Calculate the standard enthalpy of formation, AHf, of liquid N2H4. ΔΗ. combNH3 ΔΗe = -71.5 kJ/mol NH3 %3D AH NH, = -46.0 kJ/mol AHi,0 = -285.8 kJ/mol 2NH3(g) + O2(g) → N2H4(1) + H2O(1) AH; = [ ? ] kJ/mol %3D 'f H20 -> %3D Enter either a + or - sign and the magnitude. Hint: How many moles NH3 are reacting vs the AH units? AHF° (kJ/mol) Enter
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- A quantity of 1.00 x 102 mL of 0.500 M HCl was mixed with 1.00 x 102 mL of 0.500 M NaOHin a constant pressure calorimeter of negligible heat capacity. The initial temperature of the HCLand NaOH solutions was same, 22.50 0C, and the final temperature of the mixed solution was25.86 0C. Calculate the (a) heat of the reaction at constant pressure (qp) and (b) the change inenthalpy for the neutralization reaction (ΔHrxn) in kJ per mole of HCl. Assume that the densitiesand specific heat of the solutions are the same as for water (1.00 g/mL and4.184 J/g.0C, respectively).NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)A student was asked to determine the enthalpy of solution of KclO3 in water using Styrofoam calorimetry. Calibration was performed by mixing 8.00 mL 0.050 M HCI with 2.00 mL 0.200 M NaOH. The neutralization reaction (AH = -55.85 kJ/mol) was accompanied by a temperature change from 25.0 to 28.3°C. Using the same calorimeter, 0.300 g KCIO3 (MW: 122.55) was dissolved in water and the temperature was observed to change from 23.6 to 17.3°C. (Assume that the total volume of the mixture in calibration is the same in the enthalpy measurement) What is the calorimeter constant in kJ/°C? What is the enthalpy of dissolution of KCIO3 in kJ/mol?The same student wanted to determine the heat of dissolution for potassium chlorate (KClO3, MW: 122.55 g/mol) in water. He measured 10 grams of KClO3 and dissolved it in a calorimeter containing 250 g of water. The temperature drop was 3.5 K. What is qH2O? What is qrxn? What is ΔHrxn?
- a) What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by 0.68 oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) Show your working below:calculate the standard enthalpy for the reaction 2no2 -> n2o4 at 65 degree celcuidA piece of magnesium metal with a mass of 10.5 g was placed into 200 mL of a dilute hydrochloric acid solution. The balanced equation is given below: Mg(s) + 2HCI(aq) -> MgCl2(aq) + H2(g) If magnesium is the limiting reagent in this reaction what is the work done by the expansion of H2(g)? Assume the pressure and temperature are 1.05 bar and 22.4 °C throughout the expansion. Use the value 8.314 x 10-2 L Bar K-1 mol-1 as gas constant.
- The difference between heats of reaction at constant pressure and constant volume for the reaction:2C6H6(l) + 15O2(g) = 12CO2(g) + 6H2O(l) at 298K in kJ isA. -7.43 kJB. 3.72 kJC. -3.72 kJD. 7.43 kJa) What is the standard enthalpy of reaction per mole of either HCl or NaOH when 50.00 cm3 of 0.1 moldm-3 of hydrochloric acid (HCl) and 50.00 cm3 of 0.1 moldm-3 of sodium hydroxide (NaOH) are mixed? According to your simulation, the temperature rose by 0.68 oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1) b) What is the standard enthalpy of reaction per mole of KOH when 50.00 cm3 of 1.0 moldm-3 of Nitric Acid (HNO3) and 50.00 cm3 of 1.0 moldm-3 of Potassium Hydroxide (KOH) are mixed? According to your simulation, the temperature rose by __6.81__ oC. (Density of water = 1gcm-3, Specific heat capacity of water = 4.18 J g-1 oC-1)The same student wanted to determine the heat of dissolution for potassium chlorate (KClO3, MW: 122.55 g/mol) in water. He measured 10 grams of KClO3 and dissolved it in a calorimeter containing 250 g of water. The temperature drop was 3.5 K. What is qrxn?
- The same student wanted to determine the heat of dissolution for potassium chlorate (KClO3, MW: 122.55 g/mol) in water. He measured 10 grams of KClO3 and dissolved it in a calorimeter containing 250 g of water. The temperature drop was 3.5 K. What is qH2O in Joules? What is qdissolution in Joules? What is the ΔHdissolution in kilojoules per mole? What is the ΔHdissolution in kilojoules per mole?19. Solid urea, (NH2)2CO, burns to give CO2, N2, and liquid H2O. Its heat of combustion is -632.2 kJ/mol. 1.Write the balanced combustion equation. Record fractions as ratios (e.g. 1/2) if needed. Include aggregation states in your answer. 2.Calculate the heat generated per mole of H2O formed to 0.1 kJ. 3.Using this heat of combustion and the appropriate thermodynamic data, determine the heat of formation of urea to 0.1 kJ.A student poured 100 ml of water (density = 1.00 g / mL) into a coffee calorimeter, noted that the temperature of the water was 18.8oC, then added 5.33 g KOH. With the lid on, the mixture was stirred, temperature increased and the maximum temperature reached at the time of mixing 31.6 oC. Calculate the heat of the system in this dissolution reaction (qsys). ( Approximate the specific heat capacity, cp as 4.18 J g-1 K-1. Do not consider the contribution to the heat generated from the calorimeter; assume that this is zero. Only calculate the heat from the heat capacity of the solution. make sure you consider the sign of qsys qsys for dissolution of KOH = J