i am so confused :((((((((((((((((((((
the specific heat of a solution is 4.18J/g.C and its density is 1.02 g/ml. the solution is formed by combining 25.0 ml of solution a and 25.0 ml of solution b, with each solution initially at 21.4C. the final temperature of the combined solutions is 25.3 C. calculate the heat of reaction assuming no heat loss to he calorimeter. use correct sig figs
the specific heat of a solution is 4.18J/g.C and its density is 1.02 g/ml. the solution is formed by combining 25.0 ml of solution a and 25.0 ml of solution b, with each solution initially at 21.4C. the final temperature of the combined solutions is 25.3 C. calculate the heat of reaction assuming no heat loss to he calorimeter. use correct sig figs
-
Assume the volumes added together = 50.0 mL (25.0 + 25.0) mL
d = m / V
m = d V = 1.02 g/mL x 50.0 mL = 51.0 g
Q = m x dT x SH, where Q is heat, m is mass, dT is temperature change, and SH is specific heat.
Q = 50.1 g x 3.9 C x 4.18 J/gC = 831 J = 830 J (2 sig figs because dT has only 2 sig figs)
d = m / V
m = d V = 1.02 g/mL x 50.0 mL = 51.0 g
Q = m x dT x SH, where Q is heat, m is mass, dT is temperature change, and SH is specific heat.
Q = 50.1 g x 3.9 C x 4.18 J/gC = 831 J = 830 J (2 sig figs because dT has only 2 sig figs)