If 1.97g of H2 reacts with 2.77g of O2 according to the balanced reaction below, calculate the theoretical yield of H2O. 2H2(g) + O2(g) ⟶ 2H2O(g)
If 1.97g of H2 reacts with 2.77g of O2 according to the balanced reaction below, calculate...
13. Consider 28 g O2 mixed with 4.8 g H2 according to this reaction: H2 + O2 = H2O a.) Balance the reaction? b.) Find the limiting reactant? c.) What is the theoretical yield (in grams)? d.) What is the percent yield if 3.4 g H2O are obtained?
When 5.58g H2 react by the following balanced equation, 32.8 g H2O are formed. What is the percent yield of the reaction? 2H2(g)+O2(g)?2H2O(g) Select the correct answer below: 17.0 % 65.7 % 11.7 % 38.9 %
The equation H2+O2 arrow to the right H2O be balanced by changing it to: A. H2+O2 arrow to the right H2O2 B. 2H2+O2 arrow to the right 2H2O C. Nothing needs to be done; it is already balanced D. H2+2O2 arrow to the right 4H2O
According to the balanced reaction below, calculate the moles of NH3 that form when 4.2 mol of N2H4 completely reacts 3 N2H4(1) ► 4 NH3(g) + N2(g) Attempts remaining: 2 According to the balanced reaction below, calculate the moles of NO2 that form when 5.20 x 10-3 mol of N205 completely reacts: 2 N2O5(g) → 4 NO2(g) + O2(g) Attempts remaining: 2 How many moles of H2SO4 are required to completely react with 7.20 mol of Al according to the...
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?
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= ?
When 10.58 g H2 react by the following balanced equation, 32.8 g H2O are formed. What is the percent yield of the reaction? 2 H2(g) + O2(g) → 2H2O(l) Select the correct answer below: 32.2% 34.7% 65.3% 38.9%
Consider the reaction 2H2(g)+O2(g)→2H2O(l) What is the mass of water, H2O(l), produced when 5.20 g of O2(g) reacts with excess H2(g)? PLEASE HELP
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...
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?