Calculate the work, w, gained or lost by the system when a gas expands from 15 L to 45 L against a constant external pressure of 1.5 atm. 1 L atm = 101 J 0-6.8 kJ +4.5 kJ +6.8 kJ -4.5 kJ A 4.50-g sample of liquid water at 25.0 C is heated by the addition of 112 J of energy. The final temperature of the water is degree C. The specific heat capacity of liquid water is 4.18 J/gK. 25.2 129 -19.0 5.95 31.0 A 50.0-g sample of liquid water at 25.0 degree C is mixed with 35.0 g of water at 79.0 degree C. The final temperature of the water is degree C. 27.4 161 0269 52.0 47.2 What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 ml of solution having a density of 1.25 g/ml by 7.80 degree C? (The specific heat of the solution is 3.74 joules/gramK.) 6.51 kJ 8.20 kJ -7.43 kJ -12.51 kJ -9.12 kJ For a particular process that is carried out at constant pressure, q = 135 kJ and w = - 25 kJ. Delta E = 135 kJ and Delta H = 110 kJ Delta E = 110 kJ and Delta H = 135 kJ. Delta E = 160 kJ and Delta H = 135 kJ. Delta E = 135 kJ and Delta H = 160 kJ. Therefore, How much heat is absorbed/released when 35.00 g of NH3(g) reacts in the presence of excess O2(g) to produce NO(g) and H2O(1) according to the following chemical equation? 4 NH3(g) + 5 O2(g) righatarrow 4 NO(g) + 6 H2O(l) Delta H degree = 1168 kJ 600.1 kJ of heat are released. 600.1 kJ of heat are absorbed. 2400 kJ of heat are released. 2400 kJ of heat are absorbed.
Show transcribed image textCalculate the work, w, gained or lost by the system when a gas expands from 15 L to 45 L against a constant external pressure of 1.5 atm. 1 L atm = 101 J 0-6.8 kJ +4.5 kJ +6.8 kJ -4.5 kJ A 4.50-g sample of liquid water at 25.0 C is heated by the addition of 112 J of energy. The final temperature of the water is degree C. The specific heat capacity of liquid water is 4.18 J/gK. 25.2 129 -19.0 5.95 31.0 A 50.0-g sample of liquid water at 25.0 degree C is mixed with 35.0 g of water at 79.0 degree C. The final temperature of the water is degree C. 27.4 161 0269 52.0 47.2 What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 ml of solution having a density of 1.25 g/ml by 7.80 degree C? (The specific heat of the solution is 3.74 joules/gramK.) 6.51 kJ 8.20 kJ -7.43 kJ -12.51 kJ -9.12 kJ For a particular process that is carried out at constant pressure, q = 135 kJ and w = - 25 kJ. Delta E = 135 kJ and Delta H = 110 kJ Delta E = 110 kJ and Delta H = 135 kJ. Delta E = 160 kJ and Delta H = 135 kJ. Delta E = 135 kJ and Delta H = 160 kJ. Therefore, How much heat is absorbed/released when 35.00 g of NH3(g) reacts in the presence of excess O2(g) to produce NO(g) and H2O(1) according to the following chemical equation? 4 NH3(g) + 5 O2(g) righatarrow 4 NO(g) + 6 H2O(l) Delta H degree = 1168 kJ 600.1 kJ of heat are released. 600.1 kJ of heat are absorbed. 2400 kJ of heat are released. 2400 kJ of heat are absorbed.