When 50.0 Ml of 1.00 m chi was mixed with 50.0 ml of 1.00 m NaOH in a calorimeter the temperature rose from 25.0 c to 32.0 c calculate the heat change for the reaction assuming that the total volume of the solution is 100.0 ml and the specific heat is 1.00 cal/ (g.c). Is the reaction exothermic or endothermic?

See your post above.

To calculate the heat change for the reaction, you can use the formula:

Q = m * c * ΔT

where:
Q is the heat change (in calories)
m is the mass of the solution (in grams)
c is the specific heat capacity of the solution (in cal/g°C)
ΔT is the temperature change (in °C)

First, let's calculate the mass of the solution. Since the total volume is given as 100.0 mL, which is the sum of 50.0 mL of chi and 50.0 mL of NaOH, we can assume that the density of the solution is approximately equal to the density of water, which is 1.00 g/mL. Therefore, the mass of the solution is:

mass = volume * density = 100.0 mL * 1.00 g/mL = 100.0 g

Now, let's calculate the temperature change (ΔT):

ΔT = final temperature - initial temperature = 32.0°C - 25.0°C = 7.0°C

Since the specific heat capacity (c) is given as 1.00 cal/g°C, we can substitute all the values into the formula to calculate the heat change (Q):

Q = mass * c * ΔT = 100.0 g * 1.00 cal/g°C * 7.0°C = 700 cal

The heat change (Q) for the reaction is 700 calories.

To determine whether the reaction is exothermic or endothermic, we need to consider the temperature change. In this case, the temperature rose from 25.0°C to 32.0°C, indicating an increase in temperature. An increase in temperature implies that heat is absorbed from the surroundings, making the reaction endothermic.