Water has a specific heat of 4.186 J/g°C. How much heat is required to increase 10.0 g of water from 25.0°C to 30.0°C?
The answer is 209.3 J
specific heat * mass * temp change
To calculate the heat required to increase the temperature of water, you can use the formula:
q = m * c * ΔT
Where:
q = heat energy
m = mass of the water
c = specific heat capacity of water
ΔT = change in temperature
Given:
m = 10.0 g
c = 4.186 J/g°C
ΔT = 30.0°C - 25.0°C = 5.0°C
Substituting the values into the formula:
q = 10.0 g * 4.186 J/g°C * 5.0°C
q = 209.3 J
Therefore, to increase 10.0 g of water from 25.0°C to 30.0°C, 209.3 J of heat energy is required.
To calculate the amount of heat required to increase the temperature of water, we can use the equation:
Q = mcΔT
Where:
Q is the amount of heat (in Joules)
m is the mass of the water (in grams)
c is the specific heat of water (in J/g°C)
ΔT is the change in temperature (in °C)
Given:
m = 10.0 g
c = 4.186 J/g°C
ΔT = 30.0°C - 25.0°C = 5.0°C
Now, let's substitute the values into the equation to find the amount of heat:
Q = (10.0 g) x (4.186 J/g°C) x (5.0°C)
Q = 209.3 J
Therefore, the amount of heat required to increase the temperature of 10.0 g of water from 25.0°C to 30.0°C is 209.3 Joules.