If 7.50 mol of NH₃ and 7.60 mol of O₂ react in the following reaction, how many moles of H₂O will be formed? 4 NH₃ (g) + 5 O₂ (g) → 4 NO (g) + 6 H₂O (g

Benzene (C6H6) burns in air according to the following equation shown below. How many moles of O2 are required to react with 0.10 mol of C6H6  2 C6H6(l) + 15 O2(g)→12 CO2(g) + 6 H2O(g)

How many grams of Ab O3 will be created from reacting 36.0 g of Al with a sufficient amount of O2? 4Al(s) + 302(g) → 2Al¿Os(s)

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?

If 7.50 mol of NH₃ and 8.85 mol of O₂ react in the following reaction, how many moles of H₂O will be formed? 4 NH₃ (g) + 5 O₂ (g) → 4 NO (g) + 6 H₂O (g)

Determine the grams of H₂O produced when 0.485 grams of O₂ reacts with H₂ according to the following 2 reaction: 2 H₂(g) + O₂(g) → 2 H₂O(l)

Ammonium nitrate has been used as a high explosive because it is unstable and decomposes into several gaseous substances. The rapid expansion of the gaseous substances produces the explosive force. NH,NO3 (8) → N2 (g)+ O2 (g) + H2O(g) Calculate the mass of each product gas if 47.4 g of ammonium nitrate reacts. g N2 g O2 g H2O

According to the balanced reaction below, calculate the quantity of moles of NH3 gas that form when 4.20 mol of N2H. liquid completely reacts: 3 N2H4(1) → 4 NH3(g) + N2(g) X STARTING AMOUNT

3. How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol. 4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)