Answer:
There is 985.63 J heat required
Explanation:
Step 1: Data given
Number of moles of water = 0.298 moles
Initial temperature = 35.93 °C
Final temperature = 79.84 °C
Specific heat capacity of water = 4.18 J/g°C
Molar mass water = 18.02 g/mol
Step 2: Calculate mass of water
Mass of H2O = Moles of H2O * molar mass H2O
Mass of H2O = 0.298 moles * 18.02 g/mol
Mass of H2O = 5.37 grams
Step 3: Calculate heat energy
Q = m*c*ΔT
⇒ Q = heat energy in J
⇒ m = mass of water = 5.37 grams
⇒ c = the specific heat capacity of water = 4.18 J/g°C
⇒ ΔT = The change in temperature = T2 - T1 = 79.84 - 35.93 = 43.91°C
Q = 5.37g * 4.18 J/g°C * 43.91 °C
Q = 985.63 J
There is 985.63 J heat required
