A person eats a container of yogurt. The Nutritional Facts label states that it contains 195 Calories (1 Calorie = 4186 J). What mass of perspiration would one have to lose to get rid of this energy? At body temperature, the latent heat of vaporizaiton of water is 2.42 106 J/kg.
kg
masswater*Heatvaporization=195*4186
check your units, and solve for the mass of water.
To find the mass of perspiration that one would have to lose to get rid of the energy from eating the container of yogurt, we can use the equation:
Energy = mass * latent heat of vaporization
First, we need to convert the energy from calories to joules. We know that 1 calorie is equal to 4186 joules, so we can calculate:
Energy = 195 Calories * 4186 J/Calorie
Now we have the value for the energy in joules. To find the mass, we can rearrange the equation:
mass = Energy / latent heat of vaporization
Given that the latent heat of vaporization of water is 2.42 * 10^6 J/kg, we can substitute the values into the equation:
mass = (195 Calories * 4186 J/Calorie) / (2.42 * 10^6 J/kg)
Now we can calculate the mass:
mass = (195 * 4186) / (2.42 * 10^6) kg
Simplifying this expression, we find:
mass ≈ 0.334 kg
Therefore, one would have to lose approximately 0.334 kg of perspiration to get rid of the energy from eating the container of yogurt.