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?
Part A Consider the combustion of H2(g):2H2(g)+O2(g)→2H2O(g). If hydrogen is burning at the rate of 0.51...
The reaction 2NO(g)+Cl2(g)→2NOCl(g)2NO(g)+Cl2(g)→2NOCl(g) is carried out in a closed vessel. If the partial pressure of NONO is decreasing at the rate of 60 torr/mintorr/min , what is the rate of change of the total pressure of the vessel?
(a) Consider the combustion of ether, given below: 1 C4H10O(g) + 6 O2(g) 4 CO2(g) + 5 H2O(g) If C4H10O(g) is decreasing at the rate of 0.500 mol/s, what are the rates of change of O2(g), CO2(g), and H2O(g)? O2(g)/t = mol/s CO2(g)/t = mol/s H2O(g)/t = mol/s (b) The decomposition reaction given below: 3 NO(g) 1 N2O(g) + 1 NO2(g) is carried out in a closed reaction vessel. If the partial pressure of NO(g) is decreasing at the rate...
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 elementary reaction 2H2O(g)−⇀↽−2H2(g)+O2(g)2H2O(g)↽−−⇀2H2(g)+O2(g) proceeds at a certain temperature until the partial pressures of H2O,H2O, H2,H2, and O2O2 reach 0.0200 atm,0.0200 atm, 0.00550 atm,0.00550 atm, and 0.00700 atm,0.00700 atm, respectively. What is the value of the equilibrium constant at this temperature? kp= ?
For the reaction 2H2O(g)−⇀↽−2H2(g)+O2(g)2H2O(g)↽−−⇀2H2(g)+O2(g) the equilibrium concentrations were found to be [H2O]=0.250 M,[H2O]=0.250 M, [H2]=0.490 M,[H2]=0.490 M, and [O2]=0.750 M.[O2]=0.750 M. What is the equilibrium constant for this reaction?
Consider the reaction: 2H2O (l) ----> 2h2 (g) + O2 (g) What mass of H2O (MW=18.02) is required to form 1.4 L of O2 at a temperature of 30.0 degrees C and a pressure of 750 torr?
The rate law for the reaction 2H2(g) + 2NO(g) ----> N2(g) + 2H2O(g) is rate=k[H2][NO]2. What is the rate constant at 800 degrees C when [NO] = 0.050 M and [H2] = 0.010 M and the rate of the reaction is 1.5 M/s
Consider the following balanced equation: 2H2 + O2 --------> 2H2O If you start with 8.133 g of H2 and 3.425 g of O2, find the following: a) With excess O2, what mass (grams) of H2O would be produced by the H2? b) With excess H2, what mass (grams) of H2O would be produced by the O2? c) What is the chemical formula for the limiting reactant?
For the reaction 2H2O(g)−⇀↽−2H2(g)+O2(g) the equilibrium concentrations were found to be [H2O]=0.250 M, [H2]=0.340 M, and [O2]=0.750 M. What is the equilibrium constant for this reaction?
The elementary reaction 2H2O(g)−⇀↽−2H2(g)+O2(g) proceeds at a certain temperature until the partial pressures of H2O, H2, and O2 reach 0.0750 atm, 0.00850 atm, and 0.00650 atm, respectively. What is the value of the equilibrium constant at this temperature?