A1.2 kg block of iron at 32 ∘c is rapidly heated by a torch such that 12 kj is transferred to it. what temperature would the block of iron reach (assuming the complete transfer of heat and no loss to the surroundings)? if that same amount of heat (12 kj ) was quickly transferred to a 850 g pellet of copper at 27 ∘c, what temperature would the copper reach before it begins losing heat to the surroundings? use the equation for heat capacity and the following heat capacity values:

For iron

Final temperature = 54,22°C

For copper

Final Temperature = 63.67 °C

Explanation

Hello,

You are using a torch to warm up a block of iron that has an initial temperature of 32°C.

The first you have to know is that the "heat capacity" could simply define as the heat required to go from an initial temperature to a final temperature.

So you need to use the heat capacity equation as follow in the paper.

The equation has to have all terms in the same units, so:

q = 12000 J

s = 0.450 J / g °C

m = 1200 g

Ti = 32 °C

Answer is: the polarity arrows should go from sulfur (S) to the oxygen (O).

The magnitude of the dipole depends on the difference in the electronegativies and has direction from positively charged atom to negatively charged atom.

Oxygen has greater electronegativity than sulfur, because of that oxygen (χ=3.5) is partially negative and sulfur (χ=2.5) is partially positive.

Electronegativity (χ) is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.