Question

Lake Erie contains roughly 4.20E+11 m3 of water. How much heat is required to raise the temperature of that volume of water from 11.3oC to 12.0oC? How many years would it take to supply this amount of heat by using the full output of a 1120 MW electric power plant? Do not enter unit.

Answer #1

given that

volume V = 4.2*10^11 m^3

change in temperature T = (12-11.3) = 0.7 C

a) heat energy Q = mcT

here m = density*volume = 1000*4.2*10^11 = 4.2*10^14 kg

c = specific heat of water = 4.186*10^3 J/kg C

Q = 4.2*10^14*4.186*10^3 *0.7

Q = 1.231*10^18 J

b) from the relation

power p = energy/time

time = Q/p = 1.231*10^18/1120*10^6

t = 1.099*10^9 sec

t = 1.099*10^9*(1/3.154*10^7)

t = 34.84 yrs

Lake Erie contains roughly 4.00 ✕ 1011 m3
of water.
(a) How much energy is required to raise the temperature of that
volume of water from 14.4°C to 25.4°C? (Assume the density of this
water to be equal to that of water at 20°C and 1 atm.)
J
(b) How many years would it take to supply this amount of energy by
using the 1,400-MW exhaust energy of an electric power plant?
yr

Lake Erie contains roughly 4.00 ✕ 1011 m3
of water.
(a) How much energy is required to raise the temperature of that
volume of water from 15.4°C to 22.6°C? (Assume the density of this
water to be equal to that of water at 20°C and 1 atm.)
J
(b) How many years would it take to supply this amount of energy by
using the 1,400-MW exhaust energy of an electric power plant?
yr

(a) How much heat is required to raise by 13.20°C the
temperature of 1.7 kg of water.
(b) How much heat is required to raise by 13.20°C the
temperature of 1.7 kg of iron.

(a)
How much heat transfer (in kcal) is required to raise the
temperature of a 0.550 kg aluminum pot containing 3.50 kg of water
from 25.0°C to the boiling point and then boil away 0.650 kg of
water?
(b)
How long (in s) does this take if the rate of heat transfer is
600 W (1 watt = 1 joule/second (1 W = 1 J/s))?

(a)
How much heat transfer (in kcal) is required to raise the
temperature of a 0.600 kg aluminum pot containing 2.00 kg of water
from 40.0°C to the boiling point and then boil away 0.850 kg of
water?
kcal
(b)
How long (in s) does this take if the rate of heat transfer is
600 W (1 watt = 1 joule/second (1 W = 1 J/s))?
s

(a)
How much heat transfer (in kcal) is required to raise the
temperature of a 0.700 kg aluminum pot containing 1.50 kg of water
from 35.0°C to the boiling point and then boil away 0.800 kg of
water?
? kcal
(b)
How long (in s) does this take if the rate of heat transfer is
550 W (1 watt = 1 joule/second (1 W = 1 J/s))?
? s
Please explain each step thoroughly and why, I am really
confused.

(a) How much heat transfer is required to raise the temperature
of a 0.750-kg copper pot containing 2.50 kg of water from 30.0ºC to
the boiling point and then boil away 0.750 kg of water?
(b) How long does this take if the rate of heat transfer is 555
W 1 watt = 1 joule/second (1 W = 1 J/s) ? Answer in seconds.

4. In total, how much heat is required to raise the temperature
of a 450 g sample of water (c = 4.18 J/oC.g) in a saucepan that has
a heat capacity of 300 J/oC from 200C to 75oC?

How much heat is required for the following:
a) Raise the temperature from -10°C to 0°C for a 50kg block of
ice.
b) Melt the ice to water
c)Heat the water to 100°C.
d) Evaporate all the water.
e) Compute the total heat supplied.

(a)
How much heat transfer (in kJ) is necessary to raise the
temperature of a 0.210 kg piece of ice from −24.0°C to 134°C,
including the energy needed for phase changes? (Assume the
substance remains at a constant volume throughout each stage of the
heating process.)
kJ
(b)
How much time (in s) is required for each stage, assuming a
constant 20.5 kJ/s rate of heat transfer? (Enter your answers as a
comma-separated list. Enter your times in order from...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 6 minutes ago

asked 34 minutes ago

asked 34 minutes ago

asked 35 minutes ago

asked 43 minutes ago

asked 49 minutes ago

asked 53 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago