q = mc Δt
q= heat, m = mass (in grams), c=specific heat (4.18 J/°C * g or J/K * g for water), Δt = change in temperature (in kelvin)
For this equation:
q = ?, m = 50.0 g, c = 4.18 J/°C *g = 4.18 J/K *g, initial t = 20.0°C, final t = 10°C
To convert from °C to K, add 273 to °C
0°C = 273 K
Initial t = 20.0°C + 273 = 293 K
Final t = 10.0°C + 273 = 283 K
ΔT = final temperature - initial temperature = 283-293 = -10 K
Plug in what you know:
q = (50.0 g) x (4.18 J/K * g) x (-10 K) = -2090
Check sig figs and cancel out units:
Answer: -2090 J (you need 3 sig figs from the original numbers given and the units are Joules since grams and Kelvin cancel out)
Check to make sure answer makes sense:
Since heat energy is released, the answer should be negative. The answer is negative and therefore, makes sense
