based on the data table below what is the molar mass of H2O and moles released of H2O?  Aluminum Cup (Empty) 2.4 Aluminum Cup + 2.0 grams of Alum 4.4 Aluminum Cup + Alum After 1st Heating 3.7 Aluminum Cup + Alum After 2nd Heating 3.6 Mass of Released H2O 0.8 Molar mass of H2O   Moles of Released H2O

If 38.0 moles of NOBr2 decompose how many moles of O2 form ?

How many grams of N2 are needed to completely (stoichiometrically) react with  222 g of Br2 ?  N2   +   3 Br2   →   2 NBr3   +   44.0 kJ              The molar mass of Br2 is _____________ g and the molar mass of N2 is  ___________ g                                ____________ mol Br2                                                              (2.22 x 102 g Br2)(––––––––––––––––––––––––––––––)  =  __________ mol Br2                               _______________ g Br2                                                                                                                       ______________ mol N2 __________________ mol Br2 (–––––––––––––––––––––––––) =  _______________ mol N2                                                     __________________ mol Br2                                                       ___________________ g N2 _______________ mol N2 (–––––––––––––––––––––––––) =  _____________ g N2                                                    ________________ mol N2

answer question 4 in detail

80°F Mostly sunny Stoichiometry can be used to determine the mass (in grams) of a product. O True O False Search H &

Calculate the number of moles of oxygen needed to produce 2.5 moles of diphosphorus pentoxide? P4 (s) + 5 O2 (g) --> 2 P2O5 (s) * 1 point 1.0 mole 2.5 moles 3.0 moles 5 moles 6.3 moles

Read the given chemical reaction.C2H6 + O2 → CO2 + H2OHow many moles of O2 are required to react completely with 3.2 moles of C2H6?  3.5 moles of O2  6.5 moles of O2  10.4 moles of O2  11.2 moles of O2

How do I solve?

How many grams of N2 are needed to completely (stoichiometrically) react with 222 g of Br2 ? N2 + 3 Br2 2 NB13 + 44.0 kJ The molar mass of Br2 is g and the molar mass of N2 is mol Br2 (2.22 x 102 g Br2)(- mol Br2 g Br2 mol N2 mol Br2 (-- -) = mol N2 mol Br2 g N2 mol N2 (-- -) = |v g N2 mol N2 а. 1 b. 2 С. 3 d. 4 е. 5 f. 253.719 g. 3.38 х 100 h. 3.26 x 103 i. 44.0 j. 1.33 x 102 k. 9.77 x 103 I. 4.44 x 102 m. 6.66 x 10² n. 500.0 o. 556 р. 90.0 q. 3.2852 r. 159.81 s. 28.013 t. 1.750 u. 0.8750 v. 13.0 w. 0.46306 х. 1.3892 у. 24.5 z. 38.5 аа. 2.190 bb. evolved Cc. absorbed dd. exothermic ee. endothermic

B. Stoichiometry and Percent Yield DATA 1. Mass of sodium carbonate 2. Mass of filter paper 3. Mass of dry filter paper and calcium carbonate product CALCULATIONS AND QUESTIONS (show all of your work) 1. Mass of dried product (actual yield) (Mass of dry filter paper and calcium carbonate product - mass of filter paper) 1.0 g 1.2g 2.69 2. Write the balanced chemical equation for the reaction of sodium carbonate and calcium chloride. (Ignore the hydrate in this equation) 2.89 3. Use stoichiometry to calculate the theoretical yield of calcium carbonate product based on the starting mass of sodium carbonate. 4. Calculate the percent yield of the reaction based on the actual yield of dried calcium carbonate product and the theoretical yield of calcium carbonate product. 11