What is the mass in grams of H2 that can be formed from 44.8 grams of NH3 in the following reaction? 2 NH3 (g) →3 H2(g) + N2(g)

What is the mass in grams of phosphorus trichloride that can be formed from 232.6 grams of chlorine gas based on the balanced chemical equation?  balanced chemical equation: P4(s) + 6 Cl2(g)-> 4PCl2(g)

What is the mass in grams of NO that will be produced from 33.5 g of NO₂ reacted with excess water in the following chemical reaction? 3 NO₂(g) + H₂O(l) → 2 HNO₃(g) + NO(g)

What is the mass in grams of CO₂ that can be produced from the combustion of 2.45 moles of butane according to this equation: 2 C₄H₁₀(g) + 13 O₂(g) → 8 CO₂(g) + 10 H₂O(g)

According to the following balanced equation, what mass (in g) of MgO can be made from 7.5 g of 02? 2Mg (s) + O2 (g) 2MGO (s)

What is the mass in grams of CO₂ that can be produced from the combustion of 6.54 moles of butane according to this equation: 2 C₄H₁₀(g) + 13 O₂(g) → 8 CO₂(g) + 10 H₂O(g)

What is the mass in grams of NO that will be produced from 37.9 g of NO2 reacted with excess water in the following chemical reaction? 3 NO2(g) + H2O(1) → 2 HNO3(g) + NO(g)

How many grams of NO will be produced from 80.0 g of NO₂ reacted with excess 2 water in the following chemical reaction? 3 NO₂(g) + H₂O(l) → 2 HNO₂(g) + NO(g) A) 17.4 g B) 157 g C) 52.2 g D) 40.9 g

Calculate the theoretical yield (in grams) and percent yield in the following situations: Consider the following reaction:CO + 2 H2→CH3OH What is the theoretical yield and percent yield of CH3OH if the reaction of 2.50 g of H2with an excess of CO produces 8.00 g ofCH3OH?

Each step in the following process has a yield of 80.0%.CH4+4Cl2⟶CCl4+4HClCCl4+2HF⟶CCl2F2+2HClThe CCl4 formed in the first step is used as a reactant in the second step. If 2.00 mol CH4 reacts, what is the total amount of HCl produced? Assume that Cl2 and HF are present in excess.