To raise the temperature of 200.8 g of water from 50.00 °C to 60.00 °C requires how much heat?

q = mass H2O x specific heat H2O x (Tfinal-Tinitial)

when you are inthe bed you more likely in heat

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To find out how much heat is required to raise the temperature of water, we can use the equation:

q = mcΔT

Where:
q represents the heat energy (in Joules)
m represents the mass of water (in grams)
c represents the specific heat capacity of water (approximately 4.18 J/g°C)
ΔT represents the change in temperature (in °C)

Given:
m = 200.8 g (mass of water)
c = 4.18 J/g°C (specific heat capacity)
ΔT = 60.00 °C - 50.00 °C = 10.00 °C (change in temperature)

Substituting the given values into the equation, we can calculate the heat energy required:

q = (200.8 g) * (4.18 J/g°C) * (10.00 °C)

Calculating this expression:

q = 8376.64 J

Therefore, to raise the temperature of 200.8 g of water from 50.00 °C to 60.00 °C, 8376.64 Joules of heat energy is required.