Question

If 133.2 kJ of heat are added to 5.80 × 10^{2} g of
water at 22.0°C, what is the final temperature of the water?
Specific heat of water at 1.00 atm and 20.0°C is 4.186 kJ/kg·K.

Answer #1

**Specific of water is given as 4.186 kJ/Kg.K which means
it will take 1kJ of energy to heat up 1Kg of water to raise its
temperature by 1 degrees (Kelvin or celcius).**

**In this type of questions we use the formula to
calculate the energy which is:**

**Now we are given E=133.2 KJ so,**

**So change(rise) in temperature is 54.9 ^{o}C.
Hence the final temperature T_{f} is:**

**So final temperature is about 77 ^{o} C or more
precisely 76.9^{o}C.**

1. If 121.4 kJ of heat are added to 6.10 × 102 g of
water at 22.0°C, what is the final temperature of the water?
Specific heat of water at 1.00 atm and 20.0°C is 4.186 kJ/kg·K.
(Refer to Table 14.1.)
2. It takes 880 J to raise the temperature of 350 g of lead from
0°C to 20.0°C. What is the specific heat of lead?
3. A 4.00-kg steel ball at 27.3°C is dropped from a height of
10.8...

Question1:
If 2.72 kJ of heat are supplied to 2.4 × 102 g of
water at 25 °C, what is the final temperature of the water?
Question 2:
Compute the heat of fusion from these data. 21.08 kJ will
change 0.33 kg of the solid at 18.5 oC to 327
o C., the melting point. Specific heat capacity of solid
:0.129 KJ/KgK.
Give your answer as a positive number.
please solve both, I need them!!!!

803 cal of heat is added to 5.00 g ice at –20.0 °C.
What is the final temperature of the water?
SPecific heat H2O(s)= 2.087 J/(g*C)
Specific heat H2O(l)=4.184 J/(g*C)
Heat of fusion= 333.6 J/g

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.

1) A certain substance has a heat of vaporization of 36.02
kJ/mol.36.02 kJ/mol. At what Kelvin temperature will the vapor
pressure be 3.503.50 times higher than it was at 347 K?
2) A total of 767 cal767 cal of heat is added to 5.00 g5.00 g of
ice at −20.0 °C.−20.0 °C.
What is the final temperature of the water?
Specific heat of H2O(s)H2O(s)
2.087 J/(g⋅°C)2.087 J/(g⋅°C)
Specific heat of H2O(l)H2O(l)
4.184 J/(g⋅°C)4.184 J/(g⋅°C)
Heat of fusion for H2OH2O
333.6...

If 42.0 kJ of heat is added to a 32.0-g sample of liquid methane
under 1 atm of pressure at a temperature of -170 ∘C, what is the
final state of the methane once the system equilibrates? Assume no
heat is lost to the surroundings. The normal boiling point of
methane is -161.5 ∘C. The specific heats of liquid and gaseous
methane are 3.48 and 2.22 J/g⋅K, respectively.
Why is it be gas veres liqiud?
also
What is the final...

You add 50.0 g of ice initially at ‒20.0 °C to 1.00 x
102 mL warm water at 67.0 °C. When all the ice melts,
the water temperature is found to be somewhere above 0 °C.
Calculate the final temperature of the water.
[ Cice = 2.06 J/g⋅°C; CH2O = 4.184 J/g⋅°C;
dH2O = 1.00 g/mL; heat of fusion of water = 333 J/g
]

A 275-g sample of nickel at 100.0°C is placed in 100.0 mL of
water at 22.0°C. What is the final temperature of the water? Assume
that no heat is lost to or gained from the surroundings. Specific
heat capacity of nickel = 0.444 J/(g·K). a. 40.8°C b. 61.0°C c.
39.6°C d. 82.4°C e. 79.2°C

A 190 g copper bowl contains 230 g of water, both at 22.0°C. A
very hot 430 g copper cylinder is dropped into the water, causing
the water to boil, with 6.44 g being converted to steam. The final
temperature of the system is 100°C. Neglect energy transfers with
the environment. (a) How much energy is transferred to the water as
heat? (b) How much to the bowl? (c) What is the original
temperature of the cylinder? The specific heat...

A 110 g copper bowl contains 100 g of water, both at 22.0°C. A
very hot 360 g copper cylinder is dropped into the water, causing
the water to boil, with 7.52 g being converted to steam. The final
temperature of the system is 100°C. Neglect energy transfers with
the environment. (a) How much energy is transferred to the water as
heat? (b) How much to the bowl? (c) What is the original
temperature of the cylinder? The specific heat...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 16 minutes ago

asked 26 minutes ago

asked 38 minutes ago

asked 38 minutes ago

asked 49 minutes ago

asked 56 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