If 21.0 g of NO and 13.8 g of O, are used to form NO2, how many moles of excess reactant will| be left over? 2 NO (g) + O2 (g) → 2 NO2 (g)

according to the equationP4(s)+6Cl2(g)→4PCl3(l)P4(s)+6Cl2(g)→4PCl3(l)A reaction mixture initially contains 45.35 gg P4P4 and 130.9 gg Cl2Cl2.       Once the reaction has reached completion, what mass (in gg) of the excess reactant is left?

In an experiment, 12.4 g of KClO3 were carefully decomposed, and 4.52 of O2 gas were collected.  What are the theoretical, actual, and percent yields of the reaction?   The unbalanced chemical reaction is given below.               KClO3  →   KCl  + 3 O2       Was the percent yield greater or less than 100%?  What are at least three reasons for the percent yield not being exactly 100%?

According to the following reaction, how many grams of nitrogen monoxide will be formed upon the complete reaction of 24.6 grams of oxygen gas with excess nitrogen gas? N₂ (g) + O₂ (g) →→→2NO (g) grams nitrogen monoxide

A student heats a 2.8695g sample of a mixture that contains an unknown amount of potassium chlorate (KClO3). The KClO3in the mixture decomposes and releases its oxygen. The mass of the remaining sample residue was 2.0427g. KClO3(s) →KCl (s) + 3 O (g) a.How many grams of oxygen were in the KClO3sample? b.How many moles of oxygen atoms is this? c.How many moles of KClO3were in the original sample? d.How many grams of KClO3were in the original sample? e.What is the % of KClO3in the original sample?

3. How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol. 4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)

What is the mass in grams of H₂ that can be formed from 47.0 grams of NH₃ in the following reaction? 2 NH₃(g) → 3 H₂(g) + N₂(g)

If 21.7 g of NO and 13.8 g of O, are used to form NO, how many moles of excess reactant will be left over? 2 NO (g) + O, (g) → 2 NO, (g)

16 X C3H8(g) +4 Cl₂(g) → C3H4Cl4(g) + 4 HCl(g) A 6.0 mol sample of C3H8(g) and a 20. mol sample of Cl₂(g) are placed in a previously evacuated vessel, where they react according to the equation above. After one of the reactants has been totally consumed, how many moles of HCl(g) have been produced? (A) 4.0 mol (B) 8.0 mol (C) 20. mol D24 mol

A sample of 0.75 g of hydrogen gas was obtained by reacting 32.5 g hydrochloric acid with 18.0 g magnesium. Mg(s) + 2 HCI (aq) --> MgCl₂ (aq) + H₂(g) What is the percent yield for this reaction? 100% 83% 41% 50%