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LR whiteboard practice. NH 3 + O 2  NO + H 2 O. In an experiment, 3.25 g of NH 3 are allowed to react with 3.50 g of O 2. a. Which reactant is the limiting.

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Presentation on theme: "LR whiteboard practice. NH 3 + O 2  NO + H 2 O. In an experiment, 3.25 g of NH 3 are allowed to react with 3.50 g of O 2. a. Which reactant is the limiting."— Presentation transcript:

1 LR whiteboard practice

2 NH 3 + O 2  NO + H 2 O. In an experiment, 3.25 g of NH 3 are allowed to react with 3.50 g of O 2. a. Which reactant is the limiting reagent? b. How many grams of NO are formed?

3 NH 4 NO 3 + Na 3 PO 4  (NH 4 ) 3 PO 4 + NaNO 3 Which reactant is limiting, assuming we started with 30.0 grams of ammonium nitrate and 50.0 grams of sodium phosphate. What is the mass of NaNO 3 that can be formed?

4 C 4 H 9 OH + NaBr + H 2 SO 4 C 4 H 9 Br + NaHSO 4 + H 2 O If 15.0 g of C 4 H 9 OH react with 22.4 g of NaBr to yield 17.1 g of C 4 H 9 Br, what is the percent yield of this reaction?

5 CaCO 3 + FePO 4  Ca 3 (PO 4 ) 2 + Fe 2 (CO 3 ) 3 Which reactant is limiting, assuming we start with 100. grams of calcium carbonate and 45.0 grams of iron (III) phosphate. What is the mass of iron carbonate that can be formed?

6 CuCl 2 + NaNO 3  Cu(NO 3 ) 2 + NaCl a)If 15 grams of copper (II) chloride react with 20. grams of sodium nitrate, how much sodium chloride can be formed? b) What is the name of the limiting reagent? __________________ c) If 11.3 grams of sodium chloride are formed in the reaction, what is the percent yield of this reaction?

7 C 2 H 6 + O 2  CO 2 + H 2 O a)If 16.4 g of C 2 H 6 reacts with mol of O 2 how many grams of carbon dioxide gas will be produced?

8 Fe (s) + S (l)  FeS (s) In one experiment, 7.62 g of Fe are allowed to react with 8.67 g of S. What is the limiting reagent, and what is the reactant in excess? Calculate the mass of FeS formed.

9 4 C 3 H NO → 4 C 3 H 3 N + 6 H 2 O + N 2 What mass of C 3 H 3 N can be made when 21.6 g of C 3 H 6 react with 21.6 g of NO?

10 Calculate the percent yield for the reaction: P 4 (s) + 6 Cl 2 (g) → 4 PCl 3 (l) if 75.0 g of phosphorus reacts with excess chlorine gas to produce g of phosphorus trichloride.

11 MnO HCl → MnCl 2 + Cl H 2 O If 0.45 mols of MnO 2 react with 48.2 g of HCl, how many grams of Cl 2 could be produced?

12 Calculate the percent yield for an experiment in which 5.50 g of SOCl 2 was obtained in a reaction of 5.80 g of SO 2 with excess PCl 5. Use the following equation: SO 2 (l) + PCl 5 (l) → SOCl 2 (l) + POCl 3 (l).

13 Cl 2 (g) + SiO 2 (s) + C (s) → SiCl 4 (l) + CO (g) How much CO gas can be produced from 15.0 g of SiO 2 ? Ans: 14.0 g CO

14 Fe(OH) 2 + H 3 PO 4 → Fe 3 (PO 4 ) 2 + H 2 O a.If 3.20 g of Fe(OH) 2 is treated with 2.50 g of phosphoric acid, what is the limiting reagent and what is the reactant in excess? b.How many grams of Fe 3 (PO 4 ) 2 precipitate can be formed? c.If 3.99 g of Fe 3 (PO 4 ) 2 is actually obtained, what is the percent yield?

15 CO (g) + 2 H 2 (g) → CH 3 OH (l) Suppose 356g of CO is mixed with 65.0g of H 2. Which is the limiting reactant? What is the maximum mass of methanol that can be formed? ANS: CO is limiting, 408 g CH 3 OH formed

16 SiCl 4 (l) + 2 Mg (s) → Si (s) + 2 MgCl 2 (s) Suppose that 225g SiCl 4 is mixed with 225g of Mg. Is one of these reactants in short supply? If so, how much silicon can be formed if the reaction goes to completion? ANS: SiCl 4 is limiting, 37.2 g Si formed

17 You have 20.0g of elemental sulfur, S 8, and 160g of O 2. Which is the limiting reactant? What mass of SO 2, in grams, is formed in the complete reaction if the formula for the reaction is… S 8 (s) + 8 O 2 (g) → 8SO 2 (g) ANS: S 8 is limiting, 40.0 g SO 2 formed

18 TiO 2 (s) + 2 Cl 2 (g) + C (s) → TiCl 4 (l) + CO 2 (g) If one begins with 125g each of Cl 2 and C, but plenty of TiO 2 -containing ore, which is the limiting reactant in this reaction? What quantity of TiCl 4, in grams, can be produced? ANS: Cl 2 is limiting, 167 g TiCl 4 produced

19 Cl 2 (g) + NaI(aq) → NaCl(aq) + I 2 (s) Suppose that a solution containing 25.0 g NaI reacts with 5.00 g of Cl 2. What mass of iodine will be produced from the reaction above?

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