5.00 g of octane are burned in a bomb calorimeter containing 2.00 * 10^2 g of water. how many Calories of energy are released if the water temperature increases 6.00 degrees C?
q = mass x specific heat x delta T.
That's mass H2O x sp.h.H2O x delta T water.
do i use the 5.00 g or the 2.00 * 10^2 g?
ok so it'd be
(2.00*10^2)(6.00 degree C) and then what would be the specific heat?
specific heat of h2o is 4.184
i got 5020.8
you have to convert it from joules to calories and idk that off hand but other then that it looks good so far
ok, we didn't do joules in class, so hopefully that's what my teacher wants. thank you!
To calculate the amount of energy released, we need to use the equation:
q = m * C * ΔT
Where:
q = heat energy
m = mass of the water
C = specific heat capacity of water
ΔT = change in temperature
First, let's calculate the heat energy released by the combustion of octane.
We need to know the heat of combustion for octane. The heat of combustion of octane is approximately 55 kilojoules per gram.
Since we have 5.00 grams of octane, the total heat energy released during combustion is:
Q_octane = (5.00 g) * (55 kJ/g)
Q_octane = 275 kJ
Next, we can calculate the heat energy absorbed by water to increase its temperature.
Given:
Mass of water (m) = 200 g
Change in temperature (ΔT) = 6.00 degrees C
The specific heat capacity of water (C) is approximately 4.18 J/g°C, or 4.18 kJ/kg°C.
First, we need to convert the mass of water from grams to kilograms:
m_water = 200 g / 1000 = 0.200 kg
Now, we can calculate the heat energy absorbed by the water:
Q_water = (m_water) * (C) * (ΔT)
Q_water = (0.200 kg) * (4.18 kJ/kg°C) * (6.00 °C)
Q_water = 5.04 kJ
Finally, to find the total heat energy released, we need to convert the heat energy from kilojoules to Calories (1 Cal = 4.184 kJ):
Q_total = (Q_octane + Q_water) / 4.184
Q_total = (275 kJ + 5.04 kJ) / 4.184
Q_total ≈ 65.48 Calories
Therefore, approximately 65.48 Calories of energy are released during the combustion of 5.00 g of octane in a bomb calorimeter containing 200 g of water when the water temperature increases by 6.00 degrees Celsius.