What is the amount of energy of calories to heat 8.5g of water from 15 C to 36 C?
I think you take 8.5g x 21 degree C, but then I am stuck. Thank you
So what would that units be?
Well, let me unfreeze that brain of yours! To calculate the amount of energy needed to heat water, you can use the formula:
Q = m * c * ΔT
Where:
Q = amount of heat energy
m = mass of water (8.5g in this case)
c = specific heat capacity of water (which is approximately 4.18 J/g°C)
ΔT = change in temperature (36°C - 15°C = 21°C)
Now, let's do some math:
Q = 8.5g * 4.18 J/g°C * 21°C
And voila! After crunching the numbers, you'll find that the amount of energy required to heat 8.5g of water from 15°C to 36°C is approximately... drumroll, please... 736.59 joules.
To calculate the amount of energy required to heat water, you can use the equation:
Q = m * c * ΔT
Where:
Q = amount of energy (in calories)
m = mass of water (in grams)
c = specific heat capacity of water (1 calorie/gram °C)
ΔT = change in temperature (in °C)
In this case, you have the following values:
m = 8.5g
c = 1 calorie/gram °C
ΔT = 36°C - 15°C = 21°C
Now you can plug in these values into the equation:
Q = 8.5g * 1 cal/g °C * 21°C
Calculating the result:
Q = 178.5 calories
Therefore, the amount of energy required to heat 8.5g of water from 15°C to 36°C is 178.5 calories.
240 cal
amount of energy absorbed or released is given by
Q = mc*(T2 - T1)
where
Q = heat (in Joules)
m = mass (in grams)
c = specific heat capacity (J/g-K)
T = temperature (in Celsius or Kelvin)
*note that Q is (+) if the object absorbed heat, and (-) if it released heat.
for water, c = 4.184 J/g-K (you can find this in books or you can google this)
substituting,
Q = 8.5*4.184*(36-15)
Q = ?
now solve for Q. units in Joules.
hope this helps~ :)