According to the balanced reaction below, calculate the moles of NO2 that form when 5.20 x 10.3 mol of N2O5 completely reacts 2N2O5(g) -> 4NO2(g) + O2(g)

(6)For the following balanced reaction use the mass of the chemical provided to solve the mass of the chemical asked for.  6 CO2 +  6 H2O  -->  1 C6H12O6   +   6 O2   202 g of CO2 is consumed by a plant undertaking this photosynthesis reaction.  Find the mass of C6H12O6 produced.

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)

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)

22.0 g of CO​​2 gas and 9.01 g of H​​2O gas are formed from combustion of an unknown hydrocarbon (containing only hydrogen and carbon) in the presence of O​​2 gas. The molar mass of the gas is 84.2 g/mol. What is its molecular formula?

You have 22.2 g of the compound C2Hx, where x is the maximum number of hydrogens that can fit around two carbon atoms and still create a stable Lewis dot structure. If you allow all of this sample to react with excess oxygen and then allow the products to cool to room temperature, how many moles of liquid product will you have?

How many moles of HNO₃ will be produced from the reaction of 34.5 g of NO₂ with excess water in the following chemical reaction? 3 NO₂(g) + H₂O (l) → 2 HNO₃(g) + NO(g)

How much oxygen (in grams) will form from 30.2 g of N2O5?    2N2O5(s)  →  4NO2(g) + O2(g)

How many moles of water are produced when 6.33 moles of CH4 react? CH4 (g) + 2O2 (g) --> CO2 (g) + 2H2O (g) (balanced)

According to the balanced reaction below, calculate the moles of NO₂ that form when 5.20 × 10⁻³mol of N₂O₅ completely reacts: 2N₂O₅(g)→4NO₂(g)+O₂(g)