50.0 mL of water is heated from 60 C to 85 C. How much heat was absorbed by the water sample in joule
Can anybody help me understand the process or rules to figuring this out? Thanks
To calculate the amount of heat absorbed by a substance, you can use the equation:
Q = m * c * ΔT
Where:
Q is the amount of heat absorbed (in joules),
m is the mass of the substance (in grams or kilograms),
c is the specific heat capacity of the substance (in J/g°C or J/kg°C), and
ΔT is the change in temperature of the substance (in °C).
In this case, you are provided with the volume of water (50.0 mL), which we can assume to be equivalent to its mass since the density of water is about 1 g/mL. So, the mass of the water is 50.0 g.
You also know the change in temperature (ΔT) is 85°C - 60°C = 25°C.
Now, you need to use the specific heat capacity of water (c), which is approximately 4.18 J/g°C.
Plugging these values into the equation, you can solve for Q:
Q = 50.0 g * 4.18 J/g°C * 25°C
Q = 5235 J (rounded to the nearest whole number)
Therefore, the amount of heat absorbed by the water sample is 5235 joules.