Question

1a) A 25.5-g piece of lead initially at 98.6 °C is submerged into 122.3 g of water at 20.9 °C. What is the final temperature of the metal once the metal and water reaches thermal equilibrium? The specific heats of lead and water are 0.128 J/g·°C and 4.18 J/g·°C, respectively.

Answer #1

1a) A gaseous system absorbs 97 J of heat and increases its
internal energy by 85 J. Which of the following statements is
correct? The volume of the system decreases and a positive amount
of work is done. The volume of the system increases and a positive
amount of work is done. The volume of the system increases and a
negative amount of work is done. The volume of the system remains
constant and no work is done The volume...

A 60.0 g aluminum block, initially at 55.00 °C, is submerged
into an unknown mass of water at 293.15 K in an insulated
container. The final temperature of the mixture upon reaching
thermal equilibrium is 25.00 °C. What is the approximate
mass of the water? The specific
heat of water is 4.18 J/g . °C. The
specific heat of aluminum is 0.897 J/g
. °C.

A 2.29 g lead weight, initially at 10.6 ∘C, is submerged in 8.24
g of water at 52.6 ∘C in an insulated container. What is the final
temperature of both the weight and the water at thermal
equilibrium?

A 2.60 g lead weight, initially at 10.7 ∘C, is submerged in 8.18
g of water at 52.0 ∘C in an insulated container What is the final
temperature of both the weight and the water at thermal
equilibrium?

A 2.76 g lead weight, initially at 10.7 ∘C, is submerged in 8.17
g of water at 52.6 ∘C in an insulated container.
What is the final temperature of both the weight and the water
at thermal equilibrium?
Express the temperature in Celsius to three significant
figures.

A 2.53 g lead weight, initially at 10.1∘C, is submerged in 8.17
g of water at 52.4 ∘C in an insulated container. (this is all that
was given). What is the final temperature of both substances at
thermal equilibrium?

A 2.28 g lead weight, initially at 11.1 ∘C, is submerged in 8.15
gof water at 52.8 ∘C in an insulated container. What is the final
temperature (degrees Celsius) of both the weight and the water at
thermal equilibrium?

(A) A 36.0 g piece of lead at 130.0 C is placed in 100.0 g of
water at 20.0 C. What is the temperature (in C) of the water once
the system reaches equilibrium? The molar heat capacity of lead is
26.7 J/(mol·K). The specific heat capacity of water is 4.18
J/(g·K).
(B) How much energy (in kJ) will it take to heat up 1150 ml of
water in a coffee pot from 24 C to 95 C given that...

A 2.52g lead weight, initially at 10.1?C, is submerged in 7.94g
of water at 52.3?C in an insulated container.
What is the final temperature of both substances at thermal
equilibrium?

An 100-g aluminum calorimeter contains 280 g of water at an
equilibrium temperature of 20°C. A 170-g piece of metal, initially
at 277°C, is added to the calorimeter. The final temperature at
equilibrium is 32°C. Assume there is no external heat exchange. The
specific heats of aluminum and water are 910 J/kg·K and 4190
J/kg·K, respectively. The specific heat of the metal is closest
to:
a) 270 J/kg·K.
b) 240 J/kg·K.
c) 330 J/kg·K.
d) 390 J/kg·K.
e) 360 J/kg·K.

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