2H2(g)+O2(g)     2H2O(1) 8.0 moles of H2 and 6.0 moles of O2 are combined. What is the limiting reactant in the above reaction?

According to the balanced reaction below, calculate the quantity of moles of NH, gas that form when 4.20 mol of N,H, liquid completely reacts: 3 N,H,(1) → 4 NH,(g) + N,(g)

The rocket boosters of the space shuttle Discovery, launched on July 26, 2005, used a fuel mixture containing primarily solid ammonium perchlorate, NH4ClO4, and aluminum metal. The unbalanced chemical equation for the reaction is given below. (Hint: Balance the elements in the order Cl, H, O, Al, N.) Al(s) + NH4CIO4(s) Al₂O3(s) + AlCl3(s) + H₂O(l) + N₂(g) What is the mass (in kilograms) of NH4ClO4 consumed per kilogram of Al, assuming a percent yield of 87.20%? (Answer with two decimal places.)

Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce ammonia. N₂ (g) + 3 H₂(g) → 2NH₂(g) Initially, there are 0.100 mol N₂ and 0.330 mol H₂ present. How many moles of ammonia are produced after the reaction has gone to completion? moles of NH3: What is the limiting reactant? O hydrogen nitrogen How many moles of H₂ remain after the reaction has gone to completion? moles of H₂: mol mol

Glucose, C6H1206, can be represented by the molecular model shown below. If 1.00 mol of glucoseis submitted to combustion analysis, how many moles of CO2 and how many moles of H2O wouldbe formed?

Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is:2Mg(s)+O2(g)→2MgO(s)2Mg(s)+O2(g)→2MgO(s) When 10.1 gg of Mg are allowed to react with 10.5 g of O2, 13.4 gg of MgO are collected. Determine the limiting reactant for the reaction. Express your answer as a chemical formula.

If you can answer at least any of these then please do so. If you can answer all that would be best but if you can't then please answer a couple. Thanks. When 13.0 g of H2 is mixed with 10.0 g of N2, and form ammonia (NH3), what is the limiting reactant? In the following reaction, which may or may not be balanced: C3H8 + O2 = CO2 + H2O, if 100.0 g of C3H8 react and form 32.3 g of CO2, what is the percent yield? When 47.9 g of sodium carbonate is reacted with silver (I) nitrate, the products are sodium nitrate and 26.0 g of silver (I) carbonate. What is the percent yield? In the following balanced chemical equation: N2 + 3H2 = 2 NH3, if 30.0 g of N2 and 10.0g of H2 react, forming 2.1g of NH3, what is the percent yield? In the following balanced chemical reaction: CaCl2 + 2AgNO3 = 2AgCl + Ca(NO3)2, if 45.0g of CaCl2 is mixed with 95.0g of AgNO3, what is the theoretical yield of AgCl?  If 50.0g of lithium phosphate is mixed with 50.0g of iron (II) nitrate, the products are lithium…

Phosphoric acid, a mild acid used among other things as a rust inhibitor, food additive, and etching agent for cavity repair by dentists, can be made from elemental phosphorus in a two step process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: P4(s) + 50₂(g) 2 P₂O5 (g) In the second step, diphosphorus pentoxide and water react to form phosphoric acid (H₂PO4): P₂O₂(g) + 3H₂O(1) 2 H3PO4 (1) Suppose the yield of the first step is 94.% and the yield of the second step is 69.%. Calculate the mass of phosphorus required to make 8.0 kg of phosphoric acid. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.

In the atmosphere, nitrogen dioxide reacts with water to produce NO and nitric acid: NO2 (g) + H2O (I) → HNO3 (aq) + NO (g) Balance the equation How many grams of HNO3are produced for every 1 mol of NO2that reacts?

4. The reaction for the combustion of propene is:2 C3H6 + 9O2 6 CO2 + 6 H2O(a) If 15.0 g of C3H6 and 15.0 g of O2 are reacted, how many moles of H2O can be produced?(b) If 12.0 g of C3H6 and 25.0 g of O2 are reacted, how many moles of H2O can be produced?(c) If 5.0 mol of C3H6 and 15.0 mol of O2 are reacted to completion (until one reactant is completely used up), how many moles of CO2 can be produced? Which reactant is left over when the reaction has gone to completionin a closed container?