If I use 0.524g of Mg to react with 60.0mL of 1.0M H+. The density of H+ is 1.00 g/mL, and the specific heat capacity equals what water's is. The Final and Initial temp. are 65.8 and 22.
Mg(s) + 2H+(aq) ----> Mg2+(aq) + H2(g)
so to find the deltaH of this reaction .. i think i do this ...
4.184 x 60g x [65.8-22)
i'm just unsure if its 60g or some other mass i use instead ?
and how would i find the delta H of the reaction per mole of magnesium?!?!?
Yes, the 60 is correct. It's the solution that is absorbing the heat; therefore, the mass to use is that of the solution. What you have calculated is Joules for the reaction of 0.524 g Mg.
J/g = q/0.524. You can convert to J/mol from J/g x (atomic mass Mg/1 mol) = ??. The usual way to report data of this type is kJ/mol so you may want to convert J/mol to kJ/mol.
Well, it seems you're trying to calculate the change in enthalpy (ΔH) for the given reaction. Let's break it down step by step, shall we?
First, we need to calculate the heat gained or lost by the system using the formula:
q = mcΔT
Where q is the heat, m is the mass, c is the specific heat capacity, and ΔT is the temperature change.
In this case, we know the initial and final temperatures (22°C and 65.8°C), and the density of H+ (1.00 g/mL). However, we need the mass of the hydrogen ions (H+). Since we have the volume and density, we can calculate the mass using the formula:
mass = volume × density
Therefore, the mass of H+ is 60.0 mL × 1.00 g/mL = 60.0 g. It's always a fun game to find the mass!
Now we have everything we need to calculate the heat:
q = mcΔT
q = (60.0 g) × (4.184 J/g °C) × (65.8 °C - 22.0 °C)
Calculating that out will give you the heat change (q) for the reaction.
To find the ΔH of the reaction per mole of magnesium, you need to use stoichiometry. In the balanced equation, we see that 1 mole of magnesium reacts with 2 moles of hydrogen ions. So, divide the heat change (q) by the moles of magnesium used (which you can calculate using its molar mass). This will give you ΔH per mole of magnesium.
Remember, chemistry can be quite entertaining once you get into the swing of things!
To calculate the enthalpy change (ΔH) of the reaction per mole of magnesium, you need to use the balanced equation to determine the stoichiometry of the reaction.
The balanced equation is: Mg(s) + 2H+(aq) -> Mg2+(aq) + H2(g)
From the balanced equation, you can see that for each mole of magnesium, you need 2 moles of H+. So, to find the moles of H+ in the reaction, you can use the following formula:
moles of H+ = volume of H+ solution (L) x molarity of H+ solution (mol/L)
Given that the volume of H+ solution is 60.0 mL (or 0.060 L) and the molarity of H+ solution is 1.0 M, you can calculate the moles of H+ as follows:
moles of H+ = 0.060 L x 1.0 mol/L = 0.060 mol
Since there is a 1:1 stoichiometric ratio between H+ and Mg in the balanced equation, the moles of H+ also represent the moles of Mg used in the reaction.
Now, to calculate the enthalpy change (ΔH) of the reaction per mole of magnesium, you can use the formula:
ΔH = q / moles of Mg
Where q is the heat absorbed or released by the reaction.
It seems like you are trying to calculate q using the formula:
q = mass x specific heat capacity x ΔT
Given the density of H+ as 1.00 g/mL and a volume of 60.0 mL, you can calculate the mass of H+ as:
mass of H+ = volume of H+ solution x density of H+ = 60.0 mL x 1.00 g/mL = 60.0 g
Now, substituting the values into the q formula:
q = 60.0 g x specific heat capacity of water x (65.8 - 22)
However, note that you need to use the specific heat capacity of the H+ solution since it is not the same as water. Also, you'll need to convert the given mass of Mg (0.524 g) to moles of Mg by dividing by the molar mass of Mg (24.31 g/mol). Let's replace this value with the correct mass and solve the equation.
To find the molar mass of Mg, you can refer to the periodic table where the atomic mass of Mg is 24.31 g/mol.
moles of Mg = mass of Mg / molar mass of Mg = 0.524 g / 24.31 g/mol = 0.0215 mol
Now, substitute this value into the equation for ΔH:
ΔH = q / moles of Mg = (60.0 g x specific heat capacity of H+ x (65.8 - 22)) / 0.0215 mol
To find the heat absorbed or released (deltaH) in a reaction, you need to use the formula:
deltaH = mcΔT,
where:
- deltaH is the heat absorbed or released (in joules),
- m is the mass of the substance undergoing the reaction (in grams),
- c is the specific heat capacity of the substance (in J/g·°C),
- ΔT is the change in temperature (in °C).
In this case, you want to find the deltaH of the reaction between 0.524g of Mg and 60.0mL of 1.0M H+. Here's how you can calculate it step by step:
1. Calculate the mass of H+ used:
mass = volume × density
mass = 60.0 mL × 1.00 g/mL
mass = 60.0 g
2. Calculate the change in temperature:
ΔT = final temperature - initial temperature
ΔT = 65.8 °C - 22 °C
ΔT = 43.8 °C
3. Calculate the deltaH using the formula:
deltaH = mcΔT
deltaH = (mass of H+ + mass of Mg) × specific heat capacity of water × ΔT
deltaH = (60.0 g + 0.524 g) × 4.184 J/g·°C × 43.8 °C
Now, let's calculate the deltaH of the reaction and convert it to kilojoules (kJ):
deltaH = (60.524 g) × (4.184 J/g·°C) × (43.8 °C)
deltaH = 109,538.94 J
deltaH = 109,538.94 / 1000 kJ
deltaH = 109.54 kJ
So, the deltaH of the reaction is 109.54 kJ.
To find the deltaH of the reaction per mole of magnesium (ΔH per mole of Mg), you need to know the stoichiometry of the reaction. From the balanced equation, you can see that 1 mole of Mg reacts with 2 moles of H+.
Therefore, to find ΔH per mole of Mg, you divide the deltaH calculated above by the moles of Mg used. First, find the moles of Mg used:
moles of Mg = mass of Mg / molar mass of Mg
moles of Mg = 0.524 g / 24.31 g/mol (molar mass of Mg)
Now, divide the deltaH by the moles of Mg:
ΔH per mole of Mg = deltaH / moles of Mg
Calculating this will give you the deltaH per mole of Mg for the reaction.