For the reaction NaOH + HCl---> H20 + NaCl where the mass of NaOH is 2g and the Volume of Hcl is 100ml with a 0.5 concentration. The initial temp is 25 and the final is 35, what is the amount of energy absorbed by the solution?
with a 0.5 WHAT concentration.
To calculate the amount of energy absorbed or released by the solution during a chemical reaction, we can use the formula:
q = m × C × ΔT
where:
q = amount of energy absorbed or released (in joules)
m = mass of the solution (in grams)
C = specific heat capacity of the solution (in joules per gram per degree Celsius)
ΔT = change in temperature (final temperature – initial temperature)
To find the mass of the solution, we need to consider both the NaOH and HCl. Since the reaction is a complete neutralization reaction, the moles of NaOH and HCl will be in a 1:1 ratio according to the balanced equation.
To calculate the moles of NaOH:
moles of NaOH = mass / molar mass
Given that the mass of NaOH is 2g and the molar mass of NaOH is approximately 40 g/mol, we can calculate the moles of NaOH:
moles of NaOH = 2g / 40 g/mol = 0.05 mol
Since the mole ratio is 1:1, this means we also have 0.05 moles of HCl.
To calculate the mass of HCl, we can use the concentration:
mass of HCl = volume × concentration × density
Given that the volume of HCl is 100 mL and the concentration is 0.5 mol/L (Molar), we need to convert the volume to liters:
volume = 100 mL = 0.1 L
Now we can calculate the mass of HCl:
mass of HCl = 0.1 L × 0.5 mol/L × density of HCl
The density of HCl is approximately 1.19 g/mL. Therefore:
mass of HCl = 0.1 L × 0.5 mol/L × 1.19 g/mL = 0.0595 g
Now we have the total mass of the solution:
mass of solution = mass of NaOH + mass of HCl = 2g + 0.0595 g = 2.0595 g
Next, we need to determine the specific heat capacity (C) of the solution. The specific heat capacity depends on the composition of the solution, so we will assume it to be close to the specific heat capacity of water, which is approximately 4.18 J/g°C.
Now we can calculate the amount of energy absorbed or released by the solution (q):
q = 2.0595 g × 4.18 J/g°C × (35°C - 25°C) = 86.207 J
Therefore, the amount of energy absorbed by the solution during the reaction is approximately 86.207 joules.