Calculate the amount of heat (in calories) absorbed when 50.0g of water at 20C spreads over your skin and warms to body temperature, 37C.
I don't understand how to figure this out - which number is the specific heat number? 20C or 37C? I know delta temp will be 17C and mass is 50.0g. (using formula: Amount of Heat = Specific Heat x Mass X (Temp 2 - Temp 1).
Specific heat is neither of those numbers. Those numbers are T2 and T1. The specific heat of water in calories is 1 cal per grams per degree C.
Well, let me enlighten you with my humorous wisdom! When it comes to getting the specific heat number, we need to find the C in Calorie, it stands for Comedy! Just kidding! It actually stands for specific heat capacity. The specific heat capacity of water is approximately 1 calorie/gram °C. So, the specific heat number you're looking for is actually 1 calorie/gram °C.
Now, let's plug in the numbers into the formula you mentioned. We have a mass of 50.0g, a temperature change of 17°C (37°C - 20°C), and a specific heat of 1 calorie/gram °C. Now, just pop that into the formula and calculate!
Amount of Heat = 1 calorie/gram °C x 50.0g x (37°C - 20°C)
Now, grab your calculator and solve the equation to find the amount of heat absorbed. Remember to stay cool while doing the calculations!
In this case, the specific heat number refers to the specific heat capacity of water, which is a constant value. The specific heat capacity of water is typically given as 1 calorie/gram/degree Celsius (cal/g°C) or 4.18 joules/gram/degree Celsius (J/g°C).
To calculate the amount of heat absorbed by the water when it warms from 20°C to 37°C, you can use the formula: Amount of Heat = Specific Heat x Mass x ΔTemp.
Given that the mass is 50.0g, ΔTemp is 37°C - 20°C = 17°C, and the specific heat capacity of water is 1 cal/g°C, we can substitute these values into the formula:
Amount of Heat = 1 cal/g°C x 50.0g x 17°C
To calculate the result, you multiply the values together:
Amount of Heat = 850 cal
Therefore, when 50.0g of water at 20°C spreads over your skin and warms to body temperature (37°C), it will absorb 850 calories of heat.
To calculate the amount of heat absorbed when water spreads over your skin and warms up, you need to know the specific heat of water. The specific heat is the amount of heat energy required to raise the temperature of a given mass of a substance by 1 degree Celsius (or 1 Kelvin).
In this case, you are given the initial temperature (20°C) and the final temperature (37°C) of the water. The temperature change or delta temp is the difference between the final temperature and the initial temperature, which is 37°C - 20°C = 17°C.
Now, you mentioned that you're unsure which number represents the specific heat. The specific heat value for water is approximately 1 calorie/gram °C. So, in this case, the specific heat of water is 1 calorie/gram °C.
To calculate the amount of heat absorbed using the formula: Amount of Heat = Specific Heat × Mass × (Temp 2 - Temp 1), you can now substitute the known values:
Amount of Heat = 1 calorie/gram °C × 50.0g × 17°C
Now you can solve for the amount of heat absorbed:
Amount of Heat = 1 × 50.0 × 17 = 850 calories.
Therefore, when 50.0g of water at 20°C spreads over your skin and warms to body temperature (37°C), it absorbs 850 calories of heat.