a student mixed a 50.0mL of water containing 0.50 mols of HCl at 22.5 degC with 50.0 mL of water containing 0.50 mol NaOH at 22.5 degC in a foam cup calorimeter.the temp increases to 26.0 degC. how much heat in kJ was released by the reaction? please show how you found the answer so i can understand how you did it.
how many moles are present in 56.2L of NE(g)?
q = mass x specific heat x delta T.
mass = 100 g (I assume we assume the density of the solution is 1.00 g/mL).
specific heat = 4.184 J/g*C
delta T = 26.0 - 22.5 = ??
q will be in Joules and you will need to convert to kJ.
You should not piggy back on another question. Often these questions get overlooked.
moles = grams/molar mass.
By the way, there is no such thing as NE. I assume you meant Ne.
To find out how much heat was released by the reaction, we need to use the equation:
q = m * c * ΔT
Where:
q = heat (in joules)
m = mass (in grams)
c = specific heat capacity (in J/g°C)
ΔT = change in temperature (in °C)
Here's how we can calculate the heat released step by step:
1. Convert the volume of the solutions to mass, assuming a density of 1.00 g/mL for water:
- For the HCl solution:
Mass of HCl solution = Volume of HCl solution * density of water
= 50.0 mL * 1.00 g/mL
= 50.0 g
- For the NaOH solution:
Mass of NaOH solution = Volume of NaOH solution * density of water
= 50.0 mL * 1.00 g/mL
= 50.0 g
2. Calculate the total mass of the solution:
Total mass of the solution = Mass of HCl solution + Mass of NaOH solution
= 50.0 g + 50.0 g
= 100.0 g
3. Calculate the moles of HCl and NaOH:
Moles of HCl = 0.50 mol
Moles of NaOH = 0.50 mol
4. Determine the enthalpy change (∆H) for the reaction between HCl and NaOH. It can be assumed that the reaction is exothermic, so the heat released is negative (-∆H).
5. Calculate the heat released using the equation:
q = m * c * ΔT
Here comes the challenging part—the specific heat capacity (c) needs to be known. Unfortunately, the specific heat capacity is not given for the solution. We could use an estimated value for dilute aqueous solutions, which is approximately 4.18 J/g°C. However, it's important to note that this value is an approximation and might not be entirely accurate.
Let's assume a specific heat capacity of 4.18 J/g°C for the calculation:
6. Calculate the change in temperature (ΔT):
ΔT = Final temperature - Initial temperature
= 26.0°C - 22.5°C
= 3.5°C
7. Calculate the heat released (q):
q = m * c * ΔT
= 100.0 g * 4.18 J/g°C * 3.5°C
= 1463 J
Finally, we can convert the answer to kilojoules (kJ):
1463 J * (1 kJ / 1000 J)
= 1.463 kJ
Therefore, approximately 1.463 kJ of heat was released by the reaction between HCl and NaOH.