ThermochemistryHard
Question
The most exothermic ‘ordinary’ chemical reaction for a given mass of reactants is 2H(g) → H2(g), where ΔE = 103 kcal. The theoretical decrease in mass on combination of 2.0 moles of hydrogen atoms to form 1.0 mole of hydrogen molecules, assuming that the energy is released only due to decrease in mass of the system is
Options
A.4.8 × 10–12 kg
B.4.8 × 10–12 g
C.2.4 × 10–12 kg
D.9.6 × 10–12 kg
Solution
$\Delta m = \frac{E}{C^{2}} = \frac{103 \times 10^{3} \times 4.2}{\left( 3 \times 10^{8} \right)^{2}} = 4.8 \times 10^{- 12}\text{ kg}$
Create a free account to view solution
View Solution FreeMore Thermochemistry Questions
For the following reaction, C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l)Which of the following expression is incorrect?...The Δf Ho for CO2(g), CO(g) and H2O(g) are −393.5, −110.5 and −241.8 kJ mol–1, respectively. The standard enthalpy chang...The molar enthalpy of vaporization of benzene at its boiling point (353 K) is 7.4 kcal/mol. The molar internal energy ch...As a 0.1 mole sample of solid NH4Cl was dissolved in 50 ml of water, the temperature of the solution decreased. A small ...The value of ΔfH° of U3O8(s) is –853.5 kJ mol–1. ΔH° for the reaction3UO2(s) + O2(g) → U3O8(s)is −76.00 kJ. The value of...