Butane has the chemical formula C4H10 and is a component of natural gas. When butane burns, it reacts with oxygen according to the following balanced equation: 2C4H10+1302 8CO2 + 10H₂O What is the mass relationship between butane and water in this reaction? (Enter your answer to four significant figures.) g H₂0/1 g C4H10

The reaction between potassium chlorate and red phosphorus takes place when you strike a match on a matchbox. If you were to react 30.9 g of potassium chlorate (KClO3) with excess red phosphorus, what mass of tetraphosphorus decaoxide (P4O10) could be produced? Mass = KClO3(s) + P4(s) → P4O10 (s) + KCl(s) (unbalanced) g

Elemental phosphorus reacts with chlorine gas according to the equation P4(s) + 6Cl2 (g)➡️ 4PCl3 (l)A reaction mixture initially contains 45.39 g P4 and 131.0 g Cl2 .Once the reaction has reached completion, what mass (in g) of the excess reactant is left? ( Express using 3 significant figures)

You are given the balanced chemical reaction: C4H8(g) + 6 O2(g) 4 CO2(g) + 4H₂O(g). If 0.3218 moles of C4H8 are allowed to react with 2.015 moles of O2, and this is the only reaction which occurs, what is the maximum quantity of water, in grams, that could be produced and what is the limiting reagent?

A mixture of N2(g) and H2(g) reacts in a closed container to form ammonia, NH3(g). The reaction ceases before either reactant has been totally consumed. At this stage 2.4 mol N2, 2.4 mol H2, and 2.4 mol NH3 are present. Express your answer using two significant figures. How many moles of N2N2 and H2H2 were present originally? Enter your answers numerically separated by a comma.

The first step in the manufacture of nitric acid by the Ostwald process is the reaction of ammonia gas with oxygen, producing nitrogen oxide and steam. The reaction mixture contains 8.26 g of ammonia and 10.2 g of oxygen. After the reaction is complete, 6.67 g of nitrogen oxide are obtained. Write a balanced equation for the reaction. How many grams of nitrogen oxide can be theoretically obtained? How many grams of excess reactant are theoretically unused? What is the percent yield of the reaction? g nitric oxide g excess reactant %

Aqueous hydrobromic acid  HBr  will react with solid sodium hydroxide  NaOH  to produce aqueous sodium bromide  NaBr  and liquid water  H2O . Suppose 0.809 g of hydrobromic acid is mixed with 0.55 g of sodium hydroxide. Calculate the maximum mass of sodium bromide that could be produced by the chemical reaction. Be sure your answer has the correct number of significant di

The following reaction is used to produce magnesium oxide: 2Mg (s) + O2  →  2MgO                         If 32.0 grams of O2 reacts with 24.3 grams of magnesium, which is the limiting reactant and what is the theoretical yield of this reaction?

Magnesium will react with steam, forming magnesium hydroxide and hydrogen gas, as shown in the reaction below.   Mg(s) + 2 H2O(g) → Mg(OH)2(s) + H2(g)   Consider an experiment in which 81.7 g of steam and 35.2 g of magnesium are allowed to react in a sealed reaction vessel.   What mass of Mg(OH)2 will be created?

2MgO (s) -> 2Mg (s) +  O2 (g) If 1.314 * 10^24 molecules of magnesium are produced, how many molecules of oxygen will be produced? If a chemical company needs to produce 4.6 moles of magnesium oxide, how many grams of magnesium would be required?