'C according to the unbalanced equation below 75.5 g of solid CaO is reacted with 50.0 g 5) Determine the mass of the e...

Question

Question

C according to the unbalanced equation below 75.5 g of solid CaO is reacted with 50.0 g 5) Determine the mass of the excess

science chemistry

Answer 1

Answer #1

balanced equation is

2CaO + 5C ------------>2 CaC2 + CO2

75.5g/56g/mol 50g/12g/mol 0 0 intital moles

=1.348 =4.167

To know the limiting reagent , let us calculate the ratio of given to required moles

1.348/2= 0.674 4.167/5=0.833

Thus CaO is limiting reagent and C is excess reactant

Thus after reaction

2CaO + 5C ------------> 2 CaC2 + CO2

75.5g/56g/mol 50g/12g/mol 0 0 intital moles

=1.348 =4.167

0 4.167- ( 1.348x5/2)=2.482 1.348 0.674 after reaction

thus the excess reactant (carbn) remaining = 2.482 moles

mass remaining of Carbon = molesx molar mass= 2.482 mol x 12g/mol =29.784 g

Answer 2

Similar Homework Help Questions

Chlorine gas reacts with phosphorus to produce phosphorus pentachloride as shown in the chemical equation below. What i...

Chlorine gas reacts with phosphorus to produce phosphorus pentachloride as shown in the chemical equation below. What is the maximum number of grams of PCls are produced from 3.5 g of Cl2 and excess P? 5C12(g) + 2P(s) → 2PC13(s) 2) What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr2O3 with 8.00 g of aluminum according to the unbalanced chemical equation below? Al(s) + Cr2O3(s) → Al2O3(s) + Cr(s) Ammonia...
8.0 g of iron is reacted with 8.0 g of water according to the chemical equation...

8.0 g of iron is reacted with 8.0 g of water according to the chemical equation shown below. Which one of the following statements is false? 3 Fe(s) + 4 H2O(l) → Fe3O4(s) + 4 H2(g) 11.1 g of Fe3O4 are produced. Mass is conserved in this reaction. Water is the limiting reactant. 4.56 g of H2O are left over.
5.0g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the...

5.0g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below. Which one of the following statements is false? N2 (g) + 3 H2 (g) > 2 NH3 (g) A) 2.8 grams of hydrogen are left over. B) Nitrogen is the limiting reactant C) The theoretical yield of ammonia is 6.1 g D) Hydrogen is the excess reactant

If 20 g of Na2SO4 is reacted with 20 g of Al(NO3)3 according to the following...

If 20 g of Na2SO4 is reacted with 20 g of Al(NO3)3 according to the following equation: 3 Na2SO4 + 2 Al(NO3)3 --> Al2(SO4)3 + 6 NaNO3 How many grams of the excess reactant will remain after the reaction, assuming that all of the limiting reactant reacts to form the products?
any help? thanks EXAM #2 2. 20.0 g of AlzS3 and 20.0 g of H20 are reacted according to the following reaction: Al S...

any help? thanks EXAM #2 2. 20.0 g of AlzS3 and 20.0 g of H20 are reacted according to the following reaction: Al S; (s) + 6H20 (1) ► 2 Al(OH)3 (s) + 3 H2S (g) A. Determine the percent yield of the reaction if 17.5g Al(OH)3 are actually produced in this reaction. (8 pts) B. What mass of the excess reactant remains unused after the reaction in complete? (Bonus = 4 points)
Professor Edixordyh conducted an experiment in her laboratory. She reacted 25.0 g of solid cobalt(III) carbonate wi...

Professor Edixordyh conducted an experiment in her laboratory. She reacted 25.0 g of solid cobalt(III) carbonate with 50.0 cm2 of 2.00 mol dm dilute nitric acid. (a) Write a balanced chemical equation, including state symbols, for the reaction. (b) Write an ionic equation for the reaction. (c) Determine if there is any excess reagent and if yes, calculate the amount of excess reagent. (d) Draw a fully labelled diagram to illustrate the method which Professor Edixordyh.can Use to remove any...

Ammonia is produced by the reaction of nitrogen and hydrogen according to the equation N2(g) + 3H2(g) → 2NH3(g) Calculat...

Ammonia is produced by the reaction of nitrogen and hydrogen according to the equation N2(g) + 3H2(g) → 2NH3(g) Calculate the mass of ammonia produced when 32.0 g of nitrogen react with 13.5 g of hydrogen. ___________NH3 Which is the excess reactant and how much of it will be left over when the reaction is complete? hydrogen or nitrogen ________ g
A 2.00 g sample of silver nitrate is dissolved in water and then reacted with 0.250...

A 2.00 g sample of silver nitrate is dissolved in water and then reacted with 0.250 g of copper metal, according to the reaction below. Answer the questions about this process. 2 AgNO3 (aq) + Cu (s) --> Cu(NO3)2 (aq) + 2 Ag (s) What mass of the excess reactant remains after the reaction goes to completion? (I want to see if you guys get this correct because I have no idea how to approach because it doesn't tell us...
Consider the unbalanced chemical equation below. CaSiO3(-) + HF (@)-CaF2(aq) + SiF4(g) + H2O(1) Suppose a...

Consider the unbalanced chemical equation below. CaSiO3(-) + HF (@)-CaF2(aq) + SiF4(g) + H2O(1) Suppose a 34.3 g sample of CaSiO3 is reacted with 31.3 L of HF at 27.0 °C and 1,00 atm. Assuming the reaction goes to completion calculate the mass (in grams) of the SiF4 and H2O produced in the reaction. mass SiF4 = mass H2O Submit Hide Hints

Consider the equation 2KOH + H2SO4 → K2SO4 + 2H20 a lf 25 g H2SO4 is...

Consider the equation 2KOH + H2SO4 → K2SO4 + 2H20 a lf 25 g H2SO4 is reacted with 7.7 g KOH, how many grams of K2SO4 are produced? b For part a of this problem, identify the limiting reactant and calculate the mass of excess reactant that remains after the reaction is completed. c Calculate the theoretical yield of the reaction. How many grams of material would you expect to obtain if the reaction has a 67.1% yield?