How many calories of heat do you need if you want to raise the temperature of 310 g of gasoline from 17.0°C to 24.0°C? Specific heat of gasoline is 0.40 cal/g·°C.
q needed = [mass gasoline x specific heat gasoline x (Tfinal-Tinitial)
Substitute and solve for q.
To find out how many calories of heat are needed to raise the temperature of gasoline, we can use the formula:
Q = mcΔT
where:
Q = the amount of heat energy
m = mass of the substance (in grams)
c = specific heat of the substance (in cal/g·°C)
ΔT = change in temperature (in °C)
Given values:
m = 310 g (mass of gasoline)
c = 0.40 cal/g·°C (specific heat of gasoline)
ΔT = (24.0°C - 17.0°C) = 7.0°C (change in temperature)
Substituting the given values into the formula:
Q = (310 g) × (0.40 cal/g·°C) × (7.0°C)
Now we can calculate Q:
Q = 868 cal
Therefore, you need 868 calories of heat to raise the temperature of 310 grams of gasoline from 17.0°C to 24.0°C.