A generic solid, X, has a molar mass of 77.7 g/mol. In a constant-pressure calorimeter, 31.2 g of X is dissolved in 289 g of water at 23.00 °C.
The temperature of the resulting solution rises to 24.40 °C. Assume the solution has the same specific heat as water, 4.184 J/(g·°C), and that there\'s negligible heat loss to the surroundings. How much heat was absorbed by the solution?
How much heat was absorbed by the solution?
q = mass H2O X specific heat H2O x (Tfinal-Tinitial)
All the rest of that info is not needed UNLESS you want delta H/g and/or delta H/mol.
dH/g = q/31.2
dH/mol = q/g x (77.7 g/mol) = ?
Well, it seems like solid X really caused a heated situation! Let's calculate how much heat was absorbed.
To calculate the heat absorbed, we can use the equation:
q = m × c × ΔT
Where q is the heat absorbed, m is the mass of the solution, c is the specific heat capacity of water, and ΔT is the change in temperature.
First, let's find the mass of the solution. We have 31.2 g of X and 289 g of water, so the total mass of the solution is 31.2 g + 289 g = 320.2 g.
Now, let's plug the values into the equation:
q = 320.2 g × 4.184 J/(g·°C) × (24.40 °C - 23.00 °C)
Calculating that out, we get:
q = 320.2 g × 4.184 J/(g·°C) × 1.4 °C
Which gives us:
q = 1870.8016 J
So, the heat absorbed by the solution is approximately 1870.8016 J.
To calculate the heat absorbed by the solution, you can use the equation:
q = m * c * ΔT
Where:
q = heat absorbed by the solution
m = mass of the solution
c = specific heat capacity of water
ΔT = change in temperature of the solution
First, let's calculate the mass of the solution:
mass of the solution = mass of solid + mass of water
mass of the solution = 31.2 g + 289 g
mass of the solution = 320.2 g
Next, calculate the change in temperature of the solution:
ΔT = final temperature - initial temperature
ΔT = 24.40 °C - 23.00 °C
ΔT = 1.40 °C
Now, substitute the values into the equation:
q = 320.2 g * 4.184 J/(g·°C) * 1.40 °C
q = 1888.9248 J
Therefore, the heat absorbed by the solution is approximately 1888.92 J.
To calculate the heat absorbed by the solution, you can use the formula:
q = m * c * ΔT
where:
q = heat absorbed by the solution
m = mass of the solution
c = specific heat of the solution
ΔT = change in temperature of the solution
First, let's calculate the mass of the solution:
mass of solution = mass of water + mass of X
mass of solution = 289 g + 31.2 g
mass of solution = 320.2 g
Now, we can calculate the change in temperature:
ΔT = final temperature - initial temperature
ΔT = 24.40 °C - 23.00 °C
ΔT = 1.40 °C
Since the solution has the same specific heat as water, we can use the specific heat of water (4.184 J/(g·°C)) for our calculation.
Plugging the values into the formula:
q = 320.2 g * 4.184 J/(g·°C) * 1.40 °C
Calculating this expression gives us the amount of heat absorbed by the solution.