You have the following reaction: H2 + O2 --> H2O. You start the reaction with 10.0 grams of H2 and 10.0 grams of O2 and you experimentally produce 1.00 grams of H2O. What is theoretical and percent yield of H2O?
You have the following reaction: H2 + O2 --> H2O. You start the reaction with 10.0...
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?
11 If 50.0 g of H2 and 130.0 g of O2 react, how many moles of H2O can be produced in the reaction below? 2 H2(g) + O2(g) → 2 H2O(g) Attempts remaining: 2 12 If 41.1 g of NO and 26.9 g of Oz react together, how many grams of NO2 can be formed via the reaction below? 2 NO (g) + O2(g) → 2 NO2 (g) Attempts remaining: 2 13 - You have 2.2 mol Xe and 1.9...
At 1000 °C, for the reaction: 2 H2O(g) ↔ 2 H2(g) + O2(g) Kc = 7.32 x 10-18, what will be the [H2(g)] at equilibrium if 1.00 mol of H2O(g) are placed in a 10.0 L vessel?
Consider the following UNBALANCED equation: NO(g) +H2(g) ? NH3(g)+H2O(g) If you start with 89.3 g NO(g) and 28.6 g H2(g), find the theoretical yield of ammonia. Express your answer in grams. Enter only a numerical value, do not enter units.
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?
Ammonia can be produced from the following reaction: CaO (s) + 2NH4Cl (s) = 2NH3 (g) + H2O (l) + CaCl2 (s) If the expected percent yield were 25%, how many grams of CaO would be needed to react with excess ammonium chloride to produce 1.00g of ammonia? 1.00 g is the (theoretical or actual?) yield of ammonia. What is the theoretical yield of ammonia necessary to produce 1.00 g of ammonia?
help please Consider the reaction between HCl and O2 4 HCl + O2 ----> 2 H2O + 2 Cl2 Calculate the theoretical yield of H2O when 64 grams of HCl react with 19 grams of O2.
#12 (a) and (b) please! 12. For this reaction, if I start with 5.05 g of C3H§. a) What is my theoretical yield of water? b) I got a percent yield of 75% How many grams of water did I make? C3H8 + 5 O2 -→ 3 CO2 + 4 H2O
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)
Consider the reaction between CH3CHO(l) and O2(g) to form CO2(g) and H2O(l). If the percent yield of CO2(g) is 56.0% and 18.0 grams of CO2(g) forms, determine the theoretical yield of CO2(g) in moles.