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QUESTION 3 Hydrogen and oxygen gas can react to form liquid water according to the following...
QUESTION 3 Hydrogen and oxygen gas can react to form liquid water according to the following heterogeneous equilibrium: 2H2(g) + O2(g) + 2H2O(1) What is the correct equilibrium constant expression for this equation? OK - [H2]*[02] OK - [H20] Kc [H20] [H2]*[02] [H2] [02] Окс [HIO.]
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]
20 1 point Hydrogen and oxygen gas react explosively to product water vapor. How many grams of water are made from the reaction of 39.6 grams of hydrogen gas and an excess of oxygen? Reaction: 2H2(g) + O2(g) - 2H2O(g) Type your answer Previous Next
Hydrogen chloride and oxygen react to form chlorine and water, like this: 4HCl(g)+O2(g)→2Cl2(g)+2H2O(g) Also, a chemist finds that at a certain temperature the equilibrium mixture of hydrogen chloride, oxygen, chlorine, and water has the following composition: Calculate the value of the equilibrium constant Kp for this reaction. Round your answer to 2 significant digits. compound pressure at equilibrium НСІ 28.9 atm 02 96.7 atm Cl2 32.1 atm H20 13.1 atm
Hydrogen gas, H2, and oxygen gas, O2, can be reacted to form liquid water. If 2.00 g hydrogen gas and 17.20 g oxygen gas are reacted in a 1.500 L flask at 25.0 °C, calculate the total gas pressure (atm) in the flask at 25 °C. The vapor pressure of water is 23.8 mm Hg. Stoichiometry is involved in this question. Total gas pressure:
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.
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=−483.5kJ2H2(g)+O2(g)→2H2O(g)ΔH=−483.5kJ Determine the minimum mass of hydrogen gas required to produce 233 kJkJ of heat.
Question 2 (0.5 marks) Hydrogen gas. H. and oxygen gas, O2, can be reacted to form liquid water. If 2.00 g hydrogen Ras and 17.20 g oxygen gas are reacted in a 1.500 L flask at 25.0 °C, calculate the total gas pressure (atm) in the flask at 25°C. The vapor pressure of water is 23.8 mm Hg. Stoichiometry is involved in this question. Total gas pressure:
QUESTION 4 Consider the reaction between hydrogen gas and oxygen gas to form water 2 H2(g) + O2(9) - 2 H20(9) How many grams of water could be produced by the reaction of 7.01 liters of hydrogen with 4.11 liters of oxygen at STP? (Hint: check for limiting reagent).