2 HCl (aq) + Ba (OH2) (aq) ----> BaCl2 + 2 H20 (l)
deltaH = -118 kJ
Calculate the heat when 100.0 mL of 0.500 M HCl is mixed with 300.0 mL of 0.100 M Ba(Oh2). Assuming that the temp. of both solutions was initially 25.0 degrees C and that the final mixture has a mass of 400.0 g and a specific capacity of 4.18 J/g degrees C, calculate the final temp of the mixture.
what's the first step to solving this problem?
i don't even understand what the problem is asking.
Is that 118 kJ delta H for the reaction as written or it is per mol. I will assume it is 118 kJ as written (that is, for 2 mols HCl).
q = mass x sp.h. x (Tf - Ti)
You know q (don't forget to change to Joules), you know mass and sp.h. and Ti (initial T = 25 C). Solve for the one unknown of Tf = final T. Post your work if you get stuck.
is it 28.53 degrees Celsius?
The first step to solving this problem is to determine the moles of each reactant that are being combined. This can be done using the given concentrations and volumes of the solutions.
To find the moles of HCl, you can use the equation:
moles of HCl = concentration of HCl (in M) x volume of HCl (in L)
In this case, the concentration of HCl is 0.500 M and the volume is 100.0 mL (which is equivalent to 0.100 L). Plugging these values into the equation, we get:
moles of HCl = 0.500 M x 0.100 L = 0.050 mol
Similarly, you can find the moles of Ba(OH)2 using its concentration of 0.100 M and volume of 300.0 mL (equivalent to 0.300 L).
moles of Ba(OH)2 = 0.100 M x 0.300 L = 0.030 mol
Now that you have the moles of both reactants, you can proceed to calculate the heat of the reaction and the final temperature of the mixture.