4.00 g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 26. g/mol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass carbon dioxide 13.54 g water 2.77 g Use this information to find the molecular formula of X. 0 ☐☐ S P

Consider the following balanced chemical reaction: HNO3 + 3H2 → NH2OH + 2H2O If 25.0 grams of HNO3 were mixed with 8.70 grams of H2 gas, how many grams of NH2OH would result? Molar mass of HNO3 = 63.01 g/mol Molar mass of NH2OH = 33.03 g/mol

Use the References to access Important values If needed for this question. For the following reaction, 5.40 grams of ammonia are allowed to react with 17.1 grams of oxygen gas. ammonia (g) + oxygen (g) nitrogen monoxide (g)+ water (g) What is the maximum amount of nitrogen monoxide that can be formed? What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? Submit Answer Retry Entire Group 2 more group attempts remaining grams grams Previous

Consider the following balanced equation: 2 H2 + O2 → 2 H2OWhat mass of water (H2O) will be collected if 20.0 grams of oxygen gas (O2) are consumed? (Mass of H2O = 18.02 g/mol and Mass of O2 = 32.00 g/mol)

Liquid hexane  CH3CH24CH3  reacts with gaseous oxygen gas  O2  to produce gaseous carbon dioxide  CO2  and gaseous water  H2O . If  3.58g  of water is produced from the reaction of  6.03g  of hexane and  11.5g  of oxygen gas, calculate the percent yield of water.

During the decomposition of KClO3, 4.14 grams of oxygen gas are created. How many moles of KClO3 reacted? Report your answer with 3 significant figures. 2 KClO3 → 2 KCl + 3 O2

Use 1 decimal point for all atomic masses. 12.3 g of NCl3(g) are reacted with 0.605 g of H2(g) by the following reaction   NCl3(g) + 3H2(g) --> NH3(g) + 3HCl(g) What is the limiting reagent? NCl3(g) H2(g)     Based on the limiting reagent, what should the yield of NH3(g) be?

9.00g of a certain Compound X, known to be made of carbon, hydrogen and perhaps oxygen, and to have a molecular molar mass of 60./gmol, is burned completely in excess oxygen, and the mass of the products carefully measured: product mass carbon dioxide 13.20g water 5.40g Use this information to find the molecular formula of X.

For the reaction shown, calculate how many moles of NO2NO2 form when each amount of reactant completely reacts. 2N2O5(g)→4NO2(g)+O2(g)

The combustion of propane produces carbon dioxide and steam.             C3H8(g)  +  5 O2(g)  →  3 CO2(g)  + 4 H2O(g) All of the following statements concerning this reaction are correct EXCEPT a) three molecule of carbon dioxide are formed per one molecule of propane consumed. b) five molecules of oxygen are consumed per one molecule of propane consumed. c) four moles of steam are formed per five moles of oxygen consumed. d) the combined mass of reactants consumed equals the mass of products formed. e) three grams of carbon dioxide are formed per five grams of oxygen consumed.