# What is the limiting reactant in this experiment? Assume you used 1.0 g of the copper(II) sulfate pentahydrate and 7. 5 mL of 6.0 M NH3. Show your calculations. Its been a while need some help, thanks!

20,587 results
1. ## CHEM

My balanced equation is: a) 2C8H18(g) + 25O2(g) -> 16CO2(g) + 18H2O(g) b) 0.290 mol of octane is allowed to react with 0.670mol of oxygen. Which is the limiting reactant? (((Which I found Oxygen to be the limiting reactant.))) I do not understant how to

2. ## Chemistry

Consider equation 3A+B=C+D. You react 4 moles of A with 2 moles of B. Which of the following is true? 1) Limiting reactant (L.R.) is one with higher molar mass 2) A is L.R. because you need 6 moles of A and have only 4 moles 3) B is L.R. because you have

3. ## Chemistry

For each of the following unbalanced equations, suppose that exactly 15.0g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of each product is expected. assume the limiting reactant is completely consumed.

4. ## Chemistry

The fizz produced when an Alka-Seltzer® tablet is dissolved in water is due to the reaction between sodium bicarbonate (NaHCO3) and citric acid (H3C6H5O7): In a certain experiment 1.45g of sodium bicarbonate and 1.45g of citric acid are allowed to react.

5. ## chemistry

i am working on a practice worksheet and need help with a few i can not understand. please and thank you. I have to post them separately sorry 49.how many grams of water are needed to completely hydrolyze 30.8 g of the ester? A.0.416 g B.30.8 g C.11.3 g

6. ## Chemistry

1. If you had 1.73 moles of hydrogen (H2) and 0.89 moles of oxygen (O2), which would be the limiting reactant? How many moles of water can you produce from your supply of hydrogen and oxygen? My answers: H2 is the limiting reactant because it produces the

7. ## Chemistry

Take the reaction: NH3 + O2 ---> NO + H2O. In an experiment, 3.25 g of NH3 are allowed to react with 3.50 g of O2. Which reactant is the limiting reagent? You may either write the formula or the name of the limiting reactant.

8. ## Chemistry

H3C6H5O7(aq) + 3NaHCO3(aq)----Na3C6H5O7(aq) + 3H2O(i) + 3CO2. NaHCO3 = 2.00g H3C6H5O7 = 0.76 CO2 = 0.07g 1.Determine which reactant is the limiting reactant . describe your reasoning. 2. Calculate the theoretical yield of carbon dioxide in the plastic 3.

9. ## Chemistry

2Al + 3CuSO4 --> + 3Cu + Al2(SO4)3 * copper(II) sulphate is a hydrate 1.2g of CuSo4 50mL of water 1.0 g of aluminum foil What is the limiting reactant?

10. ## Chemistry :(

Disulfur dichloride, S2Cl2, is used to vulcanize rubber. It can be made by treating molten sulfur with gaseous chlorine: S8(l) + 4 Cl2(g) --> 4 S2Cl2(l) [Molar masses: 256.6 70.91 135.0] Starting with a mixture of 32.0 g of sulfur and 71.0 g of Cl2, which

11. ## chemistry

Nitrogen gas can be prepared by passing ammonia over solid copper (II) oxide according to the equation 2 NH3 + 3 CuO (s) --> N2 (g) + 3 Cu (s) + 3 H2O (g) Suppose 18.1 grams of ammonia is reacted with 90.4 grams CuO. a) What is the theoretical yield of

12. ## Chem

If 2.00 grams of potassium are allowed to react with 2.00 grams of bromine by the following equation, which reactant is the limiting reactant?

13. ## chemistry

2KI+Pb(NO3)2=2KNO3+PbI2 suppose a solution containing 1.25g of KI is combined with a solution containing 2.42g Pb(NO3)2 _what mass of the yellow PbI would result what is the limiting reactant How much in grams of the excess reactant was used how much in

14. ## aaa

Take the reaction : NH3 + O2 = NO + H2O in a experiment, 5 moles of NH3 are alloved to react with 5 moles of O2 a) which reactant is the limiting reagent ? b) How many grams of NO are formed ? c) How much of the excess reactant remains after the reaction ?

15. ## Science

1 kg of Nitrogen is mixed with 3.5 m3 of hydrogen at 300 K and 101.3 kPa and sent to ammonia converter. The product leaving the converted analyzed 13.7% ammonia, 70.32% hydrogen and 15.98% nitrogen. (a) Identify the limiting reactant? (b) What is the

16. ## Chemistry

copper(1) chloride reacts with hydrogen sulfide. if 9.90 grams of copper(1) chloride and 10.2 grams of hydrogen sulfide are reacted together, what is the limiting reactant?

17. ## Chemistry

Given this equation: 2P2O5 + 6H2O ---> 4H3PO4. If you begin with 4.8 grams of p2o5 and 15.2 grams h20, what will be your limiting reactant. I got the answer to that and it is P2O5. (6.6 grams) and H2O was 55.2 grams. so the limiting reactant P2O5. Then the

18. ## Chemistry

What is the limiting reactant when 19.9g of CuO are exposed to 2.02g of H2 according to the following equation? CuO + H2 ---> Cu + H20 My attempt at this: 19.9gCuO * 1moleCuO/79.539gCuO * 1moleCu/1moleCuO = .250moleCu 2.02gH2 * 1moleH2/2.016gH2 *

19. ## Chemistry (Help)

For the chemical reaction, sodium hydroxide + copper (II) chloride = "robin's egg blue" precipitate, do the following: write the balanced molecular, balanced total ionic, and balanced net ionic equations; determine the Limiting Reactant (LR) for each

20. ## Chemistry

1. Ca(OH)2 + H3PO4 ---> H2O + Ca3(PO4)2 (A) How many moles of H3PO4 are needed to make 15g of H2O? (B) What mass in grams of Ca(OH)2 is used to react with 5.6mol of H3PO4? (C) How many grams of Ca3(PO4)2 are made from 134g of Ca(OH)2? 2. Fe2O3 + CO ---> Fe

21. ## Chemistry

In a reaction between pure acetic acid and sodium bicarbonate, 14.7 grams of sodium bicarbonate was added to 21.0 mL of acetic acid. Which reactant is the limiting reactant in this reaction? Name of limiting reactant (acetic acid or sodium bicarbonate):

22. ## Chemistry

The fizz produced when an Alka-Seltzer® tablet is dissolved in water is due to the reaction between sodium bicarbonate (NaHCO3) and citric acid (H3C6H5O7): 3NaHCO3(aq)+H3C6H5O7(aq)→3CO2(g)+3H2O(l)+Na3C6H5O7(aq) In a certain experiment 1.20 g of sodium

23. ## Chemistry

S8+4Cl2 -----> 4S2Cl2 A) what mass of S2Cl2 can be produced? B) what mass of the excess reactant remains When the limiting reactant is consumed?

24. ## Chemistry

I was doing a lab experiment on the reaction of copper(II) sulphate and aluminum: 1) I measured 2.02g of copper(II) sulphate pentahydrate 2) I dissolved the copper(II) sulphate pentahydrate in 10mL of distilled water 3) I added 2.0mL of concentrated HCl to

25. ## Chemistry

ammonia gas reacts with copper (ii) oxide at high temperatures to produce elemental nitrogen, copper metal, and water vapor. Assume that 36.2g ammonia reacts with 180.8 g copper ii oxide. (balanced equation: 2 NH4 (ammonium) (g) + 4 CuO (copper ii oxide)

26. ## Chemistry

1. Cisplatin is an anti tumor agent. It has the molecular formula Pt(NH3)2Cl2. How many grams of cisplatin can be produced if the limiting reactant is 1 kg of platinum? I got 1538.1 g Pt(NH3)2Cl2. 2. Hydrogen cyanide is used in the production of cyanimid

27. ## Chem Very Urgent

if 4.55 g of sodium sulphide and 15.0 g of bismuth nitrate are dissolved in separate beakers of water which are then poured togehter, what is the maximum mass of bismuth sulphide an insoulble compound that could precipitate? Which reactant was the

28. ## chemistry

Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride.

29. ## Chemistry

When ammonia was reacted to copper(ll)oxide at a high temperature, it will produce nitrogen gas, copper metal and water vapour. an experiment was done with 18.0g of ammonia was reacted with 90.0g of copper(ll)oxide. (a)Write balance chemical equations for

30. ## Chemistry

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

31. ## CHEMISTRY

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

32. ## Chemistry

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

33. ## Chemistry

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

34. ## Chemistry

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

35. ## CHEMISTRY

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

36. ## CHEMISTRY

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

37. ## Chemistry

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

38. ## CHEMISTRY

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

39. ## Chemistry

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

40. ## CHEMISTRY

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

41. ## Chemistry

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

42. ## CHEMISTRY

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

43. ## Chemistry

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

44. ## Chemistry

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

45. ## Chemistry

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

46. ## Chemistry

im a little confuse on this problem. "in the production of copper from ore containing copper(II) sulfide, the ore is first roasted to change it to the oxide according to the following equation: 2CuS + 2O2 --> 2CuO + 2CO2 [i already balanced it] A. If 100 g

47. ## Chemistry

Consider the equation: A + 4B=3C+3D, when equal masses of A and B are reacted, which is limiting? My possible answers are: A)if the molar mass of A is less than the molar mass of B, then B must be limiting. B) If the molar mass of A is greater than the

48. ## Chemistry

Assume that the reaction was limited by the surface area of the nails, making Fe the limiting reactant. Based on the decrease in the mass of nails, calculate theoretical yield of copper. 2Fe+3CuCl2--->2FeCl2+3Cu

49. ## Chemistry

You have .5g of copper. If the nitric acid is 16 M HNO3, how many milliliters of nitric acid will react exactly with that amount of copper. I know that when I get that volume I will triple it so that there will be excess acid and the copper will be the

50. ## Chemistry

In an experiment 0.5300 g of ferric oxide is reacted with 0.3701 g of carbon monoxide gas according to the equation: Fe2O3 + CO ==> Fe + CO2. A. What is the limiting reactant? B. What mass of the other reactant is in exess? C. What mass of iron is

51. ## Chemistry

What is the limiting reactant if 0.500 g Aluminum is reacted with 3.500 g Copper (II) chloride (when calculating the molar mass of copper chloride you need to add mass of 2H2O because it is a dihydrate)?

52. ## Chemistry

If 10.0 grams of sodium bicarbonate reacts with 50.0mL of 2M acetic acid, what is the limiting reactant? what reactant is in excess, and by how much? What volume of carbon dioxide gas would form?

53. ## Chemistry

Determine which reactant is the limiting reactant, if, Mass of Sodium Bicarbonate= 2.00g Mass of Citric Acid = 0.76g Are my calculations right, or is it wrong? (2.00g of NaHO3)(1mol/84.01g of NaHO3)(1mol of H3C6H5O7/ 3 mol of NaHO3)(192.14g of H3C6H5O7)=

54. ## Chem 202

What is the limiting reactant in this experiment? Assume you used 1.0 g of the copper(II) sulfate pentahydrate and 7. 5 mL of 6.0 M NH3. Show your calculations. Its been a while need some help, thanks!

55. ## Chemistry

I need some help with my Limiting Reactant Experiment report sheet. There is a question asking me to write a complete formula of the limiting reactant in the salt mixture of CaC2O4 X H2O. I don't know where to begin. Could you please help me.

56. ## Chemistry

I was doing a lab experiment: 1) I measured 2.02g of copper(II) sulphate pentahydrate 2) I dissolved the copper(II) sulphate pentahydrate in 10mL of distilled water 3) I added 2.0mL of concentrated HCl to the solution and mixed well 4) I added 0.25g on

57. ## chemistry

for the reaction: 4NH3+5O2=4NO+6H2O; 15.0g of NH3 and 27.5g of O2 were reacted. a). which is the limiting reactant? b).how many moles of NO are formed from the limiting reactant in the above reaction. i know how to do the moles but i couldn't figure out

58. ## Chemistry

25.0 grams of ammonium sulfide reacts with 25.0 grams of copper nitrate A) which reactant is limiting B) how much of the Excess reactant remains C) what is the theoratical yield

59. ## CHEMISTRY! HELP

I'm not sure how to do or show the work for these two questions. A) & B.)!! please anyone help: A.) Suppose a chemical reaction starts with 5.00 g of copper (i) nitrate and 2.00 g of magnesium chloride. Balanced Equation: 2 CuNo3 + MgCl2 ---> 2 CuCl +

60. ## Chemistry

based on the following chemical equation HCN+O2 yields N2+CO2+H20 identify the limiting reactants and the mass of N2 produced when 100.0g of HCN react with 100.0g of O2. a. the limiting reactant is HCN and 25.9g of N2 are produced b. the limiting reactant

61. ## Chemistry

In an experiment 10.124 g of magnesium is reacted with 4.273 g of oxygen gas according to the equation: Mg + O2 ==> MgO. A. What is the limiting reactant? B. What mass of the other reactant is in exess? C. What mass of MgO is produced?

62. ## Chemistry

Calculations involving a limiting reactant Now consider a situation in which 20.0 g of P4 is added to 54.0 g of Cl2, and a chemical reaction occurs. To identify the limiting reactant, you will need to perform two separate calculations: 1) Calculate the

63. ## Foundation Chem

Why do we need to keep water warm in a limiting reactant experiment around 80 to 90 degree celcius

64. ## Chemistry

Given that 10.0 atm each of NO and O2 are introduced into a reaction vessel at room temperature. Calculate the partial pressure of each gas at equilibrium. 2NO(g)+O2 (g)---> 2NO2 (g) Kp =4.2x1012. at. roomtemperature. To solve this question I need to find

65. ## chemistry

for the reaction: 4NH3+5O2=4NO+6H2O; 15.0g of NH3 and 27.5g of O2 were reacted. a). which is the limiting reactant? b).how many moles of NO are formed from the limiting reactant in the above reaction. what would be the first step in this problem?

66. ## chemistry

How is a mole ratio used to find the limiting reactant? Is there a specific equation to find the limiting reactant? Can someone explain it to me because I don't understand it.

67. ## chem

18.1g of ammonia and 90.4g of copper(II) oxide are used in the reaction 2NH3+3CuO=N2+3Cu+3H3O.What is the limiting reactant? How many grams of nitrogen will be formed?

68. ## Chemistry

A decomposition reaction is one in which a reactant decomposes to a limiting reactant and a theoretical reactant. True or False

69. ## chem

3. Given a chemical reaction and H associated with the reaction: stoichiometry and limiting reactant problem involving gases. Why would we need delta H for a stoichimetry or limiting reactant problem? And can i get an example pleasE?

70. ## chemestry

Based upon the previous two questions, consider the magnesium nitride addition reaction again. This time, suppose you start with 10.0 g of each reactant. What is the maximum number of MOLES of Mg3N2 that could be produced in this case? Remember that the

71. ## Science

Hi, I am working on stoichiometry and limiting reactant problems. I have worked through examples in my book and I did them right and can solve for the excess, however there is one problem in the book that has confused me. I don't understand why they

72. ## Chemistry

4.67g of calcium reacts with 43.7g of oxygen gas. What is the limiting reactant and the excess reactant. How much of the excess reactant will be left over in grams?

73. ## Chemistry

1) 800 mL of 0.025 M Pb(NO3)2 is mixed with 500 mL of 0.030 M K2CrO4. Calculate the grams of PbCrO4 that form. I am confused on how to do this I got the answer it should be 4.85 g PbCrO4, but I would want to know how to get that. And also Limiting reactant

74. ## Science URGENT

Hi, I am working on stoichiometry and limiting reactant problems. I have worked through examples in my book and I did them right and can solve for the excess, however there is one problem in the book that has confused me. I don't understand why they

75. ## chemistry

If, in the reaction below, 31 g of C4H10 produces 41 41 g of CO2, what is the percent yield? Assume that the one reactant is limiting. 2C4H10 + 13O2 + 10H2O

76. ## Chemistry

determine how much copper you will use. based on the mass of silver nitrate, calculate how much copper will you need to ensure copper is the excess reactant. you need to use 300% excess copper. Help me please!

77. ## Chemistry

Consider equation 3A+B=C+D. You react 4 moles of A with 2 moles of B. Which of the following is true? 1) Limiting reactant (L.R.) is one with higher molar mass 2) A is L.R. because you need 6 moles of A and have only 4 moles 3) B is L.R. because you have

78. ## Chemistry

How do I distinguish between the limiting reactant and excess reactant in a chemical equation?

79. ## Chemistry

How do I distinguish between the limiting reactant and excess reactant in a chemical equation?

80. ## Chemistry

How do you find the moles of excess reactant? I already know the limiting reactant btw.

81. ## chemistry

2.00mL of 0.01 mol/L aqueous sodium sulphide is used to test a 50.omL sample of water containing 0.0005 mol/L mercury (II) nitrate ions. What mass of precipitate is formed? Na2S + Hg(NO3)2 --- 2NaNo3 + HgS determine limiting reactant using limiting

82. ## Chemistry

15.6g of Lithium fluoride reacts with 13g of nickel (II) sulfide. What is the limiting reactant and the excessive reactant? Show work.

83. ## chemistry

For the reaction: 2MnO2+ 4KOH+ O2+ Cl2 yields 2KMnO4+ 2KCL+ 2H20 there is 100. g of each reactant available. Which reagent is the limiting reactant?

84. ## chemistry

help me find which reactant is the limiting reactant when 74 g NaOH and 44 g CO2 are allowed to react when the equation is (2NaOH+1CO2=Na2CO3+1H2O)

85. ## Chemistry Dr. Bob222

Ok, UMMMM I thought I was good.. Till now.. Ok, For Cup C Mass of cup,water,stirrer: 55.15 Mass of sodium bicarbonate: 2.02g mass of citric acid: 0.77g total mass: 57.94g mass of cup,solution, stirrer after reaction: 57.64 difference (CO2): 0.30g Part B:

86. ## chemestry

Based upon the previous question, what is the THEORETICAL YIELD (in grams) of Mg3N2 if you start with 10.0 grams of each reactant? previous question:consider the magnesium nitride addition reaction again. This time, suppose you start with 10.0 g of each

87. ## Chemistry

Stoichiometry; Find the percent yield of solid calcium carbonate made when 5.0 mL of 1.0 M Sodium Carbonate reacts with 0.40g Calcium Chloride Balanced Equation; Na2(CO3)+CaCl2-->2NaCl+CaCo3 could you please help me step by step to find the theoretical

88. ## chem

Which do you run out of first, the limiting reactant or the excess reactant?

89. ## chemistry

N2 + 2O2 -->2 NO2 Suppose 31.25 g of N and 44.0 G of O react A. Calculate the mass of Nitrogen Dioxide formed. B. Which reactant is the limiting reactant? C. Calculate the mass of the excess reactant left after the reaction. D. Find the % yield if 52.3 g

90. ## chemistry

N2 + 2 O2 ---> 2 NO2. Suppose 31.25 g of N and 44.0 g of oxygen react. A. Calculate the mass of Nitrogen dioxide formed. B. Which reactant is the limiting reactant? C. Calculate the mass of the excess reactant left after the reaction. D. Find the % yield

91. ## Chem (general)

Little confused on how to get part B. A) if 3.00g of hydrosulfuric acid is reacted with 3.00g of silver nitrate, calculate the mass (in g) of solid silver sulfide formed. Which is the limiting reactant? (Hint: the other product is nitric acid). B)

92. ## chemistry

if you react 5.00g of aluminum with 20.0g of iodine, how much aluminum iodide do you expect to produce from this reaction? what is the limiting reactant ? what is the excess reactant? how much of the excess reactant do you expect to have left over?

93. ## chemistry

If 11.53g hydrogen sulfide reacts with 3.97g oxygen gas in the following reaction: 2H2S + O2 + H2O which is the maximum mass of sulfur that can be produced? which is the limiting reactant ? which reactant is in excess ? by how many grams?

94. ## Chemistry

Determine which reactant is the limiting reactant, if, Mass of Sodium Bicarbonate= 2.00g Mass of Citric Acid = 0.76g Are my calculations right, or is it wrong? (2.00g of NaHO3)(1mol/84.01g of NaHO3)(1mol of H3C6H5O7/ 3 mol of NaHO3)(192.14g of H3C6H5O7)=

95. ## chemsistry

If one pound (454g) of hexane combusts with 185 grams of oxygen which reactant is the limiting reactant and how many grams of carbon dioxide are produced? how do I do this? How do I set it up?

96. ## Chemistry

Hey guys so I was absent for my class and my teacher STILL wants me to figure out how to do limiting reactant and theoretical yield I tried Khan academy and it was no use. So basically the first question is : My data is : Mass of lead nitrate = 5.03g and

97. ## chemistry

If 80.0 g of bromine is added to 40.0 g of sodium, a) what is the limiting reactant? b) what is the excess mass of the reactant? c) what is the mass of product?

98. ## Chemistry

These are all true or false questions, and I think some of my answers may be wrong. Could someone please check them for me? 1) All stoichiometry calculations are based on STP conditions. (True) 2. Given the amount of reactant, you must use coefficients

99. ## Chemistry

given 65g of Zn and 65g of HCl, what is the limiting reactant and reactant in excess in Zn + 2HCl- ZnCl2 + H2

100. ## applying stoichiometry

10.0 g aluminum reacts with 66.5g bromine to form 65.0g aluminum bromide. determine the limiting reactant and calculate the theoretical and percent yield. once the reaction has occured as completely as possible, what mass of the excess reactant is left?