An orange contains 445 kJ of energy. What mass of water could this same amount of energy raise from 25.0 degrees C to the boiling point?

What is the boiling point?
Equation?
Thanks

q = mass water x specific heat water x delta T.

q = 445,000 joules. delta T = 100-25.

1.42KG

Well, well, well, looks like we have a fruity energy question here! Let's peel away the details, shall we?

To figure out how much water this amount of energy can raise, we need to take into account the specific heat capacity of water. For water, the specific heat capacity is approximately 4.184 J/g°C.

Now, let's assume the boiling point of water is the standard 100°C. With that in mind, we can set up an equation using the formula:

Energy = mass of water x specific heat capacity x change in temperature.

Since we know the energy (445 kJ) and the initial temperature (25.0°C), we can plug these values into the equation and solve for the mass of water.

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To find the mass of water that could be raised from 25.0 degrees C to the boiling point using the given energy, we need to use the specific heat capacity equation.

The specific heat capacity equation is given as:

q = mcΔT

Where:
q = energy (in joules)
m = mass (in grams)
c = specific heat capacity (in J/g°C)
ΔT = change in temperature (in °C)

First, we need to convert the given energy from kJ to J:

445 kJ = 445,000 J

Given information:
Energy (q) = 445,000 J
Initial temperature (T1) = 25.0°C

To find the mass of water (m), we also need the specific heat capacity of water (c). The specific heat capacity of water is approximately 4.18 J/g°C.

The boiling point of water is 100°C at standard atmospheric pressure.

Now, let's substitute the values into the equation:

q = mcΔT
445,000J = m(4.18J/g°C)(100°C - 25.0°C)

Now, solve for m:

445,000J = (4.18J/g°C)(75.0°C)m

Divide by (4.18J/g°C)(75.0°C) on both sides:

m = 445,000J / (4.18J/g°C)(75.0°C)

m ≈ 1532 grams

Therefore, the mass of water that can be raised from 25.0 degrees C to the boiling point using the given energy is approximately 1532 grams.

Please note that this calculation assumes no energy losses to the surroundings and that the specific heat capacity of water remains constant over the temperature range.

To determine the mass of water that can be raised from 25.0°C to the boiling point using the energy content of an orange, we need to know the specific heat capacity of water and the equation relating energy, mass, specific heat capacity, and temperature change.

The boiling point of water at standard atmospheric pressure is 100°C or 373.15 K.

The equation we can use is:

Q = m * c * ΔT

Where:
Q = energy (in joules or kilojoules)
m = mass of the substance (in grams or kilograms)
c = specific heat capacity of the substance (in J/g·K or kJ/kg·K)
ΔT = change in temperature (final temperature - initial temperature) (in °C or K)

In this case, we want to find the mass of water, so we rearrange the equation:

m = Q / (c * ΔT)

Given:
Q = 445 kJ (energy content of the orange)
c = 4.18 J/g·K (specific heat capacity of water)
ΔT = boiling point temperature - initial temperature = 100°C - 25.0°C = 75.0°C

Now, let's calculate the mass of water:

m = 445 kJ / (4.18 J/g·K * 75.0°C)

First, we need to convert kJ to J:

445 kJ * 1000 = 445000 J

Now, we can substitute the values into the equation and solve for the mass:

m = 445000 J / (4.18 J/g·K * 75.0°C)

m = 1668.66 g

Therefore, the mass of water that the energy content of the orange can raise from 25.0°C to the boiling point is approximately 1668.66 grams.