The density of a 1.0 M solution of NaCl is 1.04 g/mL and its specific heat, c, is 3.06 J/C*g. How much heat is absorbed by 3.14 mL of this solution if the temperature rises from 18.6C to 29.7C?
q=m*C*delta T
(1.04g)(3.06)(11.1K)=35.32 is that right?
1.04(g/ml)*3.06(J/g/°K)*11.1(°K)
The expression is missing the volume of 3.14 ml.
However, I have doubts as to the value of 3.06 J/g/°K which seems low.
Was there a typo? 4.06 seems to be in the right order of magnitude.
To calculate the amount of heat absorbed by the solution, we can use the formula:
q = m * c * ΔT,
where:
q is the amount of heat absorbed (in Joules),
m is the mass of the solution (in grams),
c is the specific heat capacity of the solution (in J/C*g),
ΔT is the change in temperature (in Celsius).
Given:
Density of the solution (NaCl) = 1.04 g/mL,
Volume of the solution = 3.14 mL,
Temperature change (ΔT) = 29.7°C - 18.6°C = 11.1°C,
Specific heat capacity of the solution (c) = 3.06 J/C*g.
To find the mass of the solution, we can use the density formula:
density = mass / volume,
mass = density * volume.
mass = (1.04 g/mL) * (3.14 mL),
mass = 3.4176 g (rounded to 4 decimal places).
Now we can substitute the values into the heat formula:
q = (3.4176 g) * (3.06 J/C*g) * (11.1°C).
Calculating the right side of the equation:
q = 115.375416 J (rounded to 3 decimal places).
Therefore, the amount of heat absorbed by 3.14 mL of this 1.0 M NaCl solution is approximately 115.375 J.
To calculate the amount of heat absorbed by the solution, you can use the formula q = m * c * ΔT, where q is the heat absorbed, m is the mass of the solution, c is the specific heat capacity, and ΔT is the change in temperature.
First, let's calculate the mass of the solution:
The density of the solution is given as 1.04 g/mL. So, for 3.14 mL of the solution, the mass can be calculated as follows:
mass = volume * density
mass = 3.14 mL * 1.04 g/mL
mass = 3.2736 g
Now, we can substitute the values into the formula:
q = m * c * ΔT
q = 3.2736 g * 3.06 J/(C*g) * (29.7°C - 18.6°C)
q ≈ 35.35 J
So, the correct answer is approximately 35.35 J, which is equivalent to 35.3 J when rounded to two significant figures.