Mango12 said:
a) how much more heat is used to boil 237 mL of water as opposed to starting the car?
b) what major concept/finding was overlooked while solving this problem?
I think this has something to do with delta H = mc(delta t) but idk
Mango12 said:
How much more heat is given off by heating 237mL of water with 216,000J than is used to start the car? I don't have the value of the energy to start the engine, but does anyone know how I could go about solving this if I did?
Hi Mango12! ;)
That actually seem to be different questions.
In your original problem statement we were boiling 237 mL of water.
That means we have:
$$V = 237\text{ mL} \\ \Delta t = 100^\circ\text C - t_{initial}$$
If we know what $t_{initial}$ is, we can calculate the heat required to boil the water.
Can we perhaps assume we start at room temperature ($20^\circ \text C$)?
Or is there perhaps an initial temperature given when starting the car?In your last response we seem to have a different question with:
$$V = 237\text{ mL} \\ \Delta H = 216,000\text{ J}$$
Or is that $\Delta H$ perhaps the heat given off when starting the car?Additionally we have the formula:
$$\Delta H = mc\Delta t$$
where $\Delta H$ is the change in heat, $m$ is the mass, $c$ is the specific heat capacity of water, and $\Delta t$ is the change in temperature.
Do you perchance have $c$ as a constant?
To calculate $m$, we can use:
$$m = \rho V$$
where $\rho$ is the density of water. Do you have that as a constant?After that we can apply the formula.
We'll get to (b) afterwards, since there are some conditions when applying the formulas.
