Question

How much heat in joules is needed to raise the temperature of 4.0 L of water from 0°C to 96.0°C? (Hint: Recall the original definition of the liter.)

since it won't let me go to the physics section

Answer 1

q = mC delta T

m is the mass of water (look up the density of water at 0 C and use it to calculate the mass of 4L)

C is specific heat of water (4.1J/g C)

Delta T is the temperature difference (96-0 C)

Answer 2

okay I just needed the joules conversion I think I have it now

Answer 3

okay so I got it wrong again I am confused

Answer 4

@vocaloid I am still confused

Answer 5

Hint: Recall the original definition of the liter. ----> originally, 1kg = 1L water

so 4.0L water = 4.0kg

using q = mc delta T ---> q = 4.0kg * 1000g/kg * 4.18 J/gC * (96 - 0)C

Answer 6

so are I multiplying the 4*1000 as well?

I multiplied the 4 and 1000 and 4.18 and 96 together and got it wrong?

Answer 7

I only have one more shot at this question

Answer 8

@AZ can you take a look at this when you get a chance

Answer 9

A quantity of steam (800 g) at 123°C is condensed, and the resulting water is frozen into ice at 0°C. How much heat was removed?

Do you know this one? These are the last two I have and it is due tonight

Answer 10

I think I have the answer now would it be 66976?

Answer 11

@vocaloid

Answer 12

I agree with Vocaloid's approach.

Your question wants the heat in joules and not kilojoules so it's not an issue of units. The only reason (I can think of) for why your answer isn't being accepted has to do with sig figs.

For your first question,

4.0 kg * 4180 J/kg C * 96 C
= 1605120
= 1.6 * 10^6 J