Question

**A 4.0 kg metal alloy block made of equal amount of iron
and aluminum is placed in 1.0 L of boiling water until its
temperature stabilizes at 100.0°C. 1500.0 mL of water with an
initial temperature of 5.0 °C is added to the mixture. What is the
new equilibrium temperature reached? (55°C) Which element in the
mixture will loose the least amount of energy during cooling
process?**

Answer #1

A 1.0 × 10^2 g Aluminum block. at 100 ° C it is placed in a calorimeter containing 1.0 × 10^2 g of water at 10ºC
Suppose there is no heat loss. What is the final temperature of the mixture?

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).

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).

A 125-g block of aluminum at room temperature (21°C) is placed
into 150 g of boiling water (100°C). If the aluminum block and
water form a closed system, what will their temperature be when
they achieve thermal equilibrium?

1. A 50-g sample of iron at 100oC is put into 75 g of
water at 0oC. What is the final temperature of the
mixture? (The specific heat of iron is 0.11 cal/g
Co.)
2. A machine part consists of 0.10 kg of iron and 0.16 kg of
copper. How much heat is added to the gear if the temperature
increases by 35oC? [Hint: Compute the heat required for
each metal and add the numbers. State your answer in joules.]...

A 10.5 g block of iron metal (Cs= 0.449 J/g⁰C) at 55°C is
submerged in 7.50 mL water (Cs = 4.184 J/g⁰C) initially at 25°C
(density of water is 1.00 g/mL). What is the final temperature of
the iron and water?
-[(10.5 g)(0.449 J/(g℃))(Tf - 55℃)] = (7.50 g)(4.184J/(g℃))(Tf -
25℃)
Tf = 29 ℃
I understand how to set the problem up but do not understand how
to isolate Tf by itself? Can someone show me the steps that...

Q 4. A metal block of heat capacity 600 J K-1
loses 1 M.J of heat energy to its surroundings. Find the decrease
in temperature.
Q5. One mega joule of heat energy is supplied to a piece
of iron and raises its temperature from
20?C to
200?C. Find the mass of the piece
of iron.( Specific heat capacity of iron
=451Jkg-1K-1
Q6. 30grams of water at
100?C are added to 100 grams of
water at 20?C. If there is no...

A 2.50-kg block of hot iron (cFe = 0.45 J/g K; Tin = 300. oC) is
dropped in cold water (Tin = 20 oC) to cool quickly.
1) how much heat needs to be absorbed to cool
the iron block to 25 oC?
A) 309 J B) 309 kJ C) 618 J D) 618 kJ E) None of the above
2) How much cold water will be needed?
A) 14.8 g B) 14.8 kg C) 14.8 m3 D) 14,800 L...

Question 1 : The temperature of a 0.555 kg block of ice is
lowered to -120°C. Heat (0.5159 MJ) is then transferred to the
block of ice (assume ice is otherwise thermally isolated). What is
the final temperature of the water in °C?
Question 2 : Calculate the time needed (seconds) to that up 285
mL of tomato soup from 4.0°C to 57°C in a 1100. watt microwave
oven. Assume that the density of tomato soup is 1.25 g/mL and...

1. What is the purpose of crystallization in an organic
chemistry procedure?
2. Using the solubility data you found for benzoic acid,
calculate the volume of water required to dissolve 1.0 g of benzoic
acid at room temperature. Calculate the volume of boiling water
needed to dissolve 1.0 g of benzoic acid.
3. Explain why a Büchner or Hirsh funnel is used to isolate the
final crystallized product instead of stem funnel.
4. Explain when a mixture of solvents would...

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