ThermochemistryHard

Question

For the reaction, 2NO(g) + O2(g) → 2NO2(g); ΔH = −35.0 kcal at 300 K. If 6.0 moles of NO reacts with 3.0 moles of O2 at constant pressure of 1.0 atm and temperature 300 K to form NO2, then which of the following statement(s) is/are correct?

Options

A.The magnitude of work done by the system is 1.8 kcal.
B.The amount of heat released by the reaction is 35 kcal.
C.The internal energy of system decreased by 103.2 kcal.
D.The internal energy of system decreased by 106.8 kcal.

Solution

$\Delta H = q = 3 \times ( - 35) = - 105\text{ kcal}$

$\Delta U = \Delta H - \Delta n_{g}RT $$${ = \left\lbrack ( - 35) - (2 - 3) \times \frac{2}{1000} \times 300 \right\rbrack \times 3 = - 103.2\text{ kcal} }{\text{and }w = u - q = ( - 103.2) - (105) = 1.8\text{ kcal}}$$

Create a free account to view solution

View Solution Free
Topic: Thermochemistry·Practice all Thermochemistry questions

More Thermochemistry Questions

When 1.0 g of oxalic acid is burnt in a bomb calorimeter whose heat capacity is 8.75 kJ/K, the temperature increases by ...The reaction CH4(g) + Cl2(g) → CH3Cl(g) + HCl (g) has ᐃH = - 25 kcalFrom the given, data, what is the bond e...Enthalpy of formation of HF and HCl are - 161 kJ and - 92 kJ respectively. Which of thefollowing statements is incorrect...CsF(S) → Cs+(aq) + F-(aq) ᐃH = - 40 kJ mol- If lattic energy of CsF is 750 kJ mol- . Then the summation of h...A volume of 4.0 L of a mixture of ethane and methane gases on complete combustion at 300 K produced 6.0 L of carbon diox...