Use the periodic table to answer the following question When 2.16 g of H2 reacts with...
Use the periodic table to answer the following question: If 1.48 g of Cl2 reacts with excess P, what is the total change in enthalpy in kilojoules? 2P+5Cl2→2PCl5 ΔH=−886kJ Round your answer to two decimals places. Include a negative sign if appropriate.
When H2(g) reacts with O2(g) according to the following reaction, 242 kJ of energy are evolved for each mole of H2(g) that reacts. Complete the following thermochemical equation. 2H2(g) + O2(g)— 2H2O(g) AH- The following information is given for bismuth at latm: T = 1627.00°C T. = 271.00°C Specific heat solid = 0.1260 J/g °C Specific heat liquid = 0.1510 J/g °C AHvap (1627.00°C) = 822.9 J/g AH (271.00°C) = 52.60 Jig A 38.40 g sample of liquid bismuth at...
? Review Constants Periodic Table Value Units The chemical reaction of hydrogen with oxygen produces water 2H2 (9)O2(9) 2H20(9) Request Answer Submit Part C How many moles of H2O form when 3.5 moles of O2 reacts? Express your answer to two significant figures and include the appropriate units. HA ? Value Units Request Answer Submit
Using standard heats of formation, calculate the standard enthalpy change for the following reaction. H2(g) + Cl2(g)—>2HCI(g) ANSWER: kJ Using standard heats of formation, calculate the standard enthalpy change for the following reaction. 2H20(1)——2H2(g) + O2(g) ANSWER: kJ
When 9.0 g of hydrogen gas, H2, reacts with oxygen gas, O2, 73.0 g of water is produced. a) What is the theoretical yield of water? b) What is the percentage yield?
Calculate the work (in kJ) done on the system when 2.80 moles of hydrogen gas are produced from the reaction of sodium in excess water at 298 K: 2Na(s) 2H2O()2NaOH(aq) + H2(g) Answer: 2.62 Calculate the work (in kJ) when 1.40 moles of methane react with excess oxygen at 463 K: CH4(g) 202(g) CO2(g) 2H20 (1) Answer: 13.1 1.927 g of an unknown hydrocarbon (129.1 g/mol) burns in bomb calorimeter in excess oxygen. The heat capacity of the calorimeter,Cv, =...
What happened to the Hindenberg? Nobody seems to know. Was it a spark? Sabotage? Lightening? Either way it did burn, a lot. We do know it was filled with hydrogen gas. The Zeppelin was filled with 2.0 x 108 L of H2. Show all work for the below. a) Calculate the enthalpy of the reaction(kJ/mol) below using the heat of formation for the reactants and products from appendix C from your text book. 2H2(g) + O2(g) à 2H2O(l) DHorxn= ?...
1) C2H6 (g) -----> C2H4 (g) + H2 (g) ΔH1 = ? 2) C2H6 (g) + 3.5O2 (g) -----> 2CO2 (g) + 3H2O (l) ΔH2 = -1560 kJ/mo 3) C2H4 (g) + 3O2 (g) -----> 2CO2 (g) + 2H2O (l) ΔH3 = -1411 kJ/mol 4) 2H2O (l) -----> 2H2 (g) + O2 (g) ΔH4 = 571.6 kJ/mol How much heat is transferred between the system and the surroundings when 25 grams of ethane (C2H6) decomposes to produce ethylene (C2H4) and...
Hydrogen is burned according to the following chemical reaction: 2H2(g) + O2(g) → 2H2O(l) ∆Hrxn = -286 kJ Given 100 g of H2 and excess O2, how much heat is released?
When 20.00 moles of H2(g) reacts with 10.00 mol of O2(g) to form 20.00 mol of H2O(l) at 25°C and a constant pressure of 1.00 atm. If 1366 kJ of heat are released during this reaction, and PΔV is equal to -74.00 kJ, then ΔH° = -1366 kJ and ΔE° = -1292 kJ.ΔH° = +1366 kJ and ΔE° = +1440 kJ.ΔH° = -1366 kJ and ΔE° = -1440 kJ.ΔH° = +1366 kJ and ΔE° = +1292 kJ.