The reaction between hydrogen and oxygen to yield water vapor
has ΔH∘=−484kJ:
2H2(g)+O2(g)→2H2O(g)ΔH∘=−484kJ
A) How much PV work is done in kilojoules for the reaction of 0.36 mol of H2 with 0.18 mol of O2 at atmospheric pressure if the volume change is -3.8 L ?
B) What is the value of ΔE in kilojoules.
The reaction between hydrogen and oxygen to yield water vapor has ΔH∘=−484kJ: 2H2(g)+O2(g)→2H2O(g)ΔH∘=−484kJ A) How much PV work is done in kilojoules for the reaction of 0.36 mol of H2 with 0.18 mol...
Hydrogen gas reacts with oxygen to form water. 2H2(g)+O2(g)→2H2O(g)ΔH=−483.5kJ2H2(g)+O2(g)→2H2O(g)ΔH=−483.5kJ Determine the minimum mass of hydrogen gas required to produce 233 kJkJ of heat.
Part A Consider the combustion of H2(g):2H2(g)+O2(g)→2H2O(g). If hydrogen is burning at the rate of 0.51 mol/s, what is the rate of consumption of oxygen? Part B What is the rate of formation of water vapor? Part C The reaction 2NO(g)+Cl2(g)→2NOCl(g) is carried out in a closed vessel. If the partial pressure of NO is decreasing at the rate of 56 torr/min, what is the rate of change of the total pressure of the vessel?
Consider the reaction 2H2O(g) →2H2(g) + O2(g) ΔH = +483.60 kJ/mol at a certain temperature. If the increase in volume is 27.7 L against an external pressure of 1.00 atm, calculate ΔU for this reaction. (The conversion factor is 1 L· atm = 101.3 J.) _______kJ
Consider the reaction 2H2O(g) → 2H2(g) + O2(g) ΔH = +483.60 kJ/mol at a certain temperature. If the increase in volume is 42.7 L against an external pressure of 1.00 atm, calculate ΔU for this reaction. (The conversion factor is 1 L · atm = 101.3 J.) _______kJ
Hydrogen gas reacts with oxygen to form water. 2H2(g)+O2(g)→2H2O(g)ΔH=−483.5kJ Determine the minimum mass of hydrogen gas required to produce 175 kJ of heat.
Hydrogen gas reacts with oxygen to form water. 2H2(g)+O2(g)→2H2O(g)ΔH=−483.5kJ Determine the minimum mass of hydrogen gas required to produce 446 kJ of heat.
When hydrogen peroxide (H2O2) is used in rocket fuels, it produces water, oxygen, and heat. 2H2O2(l)⟶2H2O(l)+O2(g)ΔH=−196kJ Part B: How many kilojoules are released when 3.05 moles of H2O2 reacts? Express your answer with the appropriate units. Part C: How many kilojoules are released when 277 g of O2 is produced? Express your answer with the appropriate units.
Given: 2H2 (g) + O2 (g) --> 2H2O (l) Calculate the mass of water produced if 3.50 L O2 is at 1.25 ATM at 22.0oC reacting with excess H2. 4.55 L sample of CO2 has a pressure of 1.12 ATM. If the pressure is increased to 2.50 ATM what would be the resulting volume? Assume constant temp and no change in moles of gas. B) 4.55 L of He is at 25.0oC in a balloon. If the temp is increased...
consider the following reaction 2H2(g)+O2(g)--> 2H2O (I) delta H= -572KJ A) how much heat is evolved when 1.00 mole of H2O (I) is produced? B) how much heat is evolved when 4.03g H2 are reacted with 40.0g of O2? C) the total volume of hydrogen gas needed to fill the Hindenburg was 2.0*10^8 L at 1.0 atm and 25 degree C. How much HEAT was evolved when the Hidenburg exploded, assuming all of the hydrogen reacted (plenty of oxygen)?
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?