Question

The specific heat capacity of S8 (s), at 25 C is 5.430 cal.K -1 . g -1 . A) what is the molar heat capacity of S8 in J.K-1.mol-1 at this temperature? hint: 1 cal = 4.184 J. B) 500.0 g sample of S8 at 25.0 C absorbs 50.00 kj of energy. what will be the final temperature of the sample in C? I dont need just the answer, I got this question wrong and I need to know how to do it.

Answer #1

specific heat capacity is given in grams which should be converted to 1 mole

Molar mass of S8 = 256.48 g/mol

molar heat capacity in calories = 5.43 x 256.48 = 1392.6864 Calories

let us convert calories to joules

1 calorie = 4.184 Joules

1392.6864 Calories = 5827 Joules

**molar heat capacity of S8 =
5827 J.K-1.mol-1**

**Q = mc∆T**

*Q* = heat energy (Joules, J),
*m* = mass of a substance (kg)

*c* = specific heat (units
J/kg∙K), *∆* is a symbol meaning "the change in"

*∆T* = change in temperature
(Kelvins, K)

5.43 calories = 22.71912 Jouels

50000 = 500 x 22.71912 x (Tf-25)

**Tf = 69.01 Deg
celcius**

**Hence the final temperature
is 69.01 Deg celcius**

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.

1- The molar mass and molar heat capacity of aluminum is 27.0
g/mol and 24.3 J/(mol K), respectively. If a 27.0-g Al sample, at
300. K, absorbed 168 J of heat, what is its final temperature?
2- The molar mass and molar heat capacity of aluminum is 27.0
g/mol and 24.3 J/(mol K), respectively. If a 27.0-g Al sample, at
300. K, absorbed 152 J of heat, what is its final temperature?
3- 100. g water, at 20 C, and...

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 500.0-g sample of an element at 153°C is dropped into an
ice-water mixture; 109.5-g of ice melts and an ice-water mixture
remains. Calculate the specific heat of the element from the
following data:
Specific heat capacity of ice: 2.03 J/g-°C
Specific heat capacity of water: 4.18 J/g-°C
H2O (s) → H2O (l), ΔHfusion: 6.02 kJ/mol (at 0°C)
a) If the molar heat capacity of the metal is 26.31 J/mol-°C,
what is the molar mass of the metal, and what...

1. A hot lump of 46.2 g of iron at an initial temperature of
77.9 °C is placed in 50.0 mL of H2O initially at 25.0 °C and
allowed to reach thermal equilibrium. What is the final temperature
of the iron and water given that the specific heat of iron is 0.449
J/(g·°C)? Assume no heat is lost to surroundings. 2.When 1422 J of
heat energy is added to 40.8 g of hexane, C6H14, the temperature
increases by 15.4 °C....

How much energy (in kJ) is required to raise the temperature of
25.0 g of H2O from –25°C to 25°C ? (ΔH°fus of H2O = 6.02 kJ/mol ;
molar heat capacity of solid H2O = 37.6 J/mol•°C ; molar heat
capacity of liquid H2O = 75.4 J/mol•°C)
(a) 70.7 kJ
(b) 8.73 kJ
(c) 61.9 kJ
(d) 12.3 kJ

In a constant-pressure calorimeter of negligible heat capacity,
25 mL of 1.00 M CaCl2 is mixed with 25 mL of 2.00 M KF, resulting
in solid CaF2 precipitating out of the solution. During this
process, the temperature of the water rises from 25.0°C to 26.7°C.
Assume the specific heat capacity of the solution is 4.184 J/°C•g
and the density of the solution is 1.00 g/mL. Calculate the
enthalpy of precipitation in kJ per mole of CaF2 precipitated.

(a) The molar heat capacity of lead is 26.44 J K-1 mol-1. How
much energy must be supplied (by heating) to 100 g of lead to
increase it’s temperature by 10.0°C? (b) The molar heat capacity of
sodium is 28.24 J K-1 mol-1. What is its specific heat capacity?
(c) The specific heat capacity of copper is 0.384 J K-1 g-1. What
is its molar heat capacity?

How much heat is released when 105 g of steam at 100.0°C is
cooled to ice at -15.0°C? The enthalpy of vaporization of water is
40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the
molar heat capacity of liquid water is 75.4 J/(mol • °C), and the
molar heat capacity of ice is 36.4 J/(mol • °C).

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 1 minute ago

asked 15 minutes ago

asked 16 minutes ago

asked 23 minutes ago

asked 39 minutes ago

asked 39 minutes ago

asked 39 minutes ago

asked 41 minutes ago

asked 47 minutes ago

asked 49 minutes ago

asked 53 minutes ago

asked 1 hour ago