Consider that 2.80 LL of N2N2, at 25 ∘C∘C and 1.83 atmatm , is mixed with 2.60 LL of O2O2, at 25 ∘C∘C and 0.181 atmatm , and the mixture is allowed to react. N2(g)+O2(g)→2NO(g)   How much NONO, in grams, is produced?

A cylinder in a car engine takes 4.50 x 10-2m3air into the chamber at 303.15 Kand at atmospheric pressure (1.013 x 105Pa). The piston then compresses the air to 10 % of the original volume and 20 times the original pressure(R = 8.314 J/mol K). (i). Calculate the number of moles in the air. (ii). What is the new temperature of the air?

You go climbing in the Andes, and stop to make tea. You find that the water boils at a temperature of 83.9 °C. What is the atmospheric pressure where you are? (Given: ΔH°vap(H2O) = 43.4 kJ/mol) (2 decimal places)

The gas cyclopropane, C3H6(g), can be used in welding. When cyclopropane is burned in oxygen, the reaction is: 2 C3H6(g) + 9 O₂(g)6 CO₂(g) + 6 H₂O(g) (a) Using the following data, calculate AH° for this reaction. AH kJ mol-¹: C3H6(g) = 53.3; CO₂(g) = -393.5; H₂O(g) = -241.8 4 AH° = kj (b) Calculate the total heat capacity of 6 mol of CO₂(g) and 6 mol of H₂O(g), using CcO₂(g) = 37.1 J K-1 mol-¹ and CH₂O(g) = 33.6 J K-¹ mol-¹. C = JK-1 (c) When this reaction is carried out in an open flame, almost all the heat produced in part (a) goes to raise the temperature of the products. Assuming that the reactants are at 25°C, calculate the maximum flame temperature that is attainable in an open flame burning cyclopropane in oxygen. The actual flame temperature would be lower than this because heat is lost to the surroundings. Maximum temperature °℃