<h2>
Δt = 71.67 °C</h2>
The temperature change of water is equal to 71.67 °C
<h3>
Explanation:</h3>
Given:
Amount of transferred energy = 30,000 K J
Mass of water = 100 ml
Initial temperature = 20°C
To find the change in temperature of water.
Formula for Heat capacity is given by
Q = m×c×Δt ........................................(1)
where:
Q = Heat capacity of the substance (in J)
m=mass of the substance being heated in grams(g)
c = the specific heat of the substance in J/(g.°C)
Δt = Change in temperature (in °C)
Δt = (Final temperature - Initial temperature) = T(f) - T(i)
Q = 30,000 J
Mass of water = m = 100 ml
1 ml = 1 g ................................................(2)
Therefore m = 100 ml = 100 g
Specific heat of water is c = 4.186 J /g.
Δt = ?
Substituting these in equation (1), we get
Q = m×c×Δt
Rearranging the terms for Δt,
Δt = ![\frac{Q}{m\times c}](https://tex.z-dn.net/?f=%5Cfrac%7BQ%7D%7Bm%5Ctimes%20c%7D)
Δt = ![\frac{30,000}{100\times 4.186} = \frac{30,000}{418.6}= 71.67\°C](https://tex.z-dn.net/?f=%5Cfrac%7B30%2C000%7D%7B100%5Ctimes%204.186%7D%20%20%3D%20%5Cfrac%7B30%2C000%7D%7B418.6%7D%3D%2071.67%5C%C2%B0C)
Δt = 71.67 °C