What does it mean when there is a physical change?
1 answer:
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Taking into account the definition of calorimetry, the specific heat of metal is 0.165 .
Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.
Sensible heat is defined as the amount of heat that a body absorbs or releases without any changes in its physical state (phase change).
So, the equation that allows to calculate heat exchanges is:
Q = c× m× ΔT
where:
- Q is the heat exchanged by a body of mass m.
- C is the specific heat substance.
- ΔT is the temperature variation.
In this case, you know:
For metal:
- Mass of metal = 50 g
- Initial temperature of metal= 45 °C
- Final temperature of metal= 11.08 ºC
- Specific heat of metal= ?
For water:
- Mass of water = 250 g
- Initial temperature of water= 10 ºC
- Final temperature of water= 11.08 ºC
- Specific heat of water = 1.035
Replacing in the expression to calculate heat exchanges:
For metal: Qmetal= Specific heat of metal× 50 g× (11.08 C - 45 C)
For water: Qwater= 1.035 × 250 g× (11.08 C - 10 C)
If two isolated bodies or systems exchange energy in the form of heat, the quantity received by one of them is equal to the quantity transferred by the other body. That is, the total energy exchanged remains constant, it is conserved.
Then, the heat that the gold gives up will be equal to the heat that the water receives. Therefore:
- Qmetal = + Qwater
- Specific heat of metal× 50 g× (11.08 C - 45 C)= 1.035 × 250 g× (11.08 C - 10 C)
Solving:
- Specific heat of metal× 50 g× (-33.92 C)= 1.035 × 250 g× 1.08 C
Specific heat of metal× 1696 g×C= 279.45 cal
Specific heat of metal=
<u><em>Specific heat of metal= 0.165 </em></u>
Finally, the specific heat of metal is 0.165 .
Learn more about calorimetry:
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<u>Answer:</u> The given amount of iron reacts with 9.0 moles of and produce 6.0 moles of
<u>Explanation:</u>
We are given:
Moles of iron = 12.0 moles
The chemical equation for the rusting of iron follows:
- <u>For oxygen gas:</u>
By Stoichiometry of the reaction:
4 moles of iron reacts with 3 moles of oxygen gas
So, 12.0 moles of iron will react with = of oxygen gas
- <u>For iron (III) oxide:</u>
By Stoichiometry of the reaction:
4 moles of iron produces 2 moles of iron (III) oxide
So, 12.0 moles of iron will produce = of iron (III) oxide
Hence, the given amount of iron reacts with 9.0 moles of and produce 6.0 moles of