Part A: How many grams of carbon dioxide are produced from 79.00 grams of butane (C4H10) ? Part B: If only 130.0 grams of carbon dioxide was formed, what was the percent yield?

Liquid nitroglycerine (CaHsNaO₂) is a powerful explosive. When it detonates, it produces a gaseous mixture of nitrogen, water, carbon dioxide and oxygen. If 5.55 g of nitroglycerine explodes and 2.98 g of CO₂ is collected, what is the percentage yield of carbon dioxide?

For the following reaction, 15.9 grams of glucose (C6H1206) are allowed to react with 12.4 grams of oxygen gas > carbon dioxide(g) + water( glucose (CH1206(s) + oxygen(g) What is the maximum amount of carbon dioxide that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams

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?

Consider the balanced chemical equation: 3 H₂(g) + N₂(g) → 2 NH₃(g) If 46.8 g H₂ and 179.4 g N₂ are mixed to form NH₃, which of the following substances is the limiting reactant?   A) nitrogen (N₂) B) hydrogen (H₂) C) ammonia (NH₃)

2 C4H10 + 13 02 → 8 CO2 + 10 H20 Part A: How many grams of carbon dioxide are produced from 79.00 grams of butane (C4H10) ? Part B: If only 130.0 grams of carbon dioxide was formed, what was the percent yield?

When the substance shown below burns in oxygen, the products are carbon dioxide and water. How many grams of water are obtained from burning 4.76 g of this substance? g H20 mass =

If 100 grams of CH4 is made to react with 200 grams of O2, what mass of CO2 (in grams) is formed?

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N2(g) → 2Li3N(s)In a particular experiment, 3.50 g samples of each reagent are reacted.a) What is the limiting reagent?b) What is the theoretical yield in grams of lithium nitride?c) If only 4.25 grams of lithium nitride is produced in the reaction, what is the percent yield?

Consider the following balanced chemical equation:    2NH3(g) + 5F2(g)  →  N2F4(g) + 6HF(g)   Determine the theoretical yield of HF, in grams, when 54.60 g of NH3 reacts with 54.60 g of F2.  g HF   What is the percent yield if 7.180 g hydrogen fluoride (HF) is actually formed during the reaction?