A 5.00-g sample of octane is burned in a bomb calorimeter containing 2.00x10 exponent2 g H2O. How much energyin calis released if the water temperature increases 6.00 Celsius?
energy=masswater*Cwater*6
To calculate the energy released, we can use the formula:
q = m × c × ΔT
Where:
q = heat energy (in calories)
m = mass of water (in grams)
c = specific heat capacity of water (1 cal/g°C)
ΔT = change in temperature (in °C)
Given values:
Mass of octane (m) = 5.00 g
Mass of water (m) = 2.00 x 10^2 g
Change in temperature (ΔT) = 6.00 °C
Let's plug these values into the formula to find the energy released:
q = (2.00 x 10^2 g) × (1 cal/g°C) × (6.00 °C)
q = 1200 cal
Therefore, the amount of energy released is 1200 calories.
To calculate the amount of energy released when a substance is burned, we can use the equation:
q = m × c × ΔT
Where:
q = energy released or absorbed (in calories)
m = mass of the substance (in grams)
c = specific heat capacity of the substance (in cal/g·°C)
ΔT = change in temperature (in °C)
In this case, we're given the mass of octane (5.00 g), the mass of water (2.00 × 10^2 g), and the change in temperature of the water (6.00 °C).
First, we need to determine the specific heat capacity of water. The specific heat capacity of water is approximately 1 cal/g·°C.
Now, we can substitute the values into the equation:
q = (5.00 g + 2.00 × 10^2 g) × 1 cal/g·°C × 6.00 °C
Calculating the expression in parentheses:
q = 7.00 × 10^2 g × 1 cal/g·°C × 6.00 °C
q = 4,200 cal
Therefore, the amount of energy released when the 5.00 g sample of octane is burned is 4,200 calories (cal).