How much energy (in Joules) is required to heat 13.48 g of water from 10.5 oC to 46.2 oC ? Use 4.184 J/goC as the specific heat capacity of water.

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

To calculate the amount of energy required to heat water, we can use the formula:

Q = m × c × ΔT

Where:
Q = energy required (in Joules)
m = mass of water (in grams)
c = specific heat capacity of water (in J/g°C)
ΔT = change in temperature (in °C)

Given:
m = 13.48 g
c = 4.184 J/g°C
ΔT = (46.2 - 10.5) °C

Let's substitute the values into the formula and calculate the energy required:

Q = 13.48 g × 4.184 J/g°C × (46.2 - 10.5) °C
Q = 13.48 g × 4.184 J/g°C × 35.7 °C

Now, we can calculate:

Q = 2052.9796 J

Therefore, the amount of energy required to heat 13.48 g of water from 10.5 °C to 46.2 °C is approximately 2053 Joules.

To calculate the amount of energy required to heat the water, we need to use the equation:

Q = mcΔT

Where:
Q is the amount of energy required (in Joules)
m is the mass of the water (in grams)
c is the specific heat capacity of water (in J/goC)
ΔT is the change in temperature (in oC)

Given values:
Mass of water (m) = 13.48 g
Specific heat capacity of water (c) = 4.184 J/goC
Change in temperature (ΔT) = 46.2 oC - 10.5 oC = 35.7 oC

Now, let's plug in the values into the formula:

Q = (13.48 g) * (4.184 J/goC) * (35.7 oC)

To find the answer, multiply the mass of water, the specific heat capacity of water, and the change in temperature:

Q = 2445.948 J

Therefore, the amount of energy required to heat 13.48 g of water from 10.5 oC to 46.2 oC is approximately 2445.948 Joules.