ThermochemistryHard

Question

For the allotropic change represented by the equation C(graphite) → C(diamond); ΔH = +1.9 kJ. If 6.0 g of diamond and 6.0 g of graphite is burnt completely in separate experiments, then the heat liberated will be higher by

Options

A.1.9 kJ in case of graphite.
B.1.9 kJ in case of diamond.
C.0.95 kJ in case of diamond.
D.0.95 kJ in case of graphite.

Solution

Heat liberated is greater for diamond by $\frac{1.9}{12} \times 6 = 0.95\text{ kJ}$

Create a free account to view solution

View Solution Free
Topic: Thermochemistry·Practice all Thermochemistry questions

More Thermochemistry Questions

The enthalpy of formation of ammonia gas is −46.0 kJ/mol. The enthalpy change for the reaction2NH3(g) → N2(g) + 3H2(g) i...Geological conditions are sometimes so extreme that quantities neglected in normal laboratory experiments take on an ove...The potential energy diagram for a reaction R &nbsp → P is give below ᐃHo of the reaction corresponds to the...The standard enthalpy of combustion of solid boron is numerically equal to...The standard heat of combustion of propane is −2220.1 kJ/mol. The standard heat of vaporization of liquid water is 44 kJ...