Calculate the change in temperature that occurs when 3.50 x 10^-2kg of copper heated by 635 J of energy. Ccu = 0.385 j/gxC

The change in T° is 47.1 °C

Explanation:

Calorimetry formula to solve this:

Q = m . C . ΔT

We replace the data gien:

635 J = 3.50×10⁻² kg . 0.385 J/g°C . ΔT

In units of C, we have g and the mass (m) is in kg. So let's convert it from kg to g → 3.50×10⁻² kg . 1000 g / 1kg = 35 g. Now we can determine the ΔT:

635 J = 35 g . 0.385 J/g°C . ΔT

635 J / 35 g . 0.385 J/g°C = ΔT

47.1°C = ΔT

The change in temperature is 47.12 °C

Explanation:

Step 1: Data given

Mass of copper = 3.50 * 10^-2 kg = 35 grams

Energy = 635 J

Specific heat of copper = 0.385 J/g°C

Step 2: Calculate change in temperature

Q = m*c*ΔT

⇒ Q = the energy required = 635 J

⇒ m = the mass of copper = 35 grams

⇒ c = the specific heat of copper= 0.385 J/g°C

⇒ ΔT = Change in temperature = TO BE DETERMINED

635 J = 35g * 0.385 J/g°C * ΔT

ΔT = 635 / (35*0.385)

ΔT = 47.12 °C

The change in temperature is 47.12 °C

50.23 i believe is correct but don't quote me on that.