΔT for each case.

However, the question only provides the initial temperatures of the metals and water, but it does not provide the final temperature at equilibrium.

Therefore, without the value of the final temperature, we cannot calculate the ΔT or the heat absorbed, Q, for each metal. As a result, we cannot determine which metal will cause the temperature of the water in the beaker to change the most.

So the correct answer is: Insufficient data is provided to determine which metal will cause the temperature of the water in the beaker to change the most.