Question

Using the average bond energy values on the CH122 Equation Sheet, estimate the energy required (in kJ) to break all of the bonds in one mol of CH4 Question 17 4 pts A 36.2 g object has a heat capacity of 12.5 J/ °C. How much energy (in J) is required to raise the temperature by 2.03 °C?

Answer 1

Ans 16:

In CH₄, we have four C-H bonds.

Each C-H bond energy is +415.5 kJ per mole of bonds (data from the standard book), which means that we need to give +415.5 kJ to break one C-H bond.

So, to break 4 C-H bonds we need 4 * 415.5 kJ i.e 1662kJ per mole to break all four bonds C-H bonds present in the methane molecule.

Ans 17:

According to laws of thermodynamics we know:

Q = C ΔT.

Where Q = heat required to raise the temperature by 2.03^oC

C = heat capacity

ΔT. = temperature change

Q = 12.5 J/^oC * 2.03^oC

= 25.375 J

hope this helps!