Question

13. You are using a nozzle to extinguish a fire. The nozzle is delivering at a rate of 100
gallons per minute. You open the nozzle and water flows for 30 seconds. (Therefore you flowed
50 gallons and a gallon of water weighs 8.34 pounds.) The water in the nozzle is at room
temperature which is 20°C. The water hits the fire and it absorbs heat, raising the temperature
of the water to 95°C.
Using the following formula, calculate how much energy, in joules, was required to raise the
temperature of the volume of water from 20°C to 95°C.
Z
You will need to convert to metric because the temperature is in Celsius; therefore your
answer will be in joules or kilojoules. The specific heat of water is 4.18 J/g °C.
Show your work for partial credit.
q=CPMAT

Answer 1

The amount of energy is the energy needed to extinguish the fire

The amount of energy is 1187.0 kilojoules

How to calculate the amount of energy

The given parameters are:

• Mass, m = 8.34 pounds
• Initial Temperature = 20°C
• Final Temperature = 95°C
• Specific heat of water, C = 4.18 J/g °C.

Start by converting the mass from pounds to grams

$m = 8.34\ lb$

Convert

$m = 8.34 * 454\ g$

$m = 3786.36\ g$

The amount of energy is then calculated as:

$q = C_p * m * \Delta T$

So, we have:

$q = 4.18 * 3786.36 * (95 - 20)$

Evaluate the product

$q = 1187023.86j$

Express as kilojoule

$q = 1187023.86 * 0.001 kJ$

$q = 1187.02386kJ$

Approximate

$q = 1187.0kJ$

Hence, the amount of energy is 1187.0 kilojoules

Read more about specific heat capacity at:

https://brainly.com/question/13439286