Question

Question 1 (1 point) In an exothermic gas compression, 22.1 kJ of heat and 7.6 kJ of work are exchanged between the system and its surroundings. What is the overall change in internal energy for the system? 0-14.5 kJ 29.7 kJ O-29.7 kJ 14.5 kJ Question 2 (1 point) 3 In a thermochemistry demonstration, a 1.00 L balloon at room temperature (22.1 Celsius) is placed into liquid nitrogen (-196 Celsius). If the gas inside the balloon acts ideally, its new volume will be ml. 4 Question 3 (1 point) The volume occupied by 2.47 moles of hydrogen gas at 1.02 atmospheres and 23.8 degrees Celsius is liters. 27

please answer all three questions

Answer 1

1: Given that : Heat = 22.1 kJ and work done(W) = 7.6 kJ

As the reaction is exothermic,So q = -22.1 kJ

From 1st law of thermodynamics, $\Delta$ U= q + W

where $\Delta$ U is change in internal energy, q is heat transfer and W is work done on system

Now,putting the values:

$\Delta$U = (-22.1) + 7.6 = -14.5 kJ

Thus overall change in internal energy of system is -14.5 kJ.