What is the change in enthalpy when 1.50 moles of H₂ are reacted with an excess O2 of according to the following balanced chemical reaction: -381 mol H₂ ADD FACTOR 381 g 0₂ -572 KJ 2 H₂(g) + O₂(g) -429 ΔΗ = -572 1.50 g H₂O 32.0 - kJ 1 2 H₂O(l) ANSWER mol O₂ 429 2 mol H₂O RESET J 2 18.02 2.02 g H₂

Given the thermochemical equation 2S02(9) +O2(9) 2503(g). AH pxn= -198 kJ/mol, how much heat is evolved when 600. g of SO2 is burned? Multiple Cholce 59,400 kJ O 185 - 103 kJ 5.46 - 10-2 kJ 928 kJ O 371 x 103 kJ

Consider the following thermochemical equation: 2NO (9) + O2(g) 2 NO, 2(g) AH = -114.1 kJ Choose... If 3.00 x 10 g NO, were produced, then the amount of heat released (in kJ) would -2 be: Consider the following reactions: 2W, + 30, 2 (g) 2 WO3 AH= -1939.40 (s) kJ/mol 2H, + 2 (g) 02 (g) 2H,0 "2 (g) AH= - 477.84 kJ/mol Choose... Use Hess's law to Calculate AH (in kJ/mol) for the following reaction: WO3 (6) + 3H2 (g) W. + ЗН,0 (g) What is the molar heat of combustion of methanol CH,0OH ( in kJ/mol), if the combustion of 1.0 g of methanol causes a temperature rise of 3.68 °C in a bomb calorimeter that has a heat capacity of Choose... 6.43 J/°C? The mole fraction of N, gas in the air is 0.781 at 760 torr. Calculate the partial pressure of N, in air Choose... DI f th

the first picture is the question and the second picture is the expected answer (please apply thermochemistry and their formula)

The average molecular speed in a sample of Kr gas at a certain temperature is 298 m/s. The average molecular speed in a sample of O3 gas is m/s at the same temperature.

Thermochemistry and Stoichiometry

- Use the following information for the following questions. The chemical reaction is given by the equation Mg + 2 HCl H2 + MgCl2 . The enthalpies of formation for the substances are for Mg = 0 kJ, HCl = -92.3 KJ, H2 = 0 kJ, MgCl2 = -641.8 kJ, what is the total enthalpies of formation of the products?

Calculating a Heat of Formation Using Hess’s LawAs discussed in lecture, the simplest and most general method for determining theenergy change during a chemical reaction involves the use of the heat of formation (ΔHf) for thereactants and products. Conceptually, the heat of formation is the heat released or absorbedwhen one mole of the substance is created from its elements at standard temperature andpressure. In some cases, this number can be measured directly (i.e. by reacting the elements at1.0 atm and 25oC and observing the heat given off). In most cases, however, this is notpractical. For instance, the direct calculation of the ΔHf for magnesium oxide would involveburning magnesium metal in a pure oxygen atmosphere; while such a reaction is certainlypossible, it would difficult to measure changes in temperature since the reaction is highlyexothermic and the product is a solid powder. Instead, in this lab you will be calculating the ΔHf for magnesium oxide by determiningthe heat of…

11) q of combustion of the food sample equals a) q absorbed by the calorimeter - q absorbed by the water b) q absorbed by the water - q absorbed by the calorimeter c) negative (q absorbed by the water + q absorbed by the calorimeter) d) (q absorbed by the water + q absorbed by the calorimeter) 12) Heat produced by combustion of a 3.000 g food sample was -9643J. How much heat, in Joules, was pipduced per gram? a) 3 J/g b) 4.18 J/g c) 9643 J/g d) 3214 J/g 13) Heat produced by combustion of a different food sample is 10,000 J/g. How many Calories per gram is that? (1 capital C Calorie = 4184 J). a) 2 Cal/g b) 4 Cal/g c) 9 Cal/g d) 4184 Cal/g 99+ ASUS ZenBook F10 F1 F7 F8 F9 F3 F4 F6 $4 5 7. 8. 3.

Given the thermochemical equation 2S02(g) +02(g)-2S03(g). AHpxn=-198 kJimol. how much heat is evolved when 600 g of S02 is burned Multiple Choice 3.71x 103 kJ 5.46 x 10-2 kJ 928 kJ 1.85 x 103 kJ 59,400 kJ