2. 50.0 mL of 1 M NaOH(aq) and 50.0 mL of 1 M HNO3(aq), both initially at 18.6°C, were mixed in a Styrofoam cup calorimeter. The temperature of the solution rose to 25.4°C. How much heat was released? Assume that the heat capacity and density of the solution are the same as water. Show all working.
vbnfg
To determine the amount of heat released in this reaction, we can use the equation:
q = m * c * ΔT
Where:
q is the heat released or absorbed (in Joules)
m is the mass of the solution (in grams)
c is the specific heat capacity of the solution (in J/g°C)
ΔT is the change in temperature (in °C)
First, let's calculate the mass of the solution by using the density of water. The density of water is approximately 1 g/mL, so the total volume of the solution is 100 mL (50 mL + 50 mL). Therefore, the mass of the solution is:
mass = volume * density = 100 mL * 1 g/mL = 100 g
Next, we need to calculate the change in temperature. The initial temperature of the solution is 18.6°C, and it rose to 25.4°C, so:
ΔT = final temperature - initial temperature = 25.4°C - 18.6°C = 6.8°C
Now, we need to determine the specific heat capacity of the solution. Since it is assumed to be the same as water, the specific heat capacity of water is given as 4.18 J/g°C.
Substituting the values into the formula:
q = m * c * ΔT
q = 100 g * 4.18 J/g°C * 6.8°C
q = 2854.4 J
Therefore, the amount of heat released is 2854.4 Joules.