Mass of hydrogen reacted = 6.06 gm
Moles of Hydrogen gas = 6.06 g / 2.016 g/mol = 3.0059 Moles
Mass of oxygen reacted = 40 gm
Moles of oxygen gas = 40 g / 32 g/mol = 1.25 Moles
Limtiing reagent is oxygen
Moles of oxygen reacted = 1.25 moles
According to the balanced equation, one mole of oxygen will release 572 kJ of energy
Amount of heat released by 1.25 mol of O2 = 1.25 mol x -572 kJ/mol = -715 kJ
Siince energy is released from the reaction, we need to add the negative reaction
Hence the correct answer is option C) -715
The combination reaction between hydrogen gas and oxygen gas proceeds according to the following balanced thermochemical...
The following thermochemical equation is for the reaction of hydrogen(g) with oxygen(g) to form H2O(g). 2H2(g) + O2(g) 2H2O(g) AH=-484 kJ How many grams of H2(g) would have to react to produce 61.5 kJ of energy? grams
QUESTION 3 Hydrogen and oxygen gas can react to form liquid water according to the following heterogeneous equilibrium: 2H2(g) + O2(g) + 2H200) What is the correct equilibrium constant expression for this equation? ok [H₂0] [H2][02] [H, 105] [H2]*[02] lo kc = [H2]”[02] o Kc = [H20]
The following thermochemical equation is for the reaction of hydrogen(g) with oxygen(g) to form water(g). 2H2(g) + O2(g)--2H2O(g) ΔΗ--484 kJ How many grams of H2(B) would have to react to produce 95.6 kJ of energy? grams Submit Answer Retry Entire Group 7 more group attempts remaining
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all 3. Calculate the heat released (kJ) in the reaction of 1.35L of acetylene (C2H2) and 0.235L of hydrogen gas at STP to form ethane gas as determined by the following equation: C2H2(g) + 2H2() → C2H6(g) Given: 2C2H2(g) +502(g) + 4CO2(g) + 2H20(g) 2C2H.(g) + 702(g) → 4CO2(g) + 6H20(g) 2H2(g) + O2(g) → 2H2O(g) AH = -2320 kJ/mol AH = -3040 kJ/mol AH = -572 kJ/mol
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.
The reaction of hydrogen sulfide(g) with oxygen(g) to form water(g) and sulfur dioxide(g) proceeds as follows: 2H2S(g) + 302(g) 2H2O(g) + 2802(g) When 12.9 grams of H2S(g) react with sufficient O2(g), 197 kJ of energy are evolved. What is the value of AH for the chemical equation given? kJ
Which of the following statements is false concerning the reaction of hydrogen gas and oxygen gas given below? H2(g)+1/2O2(g)>H2O Which of the following statements is false concerning the reaction of hydrogen gas and oxygen gas given below? H2(g) +029) - H20(1; AH = -285.8 kJ Select one: a. For the reaction H2(g) + O2(g) - H2O(g), AH is not equal to -285 b. If the equation is reversed, AH becomes +285.8 kJ. If the equation is multiplied by 2, AH...
The following thermochemical equation is for the reaction of hydrogen sulfide(g) with oxygen(g) to form water(g) and sulfur dioxide(g). 2H2S(g) + 3O2(g)2H2O(g) + 2SO2(g) H = -1.04×103 kJ When 13.5 grams of hydrogen sulfide(g) react with excess oxygen(g), kJ of energy are .