Question

If you combine 240.0 mL of water at 25.00 °C and 140.0 mL of water at 95.00 °C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water

Answer 1

Volume of 140 = 240 OmL T = 25°C density = 1.0ogimL & mans = m = 1.00g/mL x 240.0m2 2 240.09. and Up= 4.184 Igrkt me = V₂ x d = 140.0 mL x 1.00g/mL 72= 95.0°C - 140.09. If two liquids are combined (mined) having difference in There temperature. Heat will How until the energy amount going out of the warm water is equal to the energy amount going into the cool crates quast - a gain q=cm (at) (CP bet be the equilibrium temperature attained so. (M) (95°C -1) (Cp) = (m.) (T-25°c) (cp) + m₂ (95°C-T) = m. (T-25°c) - 140.0 (95°C-.7) = 240 (T-25°C) >> 13300 - 1401 - 2401 - 6000 » 13300 +6000 = 240T + 140T 19300 - 3.T To f nn 380 T = 50.78