Nitromethane, CH3N02, can be used as a fuel. When the liquid is burned, the (unbalanced) reaction is mainly CH3NO2(l) + O2 (g) → CO2 (g) +N2 (g) + H2O(g) a.The standard enthalpy charuge of reaction (ΔH°van ) for the balanced reaction (with lowest whole·number coefficients) is -1288.5kJ. Calculate ΔH°f for nitromethane.b. A 15.0·L flask containing a sample of nitromethane is filled with O2 and the flask is heated to 100.0°C.At thistemperature, and after the reaction is complete, the total pressure of all the gases inside the flask is 950.torr. Ifthe mone fraction of nitrogen (Znitrogen) is 0.134 after the reaction is complete, what mass of nitrogen was produced?

5. Reaction Enthalpy. balance and calculate AHxn for the following chemical equations. AH (kJ/mol): HCN= 130.5, Ca3(PO4)2=-4120.8, H3PO4--1288, SiCl4=-640.1, SiO2= -910.9, Mg0=-601.6, HCl--167.16 a)NH₂(g) + O₂(g) + CH CH4(g) b)Ca₂(PO4)2(6) +H₂SO4(1) c)SICI(1) + H₂0 (1) d) MgO(s)+ H₂ H₂O(g) SIO₂ (s) + HCN HCN(g) + Caso (s) + H₂PO.(1) Mg(OH)2(s) H₂O(g) HCl(aq)

Consider the following reaction. CH3OH(g)  CO(g) + 2 H2(g)    H = +90.7 kJ (a) Is the reaction exothermic or endothermic? endothermicexothermic     (b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H =   kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced?  g(d) How many kilojoules of heat are released when 13.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H =  kJ(e) Calculate E when 360.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K   kJ HopHelpCh5N1

Consider the following reaction. CH3OH(g)  CO(g) + 2 H2(g)    H = +90.7 kJ (a) Is the reaction exothermic or endothermic? endothermicexothermic     (b) Calculate the amount of heat transferred when 40.0 g of CH3OH(g) are decomposed by this reaction at constant pressure.H =   kJ(c) If the enthalpy change is 11.0 kJ, how many grams of hydrogen gas are produced?  g(d) How many kilojoules of heat are released when 13.5 g of CO(g) reacts completely with H2(g) to form CH3OH(g) at constant pressure?H =  kJ(e) Calculate E when 360.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K   kJ HopHelpCh5N1

Use Hess’s law to calculate the enthalpy change for the reaction WO3(s) + 3H2(g) —> W(s) +3H2O(g) from the following data: 2W(s) + 3O2(g) —> 2 WO3(s) H=-1685.4 2H2(g) + O2(g) —> 2H2O(g) H=-477.84

Given the following reactions: N2 (g) + O2 (g) → 2NO (g) AH = +180.7 kJ 2N20 (g) → O2 (g) + 2N2 (g) AH = -163.2 kJ the enthalpy of reaction for 2N20 (g) → 2NOo (g) + N2 (g) is kJ. -343.9 343.9 -145.7 145.7 O 17.5

Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g), by the reaction 2 SO2(g) + O2(g) → 2 SO3(g) The standard enthalpies of formation for SO2(g) and SO3(g) are AH; [SO2(g)] = -296.8 kJ/mol AH; [SO3(g)] = -395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 2.25 L of SO2(g) is converted to 2.25 L gas behavior. of SO3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C. Assume ideal AH= kJ

MN.19.

uestion 27 "A new element (Rr) has been synthesized and its properties analyzed. When 0.157g of RrO (s) is added to 125g of water at 22.2° C in a coffee cup calorimeter, the following reaction occurs. RrO(s) + H 20(1) – Rr(OH) 2 (aq) AH = -83.1k/mol Given the molar mass for RrO is 74g/mol calculate the following moles of Rro round answer to 4 decimal places omit trailing zeroes 9 rxn in joules round answer to the nearest whole number 9 water in joules round answer to the nearest whole number Final temperature round answer to 1 decimal place omit trailing zeroes " A Moving to another question will save this response.

Gasoline is composed primarily of hydrocarbons, includingmany with eight carbon atoms, called octanes. One ofthe cleanest–burning octanes is a compound called 2,3,4-trimethylpentane, which has the following structural formula: The complete combustion of one mole of this compoundto CO21g2 and H2O1g2 leads to ΔH° = -5064.9 kJ.(a) Write a balanced equation for the combustion of1 mol of C8H181l2. (b) By using the information inthis problem and data in Table 5.3, calculate ΔHf° for2,3,4-trimethylpentane.