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- The combustion of 5.9 g of CXHYNZ yields 13.2 g CO2 and 8.1 g H2O. What is the empirical formula? Question 5 options: C2H7N2 C4H11N2 C3H9NHow many grams of chlorine gas can be produced from the decomposition of 73.4 g. of AuCl3 by this reaction:2AuCl3 ® 2 Au + 3 Cl2 Question 19 options: 25.7 g 33.6 g 11.4 g 195.3 gQuestion: Using this equation: C3H8 + 5O2 -> 3CO2 + 4H2O: to solve this: how many grams of water will be produced if 1.2 mol of oxygen reacts with excess C3H8
- QUESTION: If the sample in parts a, b, and c contained a carbon-based impurity, how would this affect the final empirical formula determined? ***Please do NOT solve parts a,b,c!! I ONLY need help with the question above about the carbon impurity.*** part a: A 10.00g unknown sample with a formula of CxHY was analyzed by combustion analysis. The sample produced 27.42g of CO2(g) and 22.46g H2O(g). Find the empirical formula of the unknown sample. for part a I determined the empirical formula to be: CH4 part b: A 10.00 gram unknown sample containing C, H, O, was analyzed by combustion analysis. The sample produced 19.10 grams of CO2 and 11.73 grams of H2O. Find the empirical formula of the unknown sample. for part b I determined the empirical formula to be: C2H6O part c: A 15.00 gram unknown sample containing C, H, O was analyzed by combustion analysis. The sample produced 29.3 grams of CO2 and 20.8 grams of H2O. Find the empirical formula of the unknown. for part c I determined the…How many grams of PbO (molar mass = 223.2 g/mol) are produced from the reaction of 4.0 grams of oxygen gas? Given the reaction 2PbS(s) + 3O2(g) ® 2PbO(s) + 2SO2(g) Question options: 334.8 2.7 42 1.9 x 10*4 19 3.7 x 10-4PLEASE SHOW ALL WORK FOR THE QUESTION BELOW IF POSSIBLE!! THANK YOU SOO MUCH!!!! Given the balanced equation: 2 H2 + CO ? CH3OH , how many moles of CH3OH will be produced if 12.6 g H2 reacts with 114.5 g CO?
- Answer the following: A 0.498g sample contains 26.0% aluminum triiodide, All3, (MW=407.695) by weight. What is the mass of aluminum triiodide in the sample? If the sample is reacted with silver nitrate, AgNO3, to precipitate silver iodide, Agl, what will be the stoichiometric ratio of AgNO3 to All3? What is the maximum mass of Agl (MW=234.77) that can be produced from the sample?how many water moleculesare produced if .34 moles of propane C3H8 combusts in excess oxygen? C3H8+5O2=3CO2+4H2Ohow many moles of CO would be produced by the reaction 2FE + 3CO -->fe2O3 + 3CO
- Please help :) A 49.2-gram sample of aluminum metal is mixed with 144.1 grams of rust (Fe2O3) in the reaction shown below in a sealed container. The balances equation is: 2Al + Fe2O3 --> Al2O3 + 2Fe A. How many atoms of aluminum are contained in the reaction vessel? B. How many atoms of aluminum will remain in the container after the reaction? C. What mass of iron metal is produced from this reaction? D. Which substance is the limiting reactant? E. How much limiting reactant is left over after the reaction is performed? F. How much excess reactant is left over after the reaction? G. Calculate the amount of aluminum oxide that will be produced. Use this answer and the ones above to demonstrate that mass is conserved before and after the reaction occurs.Question: Given the following equation: 2 C4H10 + 13 O2 → 8 CO2 + 10 H2O How many moles of C4H10 are needed to react with 4 mol of O2?Suppose you were tasked with producing some nitrogen monoxide (a.k.a. nitric oxide). I'm sure this is often requested of you. You can do it by combusting ammonia (be careful!). The equation would be as follows: 4NH3 + 5O 2→ 4NO + 6H2O. If you form 2 mol of water, how much NO forms?