Question

3. A sample of metal weighing 35.5g at a temperature of 100 oC was placed in a calorimeter containing 50 g of water at 25.0 oC. At equilibrium the temperature of water and metal was 35.5 oC. Calculate the heat capacity of the metal. . Use this value for Cp:27.65.

4. When 0.50 g of magnesium metal is placed in a calorimeter, and 100. mL of 1.0 M HCl were added the temperature of solution increased from 22.2 oC to 44.2 oC. Assume that the specific heat of solution is 4.18 J/goC and that the density is 1g/mL. Write a balanced equation for the above reaction. Calculate the enthalpy of reaction per mole of magnesium. . Use your value for Cp:27.65.

step by step please

Answer #1

3. Heat lost by the metal = Heat gained by the calorimeter

Heat lost by the metal = m*c*deltaT

m = mass of metal = 35.5g

c = specific heat capacity of metal

DeltaT = change in temperature = 100°C - 35.5°C = 64.5°C

So, heat lost by metal = 35.5*c*64.5 = 2289.75c

Heat gained by water = m*cp*deltaT

m = mass of water = 50g

cp = specific heat capacity of water = 27.65

DeltaT = 35.5°C - 25°C = 10.5°C

Heat gained by water = 50g*27.65*10.5 = 14516.25

Heat lost = heat gained

2289.75c = 14516.25

c = 14516.25 / 2289.75

= 6.34

Heat capacity of metal = 6.34J/g°C

A metal sample weighing 72.1 g is placed in a hot water bath at
95.0 oC. The calorimeter contains 42.3 g of deoinized water. The
initial temperature of the water is 22.3 oC. The metal is
transferred to the calorimeter and the final temperature reached by
the water + metal is 32.2 oC.
A. Calculate ∆T for the water (Tfinal – Tinitial).
B. Calculate ∆T for the metal.
C. The specific heat of water is 4.18 J/goC. Calculate the
specific...

A student dissolves 5g of NaOH in 100mL of water at 25.0
oC in a calorimeter. The final temperature of the
solution was found to be 35.4 oC. Assume the calorimeter
constant is 92J/oC , the density of the solution is
1g/ml, and the specific heat of the solution is 4.184J/g
oC. Calculate the enthalpy of solution of NaOH in kJ/mol
NaOH.

A student mixes 100mL of 0.5M NaOH and 100mL of 0.5M HCl at 25.0
oC in a calorimeter. The final temperature of the
solution was found to be 28.02 oC. Assume the
calorimeter constant is 92J/oC , the density of the
solution is 1g/ml, and the specific heat of the solution is
4.184J/g oC. Calculate the enthalpy of neutralization
NaOH(aq) in kJ/mol NaOH.

1.)
A volume of 36.7 mL of H2O is initially at 28.0 oC. A chilled
glass marble weighing 4.00 g with a heat capacity of 3.52 J/oC is
placed in the water. If the final temperature of the system is
26.4 oC , what was the initial temperature of the
marble? Water has a density of 1.00 g/mL and a specific heat of
4.18 J/goC.
Enter your answer numerically, to three significant
figures and in terms of oC.
2.)
A 2.24...

1. A 78.0 g piece of metal at 89.0°C is placed in 125 g of water
at 21.0°C contained in a calorimeter. The metal and water come to
the same temperature at 27.0°C.
- How much heat (in J) did the metal give up to the water?
(Assume the specific heat of water is 4.18 J/g·°C across the
temperature range.)
- What is the specific heat (in J/g·°C) of the metal?
2. A 0.529 g sample of KCl is added...

A student places a 72.0 gram sample of metal at an initial
temperature of 100.˚C in a coffee cup calorimeter that contains
40.0 grams of water at an initial temperature of 25.0 ˚C. After
addition of the metal, the temperature of the water / metal mixture
was monitored using a temperature probe. The highest temperature of
the water / solid combination was found to be 35.0 ˚C. (The
specific heat of water = 4.18 J / g ˚C )
Do...

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).

What final temperature would you expect from a chemical ice pack
with an initial temperature of 25.0 oC that mixes 30.00
g of KNO3 (∆H = 34.89 kJ/mol) with 200.0 g water? Assume
that the specific heat of the solution is 4.18
J/goC.

A.The heat change in a chemical reaction at constant
_____________ is quantitatively expressed as the change of the
enthalpy for the reaction.
temperature
volume
pressure
amount of mole
B.What will be final temperature if you mix the 50.g of water at
0.0oC to 50.g of water at 100.0oC.
75.0 degree Celsius
20.0 degree Celsius
90.0 degree Celsius
50.0 degree Celsius
C.Which will be the range of final temperature, Tfinal (oC) if
you mix the 50.g of Magnesium metal (S=1.020 J/goC)...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 1 minute ago

asked 16 minutes ago

asked 32 minutes ago

asked 38 minutes ago

asked 45 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago