Question

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 that its specific heat capacity is 4.21 J/g°C.

Question 3 : The tallest building on Earth in 2016 is the Burj Khalifa in Dubai, which stands at 2717 ft tall. A 15.0 kg iron sphere is dropped from the very top of the Burj Khalifa building. What is the theoretical maximum temperature increase possible in degrees Celsius for the iron sphere if measured a minute distance above the ground before impact?

Question 4 : You suspect that your water supply is contaminated with bacteria so decide to boil 15.0 gallons of water. A sudden power outage in your home forces you to use camping gas (propane) as a fuel to boil the water. What volume of fuel (litres) will you need to boil the water if its initial temperature is 22.5°C? (the density of liquid propane is 0.493 g/cm

^33. Only 17% of the heat of combustion of propane goes towards heating the water).

Question 5 : The Dulong-Petit law states that the specific heat capacity (c) of any element is equal to 3R/M, where R is a constant equal to 8.314 J/mol K, and M is the molar mass of the element measure in units of g/mol. Use specific heat capacity data from table 5.2 to plot the Dulong-Petit law as a straight line graph. Use the equation from your straight line graph to identify the element whose specific heat is 0.137 J/g°C.

I really need help!!!

Answer #1

**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?**

We require 2 type of heat, latent heat and sensible heat

Sensible heat (CP): heat change due to Temperature difference

Latent heat (LH): Heat involved in changing phases (no change of T)

Then

Q1 = m*Cp ice * (Tf – T1)

Q2 = m*LH ice

Q3 = m*Cp wáter * (Tfinal– Tfusion)

**Note** that Tf = 0°C;
Tb = 100°C, LH ice = 334 kJ/kg;

Cp ice = 2.01 J/g°C ; Cp water = 4.184 J/g°C

Then

Q1 = **555***2.01 * (0 – **-120**)

Q2 = 555*****334

Q3 = **555***4.184 * * (Tfinal– 0)

0.5159*10^6 = 555*(2.01*(120) + (334) + 4.184*Tf)

(0.5159*10^6) - 555*(2.01*(120) + (334)) = 555*4.184*Tf

196664 = 555*4.184*Tf

Tf = 196664 /(555*4.184) = 84.69°C

Tfinal of block --> melted = 84.69°C

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?

Suppose that 0.1 kg of ice at an initial temperature of -10°C are
put into 0.40 kg of water at an initial temperature of 20°C. Assume
the final temperature is 0°C. How many grams of ice will melt?
Specific heat capacity of water is 4,200 J/kg/°C. Specific heat of
fusion of water is 336,000 J/kg and specific heat capacity of ice
is 2,100 J/kg/°C.

1. A 36.6-kg block of ice at 0 °C is sliding on a horizontal
surface. The initial speed of the ice is 9.02 m/s and the final
speed is 3.89 m/s. Assume that the part of the block that melts has
a very small mass and that all the heat generated by kinetic
friction goes into the block of ice, and determine the mass of ice
that melts into water at 0 °C.
2. A rock of mass 0.396 kg...

A 24 g block of ice is cooled to −63◦C. It is added
to 572 g of water in a 98 g copper calorimeter at a temperature of
30◦C.
Find the final temperature. The specific heat of copper is 387
J/kg ·◦C and of ice is 2090 J/kg ·◦C. The
latent heat of fusion of water is 3.33 × 105 J/kg and its specific
heat is 4186 J/kg·◦C.
Answer in units of ◦C.

A 31 g block of ice is cooled to −90◦C. It is added to 591 g of
water in an 65 g copper calorimeter at a temperature of 26◦C. Find
the final temperature. The specific heat of copper is 387 J/kg · ◦C
and of ice is 2090 J/kg · ◦C . The latent heat of fusion of water
is 3.33 × 105 J/kg and its specific heat is 4186 J/kg · ◦C . Answer
in units of ◦C.

A 78 kg block of Iron (Specific Heat Capacity 348 J/kg.K) at
temperature T kelvin is inserted into 5 kg of water (Specific Heat
Capacity 4005 J/kg.K and initial temperature is 300 K). Final
temperature of the mixture is 308 K. Assuming no heat loss to
surrounding calculate the initial temperature of the iron block:
_______ K

A 2.5 kg metallic block with an initial temperature of 80°C is
placed in a styrofoam cup containing 0.1 kg of ice at -15°C.
Assuming that no heat escapes from the cup what is the final
temperature of the metallic block? The specific heat of the metal
is 480 J/kg ∙ K, specific heat of ice is 2090 J/kg ∙ K, the latent
heat of fusion of water is 3.33 × 105 J/kg, and the specific heat
of water is...

A 1.000 kg block of ice at 0 °C is dropped into 1.354 kg of
water that is 45 °C. What mass of ice melts?
Specific heat of ice = 2.092 J/(g*K) Water = 4.184
J/(g*K) Steam = 1.841 J/(g*K) Enthalpy of fusion =
6.008 kJ/mol Enthalpy of vaporization = 40.67 kJ/mol

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...

A 40 g block of ice is cooled to -78°C. and is then added to 610
g of water in an 80 g copper calorimeter at a temperature of 26°C.
Determine the final temperature of the system consisting of the
ice, water, and calorimeter. Remember that the ice must first warm
to 0°C, melt, and then continue warming as water. The specific heat
of ice is 0.500 cal/g ·°C = 2090 J/kg°C

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 28 minutes ago

asked 37 minutes ago

asked 1 hour 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

asked 2 hours ago

asked 2 hours ago