Question

Calculate the amount of heat needed to raise the temperature of 4 ml of water from 10C to 30C

Answer 1

Answer:

Heat energy (Q) = 334.72

Explanation:

Volume = 4mL

Initial temperature (T1) = 10°C

Final temperature (T2) = 30°C

Mass = ?

Specific heat capacity of water = 4.184J/g°C

Density of water = 1.0g/mL

Heat energy = ?

Density = mass / volume

ρ = mass / vol

Mass = volume × density (ρ)

Mass = 4 × 1.0

Mass = 4g

Heat energy (Q) = mc∇T

Q = heat energy

M = mass of the substance

C = specific heat capacity of the substance

∇T = change in temperature of the substance = T2 - T1

Q = mc(T2 - T1)

Q = 4 × 4.184 ×(30 - 10)

Q = 16.736 × 20

Q = 334.72J

The heat energy required to raise 4ml of water from 10°C to 30°C is 334.72J

Answer 2

Answer:

$Q=334.4J$

Explanation:

Hello,

In this case, for the given heating process, we should use the following equation in order to compute the amount of heat needed for such change in the temperature of water:

$Q=mCp(T_2-T_1)$

Now, since the density of water is 1 g/mL and its heat capacity is 4.18 J/(g*°C), we are able to compute the heat as follows:

$Q=4mL*\frac{1g}{4mL}*4.18\frac{J}{g\°C} (30\°C-10\°C)\\\\Q=334.4J$

Best regards.