How many moles of oxygen are produced by decomposing 85.5g of H2O2 according to the equation 2H2O2 --> 2H2O + O2

A sample of 48.7 g of tetraphosphorous decoxide (P₁0₁0) reacts with 84.6 g of water to produce phosphoric acid (H₂PO4) according to the following balanced equation. PAO10 + 6H₂O4 H₂PO4 Determine the limiting reactant for the reaction. H₂O OH₂PO4 OP4010 Calculate the mass of H3PO4 produced in the reaction. mass of H₂PO4: g

Consider the following reaction: 4 NH3 + 5 O2 → 4 NO + 6 H2O If 0.800 mol of O2 reacts via this reaction in excess NH3, how many mol of H2O will be produced?

For the reaction represented by the equation 2H2 + O2 → 2H2O, what is the mole ratio of H2 to H2O?

4. How many moles of oxygen are used when 2.22 moles of carbon dioxide are produced? \1_0₂ 6CO₂ + 10 H₂O 2 C3H ₂0 +

How many grams of oxygen are required to completely burn 5.90 g of C3H8 in the followingunbalanced equation? C3H8 (g) + O2 (g) → CO2 (g) +  H2O(g)

How many moles of NO can be produced by the reaction of 65.00 g of NH3 with 150.0 g of O2 according to the following balanced chemical equation? 4 NH3(g) + 5O2(g) → 4NO(g) + 6 H2O(g)

what is the mole to mole ratio between alumin um and hydrogen gas? 2 Al + 6 H2O -> 2 Al(OH)3 + 3 H2

An explosive reaction between butane and oxygen occurs as follows. 2 C4H10 (g) + 13 O2 (g) -->  8 CO2 (g) + 10 H2O (g) If 0.625 moles of butane and 3.5 moles of oxygen gas react predict the theoretical yield (in moles) of water vapor that would be produced.

2H2 + O2 -->  2 H2O How many moles of oxygen is required to produce 19.7 moles of water?