Calculate the amount of heat necessary to raise the temperature of 12.0 g of water from 15.4ºC to 93ºC. The specific heat of water = 4.18 J/gºC.
q = ms∆T
q = (12.0g) (4.18) (93.0 - 15.4)
q = 3892.416 J ??
Looks ok but I didn't check the calculation.
3892.416 J? That's hotter than a summer day in the desert! Nice job with the calculation. Just remember, heat and temperature have a love-hate relationship. They're always playing this game of catch-up.
To calculate the amount of heat necessary to raise the temperature of a substance, you can use the equation q = ms∆T, where q is the heat, m is the mass of the substance, s is the specific heat, and ∆T is the change in temperature.
In this case, the mass of water (m) is 12.0 g, the specific heat (s) of water is 4.18 J/gºC, and the change in temperature (∆T) is (93.0 - 15.4) = 77.6ºC.
Plugging in these values into the equation, we get:
q = (12.0g) (4.18 J/gºC) (77.6ºC)
q ≈ 3892.416 J
Therefore, the amount of heat necessary to raise the temperature of 12.0 g of water from 15.4ºC to 93ºC is approximately 3892.416 J.
To calculate the amount of heat necessary to raise the temperature of water, you need to use the formula q = ms∆T, where q is the heat energy, m is the mass of the water, s is the specific heat capacity of water, and ∆T is the change in temperature.
In this case, the mass of the water is given as 12.0 g, the specific heat capacity of water is 4.18 J/gºC, and the change in temperature is from 15.4ºC to 93ºC.
Plugging in the values into the formula:
q = (12.0 g) (4.18 J/gºC) (93.0ºC - 15.4ºC)
Calculating the value:
q = 12.0 g * 4.18 J/gºC * (93.0ºC - 15.4ºC)
q = 12.0 g * 4.18 J/gºC * 77.6ºC
q = 3892.416 J
So, the amount of heat necessary to raise the temperature of 12.0 g of water from 15.4ºC to 93ºC is approximately 3892.416 J.