Question

1) How much energy, in joules, is needed to change 26.5 g of solid water at 0.0 deg C to liquid water at 48.3 deg C?​

Answer 1

Answer:

Q = 5350.2 Joules.

Explanation:

Given the following data;

Mass, m = 26. 5g

Initial temperature, T1 = 0°C

Final temperature, T2 = 48.3°C

Specific heat capacity of water, c = 4.18 J/g°C.

*To find the quantity of heat*

Heat capacity is given by the formula;

$Q = mcdt$

Where;

• Q represents the heat capacity or quantity of heat.

• m represents the mass of an object.

• c represents the specific heat capacity of water.

• dt represents the change in temperature.

dt = T2 - T1

dt = 48.3 - 0

dt = 48.3°C

Substituting the values into the equation, we have;

$Q = 26.5*4.18*48.3$

Q = 5350.2 Joules.

Therefore, the amount of heat absorbed is 5350.2 Joules.