A small electric immersion heater is used to boil 191.0 g of water for a cup of instant coffee. The heater is labeled 355.0 W, which means that it converts electrical energy to heat at this rate. Calculate the time required to bring this water from 12.0°C to the boiling point ignoring any heat losses.

nvm got it

To calculate the time required to bring the water from 12.0°C to the boiling point, we need to use the formula:

Q = mcΔT

Where:
Q is the heat energy required in joules (J)
m is the mass of the water in grams (g)
c is the specific heat capacity of water (4.18 J/g°C)
ΔT is the temperature change in degrees Celsius (°C)

First, let's calculate the temperature change:

ΔT = boiling point of water - initial temperature
ΔT = 100°C - 12.0°C
ΔT = 88.0°C

Next, let's convert the mass of water from grams to kilograms:

m = 191.0 g / 1000
m = 0.191 kg

Now we can calculate the heat energy required:

Q = mcΔT
Q = 0.191 kg * 4.18 J/g°C * 88.0°C
Q = 72.25 J

The unit of power (W) tells us that 1 watt is equal to 1 joule per second. So, we can calculate the time required by dividing the heat energy required by the power of the immersion heater:

Time = Q / Power
Time = 72.25 J / 355.0 W
Time = 0.203 seconds

Therefore, it would take approximately 0.203 seconds to bring the water from 12.0°C to the boiling point, assuming no heat losses.