Question

The following table lists the specific heat capacities of select substances: Substance Specific heat capacity [J/(g⋅∘C)] silver 0.235, copper 0.385, iron 0.449, aluminum 0.903, ethanol 2.42, water 4.184, Water (2430 g ), is heated until it just begins to boil.

If the water absorbs 5.07×105 J of heat in the process, what was the initial temperature of the water? Express your answer with the appropriate units.

Answer #1

water is heated until to boil

So final temperature of water = Tf = 100 ^{0}C

Mass of sample = m = 2430 g

amount of heat gain = q = 5.07 x 10^{5} J

And Specific heat of water = c = 4.184 g/^{0}C

Now

We know the formula

q = m.c.T

So T = q / (m.c)

putting given values

T
= 5.07 x 10^{5} J /(2430 g x 4.184
J/^{0}C)

= 49.86 ^{0}C

Then

T = Tf - Ti = change in temperature

49.86 ^{0}C = 100 ^{0}C - Ti

Ti = 100 ^{0}C - 49.86 ^{0}C

= **50.14 ^{0}C**

So intial temperature of water = **50.14
^{0}C**

A 25 g gold nugget with an initial temperature of 60 °C is
dropped into an insulated cup containing 100 ml of water initially
at a temperature of 5°C. What is the final temperature after
thermal equilibrium is established?
Table 3.4 Specific Heat Capacities of Some Common Substances
Substance Specific Heat Capacity (J/g °C) Lead 0.128 Gold 0.128
Silver 0.235 Copper 0.385 Iron 0.449 Aluminum 0.903 Ethanol 2.42
Water 4.184

Which of the following will have the largest temperature
increase in response to 250 J of heat? ethanol, 2.42 J/g°C
aluminum, 0.903 J/g°C copper, 0.385 J/g°C gold, 0.128 J/g°C

You have three metal pans (Cu, Fe, Al) that you want to pre-heat
on the stovetop to cook. If the metal pans were all the same mass,
which would you heat up the quickest? Explain your reasoning.
Metal
Specific Heat Capacity (J/ g * C)
Copper
0.385
Iron
0.449
Aluminum
0.903

Copper has a specific heat capacity of 0.385 J/goC.
If 12.8 g of copper initially has a temperature of 35.0
oC and it absorbs 367 J of heat, what will be its new
temperature? please give me the process not just the answer

A 35.7 gram sample of iron (heat capacity 0.45 g/J°C) was heated
to 99.10 °C and placed into a coffee cup calorimeter containing
42.92 grams of water initially at 15.15 °C. What will the final
temperature of the system be? (Specific heat of water is 4.184
J/g°C).
Please show work.

1. Calculate specific heat for Aluminum in J/(g °C) showing all
work: (use 4.184 J/(g °C) for water)
solve -----> q= 100g x 4.184 J/(g °C) x (41°C - 100 °C)

19. How much heat is liberated (in kJ) from 2.47E+2 g of silver
when it cools from 8.86E+1 °C to 2.57E+1 °C? The heat capacity of
silver is 0.235 J g^{-1} °C^{-1} g−1°C−1. Note,
"heat liberated" implies that the change in heat is negative. Enter
a positive number
20. A sample of sand initially at 2.18E+1 °C absorbs 1.386E+3 J
of heat. The final temperature of the sand is 6.7E+1 °C. What is
the mass (in g) of sand in...

11.
Consider the following specific heat capacities:
H2O (s) = 2.09 J/g·°C
H2O (l) = 4.18 J/g·°C
H2O (g) = 2.03 J/g·°C
The heat of fusion for water is 334 J/g and its heat of
vaporization is 2260 J/g. Calculate the amount of heat required to
convert 93 g of ice at -36°C completely to liquid water at
35°C.
52 kJ
21 kJ
7 kJ
38 kJ

A substance has the following properties:
Heat capacities:
1.34 J/g oC (solid)
3.02 J/g oC (liquid)
2.55 J/g oC (gas)
Heat of Fusion = 4.23 kJ/mole
Heat of Vaporization = 23.5 kJ/mole
Melting Point = -30.0 oC
Boiling Point = 88.5 oC
Molar Mass = 69.3 g/mole
How much energy (in kJ) would be needed to heat
555 g of this substance from 1 to 201oC?

A 6.40 g sample of iron (specific heat capacity = 0.451 J/g*C)
is placed in a boiling water bath until the temperature of the
metal is 100.0*C. The metal is quickly transferred to 119.0g of
water at 25.0*C in a calorimeter (specific heat capacity of water =
4.18 J/g*C). Determine the final temperature of the water in the
calorimeter (3 significant figures).

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