# chemistry 101

Consider the following reaction. CaO (s) + CO2 (g) = CaCO3 (s) A chemist allows 14.4 g of CaO and 13.8 g of CO2 to react. When the reaction is finished, the chemist collects 19.4 g of CaCO3. Determine the limiting reactant, theoretical yield, and percent yield for the reactio
options:
CaO; 32 g CaCO3; 60.6%
CaCO3; 25.7 g CaO; 45.5%
CaCO3; 67.2 g CaO; 28.9%
CaO; 25.7 g CaCO3; 75.5%
CaO; 15.0 g CaCO3; 129%

1. 👍 0
2. 👎 0
3. 👁 1,450
1. Limiting reagent problem, I think, are easiest to do if you do TWO simple stoichiometry problems. The first time you use CaO and determine moles CaCO3 produced. The second time use 13.8 g CO2 and determine moles CaCO3 produced. The correct answer, in limiting reagent problems, is ALWAYS the smaller value and the reagent producing that smaller value is the limiting reagent. That value of CaCO3 produced will be the theoretical yield.
percent yield = (actual yield/theoretical yield)*100 = ??
(note: actual yield is 19.4 g from the problem.).

1. 👍 0
2. 👎 0
posted by DrBob222
2. afgs

1. 👍 0
2. 👎 0

## Similar Questions

The equilibrium constant, Kc for the system, CaO(s) + CO2(g) == CaCO3(s), is A. Kc = (CaO) (CO2) / (CaCO3) B. Kc = (CO2) C. Kc = (CaCO3)/(CaO) D. Kc = (CaCO3) / (CaO) (CO2) E. Kc = 1 / (CO2) My answer is (CaCo3) / (CaO)(CO2).

asked by Hannah on March 3, 2012

For the system CaO(s) + CO2(g) = CaCO3(s), I added 1.00 mol of CaO(s) to 1.00L of 0.500M CO2(g) at 200 oC. At equilibrium the [CO2] = 0.150M. What is the value of Kp for this reaction? Kp would = CaCO3/(CaO)(CO2) I do not know

asked by Hannah on March 14, 2012
3. ### chem, predicting direction of change in entropy

Predict the direction of the entropy in each reaction. a. CaCO3(s)-> CaO(s) +CO2(g0 b. NH3(g)+HCl(g)->NH4Cl(s) c. 2NaHCO3-> Na2CO3(s)+H20(g) +CO2 d. CaO(s)+CO2(g)-> CaCO3

asked by bkue on May 17, 2012
4. ### Science

Consider the following reaction: CaCO3 - CaO + CO2 Calcium carbonate (CaCO3) was heated to yield CaO and CO2. If 60.0g of CaCo3 was heated and the yield for CaO was 44.6%, calculate the mass of CaO created.

asked by Nasa on November 12, 2015
5. ### Chemistry

CaCO3(s) CaO(s) + CO2(g) What would happen if CO2 was removed? Would the reaction shift left? Does that mean CaCO3 increases and CaO and CO2 decrease ?

asked by scilover on May 15, 2013
6. ### Chemistry

Quicklime (CaO) can be prepared by roasting limestone (CaCO3) according to the reaction CaCO3(s)  −!CaO(s) + CO2(g) . When 2.6 ×10^3 g of CaCO3 are heated, the actual yield of CaO is 1.06 ×10^3 g. What is the percent yield?

asked by Jack on March 23, 2011
7. ### chemistry

Calculate the temperature (K) at which the equation as written is at equilibrium. Express your answer to three significant figures. CaO(s) + CO2(g) → CaCO3(s) ∆G°f (kJ/mol) CaO(s)-604.0 CO2(g)-394.4 CaCO3(s)-1128.8 ∆H°f

asked by Penny on March 11, 2013
8. ### Chemistry

1. The value of ΔH° for the reaction below is -6535 kJ. _________ kJ of heat are released in the combustion of 16.0 g C6H6 (l). 2C6H6 (l) + 15O2 (g) --> 12CO2 (g) + 6H20 (l) 3. Given the following reactions CaCO3 (s) --> CaO (s)

asked by Jess on October 31, 2017
9. ### Chemistry(Please respond, thank you!)

For the system CaO(s) + CO2(g) = CaCO3(s), I added 1.00 mol of CaO(s) to 1.00L of 0.500M CO2(g) at 200 oC. At equilibrium the [CO2] = 0.150M. What is the value of Kp for this reaction? Kp would = CaCO3/(CaO)(CO2) I do not know

asked by Hannah on March 15, 2012
10. ### college chemistry

Calcium oxide (CaO), an important ingredient in cement, is produced by decomposing calcium carbonate (CaCO3) at high temperature: CaCO3(s) → CaO(s) + CO2(g) In one particular reaction, 40 g of CaCO3 is heated at 750°C in a 5.0

asked by Liz on February 8, 2011

More Similar Questions