3. Table salt (NaCl) is produced when sodium element reacts with chlorine gas. a) Write the balance chemical reaction. 2 Na +Cl2 2nacI b) Determine the mass of NaCl produced when 12.8 g of sodium reacts. c) Determine the mass of NaCl produced with 10.2 g of chlorine gas reacts. d) Which amount, 12.8 g of sodium or 10.2 g of chlorine gas, provides a better yield of NaCI?

3. Table salt (NaCl) is produced when sodium element reacts with chlorine gas. a) Write the balance chemical reaction. 2 Na +Cl2 2nacI b) Determine the mass of NaCl produced when 12.8 g of sodium reacts. c) Determine the mass of NaCl produced with 10.2 g of chlorine gas reacts. d) Which amount, 12.8 g of sodium or 10.2 g of chlorine gas, provides a better yield of NaCI?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

For the following reaction, 5.88 grams of bromine are mixed with excess chlorine gas . The reaction yields 6.50 grams of bromine monochloride . bromine ( g ) + chlorine ( g ) →→→→ bromine monochloride (g) What is the theoretical yield of bromine monochloride ? What is the percent yield for this reaction ? grams %
Consider the balanced chemical equation: 3 H₂(g) + N₂(g) → 2 NH₃(g) If 46.8 g H₂ and 179.4 g N₂ are mixed to form NH₃, which of the following substances is the limiting reactant? A) nitrogen (N₂) B) hydrogen (H₂) C) ammonia (NH₃)
If a 88.2 gram charcoal briquette (assume pure carbon) is burned in an excess of oxygen, what mass of CO2 is produced by the reaction?
6. Magnesium oxide can be produced by heating magnesium metal in the presence of oxygen. The balanced chemical equation for the reaction is: 2 Mg (s) + O2 (9) → 2 MgO (s) When 10.1 g of Mg react with 10.5 g of O2, 11.9 g of MgO are collected. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.
When 15.5 g of solid carbon combines with 8.0 g of oxygen gas, it will produce carbon monoxide gas. (atomic masses: C = 12.01 g/mol; O = 16.0 g/mol) Write the correct and balanced chemical equation for this reaction. Which is the limiting reactant? Which is the excess reactant?
[References] Use the References to access important values if needed for this question. For the following reaction, 168 grams of iron are allowed to react with 32.0 grams of oxygen gas. 2Fe (s) + O₂(g) →→→2FeO (s) What is the FORMULA for the limiting reagent? What is the maximum amount of iron(II) oxide that can be formed? What amount of the excess reagent remains after the reaction is complete? Submit Answer Retry Entire Group 9 more group attempts remaining grams grams
Calculate the amount of excess reactant left over at the end of the reaction, use the example.
what mass of calcium hydroxide in grams is needed to produce 5.11 mol of water?
6) Oxygen gas and hydrogen gas combine to make water according to the following chemical reaction. Assume a reaction mixture contains 237.1 g of 02 (g) and 53.8 g of H2 (g). Show calculations to support your answers. _02(9) + _H2(g) →_H,0(g) a. Write the balanced chemical reaction. b. Find the limiting reagent and calculate the theoretical yield in grams. c. If the actual yield is 201.5 g of H2O, what is the percent yield?
7. Silicon dioxide reacts with elemental carbon to give silicon carbide and carbon monoxide. SiO2(s) + 3 C(s) → SiC(s) + 2 CO(g) When 12.7 g SiO2 reacts with excess carbon, 7.28 g SiC is actually formed. What is the percent yield? (Hint: first calculate the theoretical yield).
This question has two parts and requires two answers. Consider the reaction 4 Fe + 3 02→ 2 Fe203 a) What is the theoretical yield, in grams, of iron(III) oxide if 20.0 g of iron are mixed with 10.5 grams of oxygen gas? b) What is the limiting reactant?
The limiting reactant is the reactant that is completely consumed in chemical reactions and determines the theoretical yield of reactions. When solid iron filings are added to a solution of copper(II) sulfate, an redox reaction occurs to form copper metal and one of two possible iron sulfate compounds. The unbalanced equations for the two possible reactions are given below. If 1.152 g of the Fe (the limiting reactant) are used, what is the theoretical yield according the balanced equation for reaction 1? Reaction 1: CuSO4(aq) + Fe(s) ⟶ ⟶ FeSO4(aq) + Cu(s) Reaction 2: CuSO4(aq) + Fe(s) ⟶ ⟶ Fe2(SO4)3(aq) + Cu(s)