Question

A 1.719 g sample of CaCO3 mixture is thermally decomposed, producing CaO(s) and CO2(g). After the...

A 1.719 g sample of CaCO3 mixture is thermally decomposed, producing CaO(s) and CO2(g). After the reaction, the mixture has a mass of 1.048g. How many moles of CO2 are evolved? (Your answer should be in moles, just enter your numeric answer, without the unit of measure.)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
4.430g mixture containing CaCO3 (s) is heated until all CaCO3 (s) is decomposed completly. CaCO3 (s)...
4.430g mixture containing CaCO3 (s) is heated until all CaCO3 (s) is decomposed completly. CaCO3 (s) >>>> CaO (s) + CO2 (g) (Molar mass: CaCO3= 100.0g/mol CaO= 56.1g/mol CO2= 44.0g/mol) If the mass of the mixture remaining after heating is 3.580g, calculate the percent CaCO3 in the mixture from the mass loss of the sample.
Constants | Periodic Table A 3.80 −g sample of a mixture of CaO and BaO is...
Constants | Periodic Table A 3.80 −g sample of a mixture of CaO and BaO is placed in a 1.00-L vessel containing CO2 gas at a pressure of 735 torr and a temperature of 26 ∘C. The CO2 reacts with the CaO and BaO, forming CaCO3 and BaCO3. When the reaction is complete, the pressure of the remaining CO2 is 155 torr . Part A Calculate the number of moles of CO2 that have reacted. n =    mol   Part...
For the reaction below, Kp = 1.16 at 800.°C. CaCO3(s) equilibrium reaction arrow CaO(s) + CO2(g)...
For the reaction below, Kp = 1.16 at 800.°C. CaCO3(s) equilibrium reaction arrow CaO(s) + CO2(g) If a 25.0-g sample of CaCO3 is put into a 13.3 L container and heated to 800°C, what percentage by mass of the CaCO3 will react to reach equilibrium?
Consider the following thermochemical equation: CaCO3(s) CaO(s) + CO2 Ho = +178 kJ a) How many...
Consider the following thermochemical equation: CaCO3(s) CaO(s) + CO2 Ho = +178 kJ a) How many moles of CaCO3 are in 12.0g of CaCO3? moles b) How much heat must be absorbed by 12.0 g of CaCO3 to convert it completely to CaO? kJ
When solid CaCO3 is heated, it decomposes to give solid CaO and CO2 gas. A volume...
When solid CaCO3 is heated, it decomposes to give solid CaO and CO2 gas. A volume of 560 mL of gas is collected over water at a total pressure of 730 mmHg and 16 ∘C. The vapor pressure of water at 16 ∘C is 14 mmHg. CaCO3(s)→CaO(s)+CO2(g) 1)How many moles of CO2 gas were in the CO2 gas sample? Express your answer with the appropriate units
The equilibrium reaction CaCO3(s) ↔ CaO(s) + CO2(g) reaches ΔG° = 0 at 835°C. At this...
The equilibrium reaction CaCO3(s) ↔ CaO(s) + CO2(g) reaches ΔG° = 0 at 835°C. At this temperature: the pressure of CO2 is 1 atm the percent yield of CaO reaches 100% ΔH° = ΔS° the decomposition of CaCO3 begins the reaction becomes exothermic
Consider the following reaction between calcium oxide and carbon dioxide: CaO(s)+CO2(g)→CaCO3(s) A chemist allows 14.4 g...
Consider the following reaction between calcium oxide and carbon dioxide: 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 20.7 g of CaCO3. --->Determine the theoretical yield for the reaction. --->Determine the percent yield for the reaction. --->Determine the limiting reactant for the reaction.
A .276g sample of a CoCO3 heterogenous mixture was placed into a gas generator, the total...
A .276g sample of a CoCO3 heterogenous mixture was placed into a gas generator, the total mass which is 87.719g (containing the CaCO3 sample and the beaker, an HCl solution, and the test tubes) is connected to a gas collection appartus. The following data were collected following the reaction Volume of wet CO2: 37/7 mL Temperature of wet CO2: 20.0 degrees celcius Pressure of wet CO2: 770 Torr Mass of gas generator after reactionL 87.642g Answer parts A-G and show...
A sample of limestone and other soil materials was heated, and the limestone decomposed to give...
A sample of limestone and other soil materials was heated, and the limestone decomposed to give calcium oxide and carbon dioxide. CaCO3(s) → CaO(s) + CO2(g) A 6.498 g sample of limestone-containing material gave 2.44 g of CO2, in addition to CaO, after being heated at a high temperature. What was the mass percent of CaCO3 in the original sample? ___%
Given the following reaction: heat + CaCO3(s) <----> CaO(s) + CO2(g) a. In which direction, if...
Given the following reaction: heat + CaCO3(s) <----> CaO(s) + CO2(g) a. In which direction, if any, will the equilibrium shift when the pressure of CO2 is increased? b. In which direction, if any, will the equilibrium shift if the temperature is decreased? c. In which direction, if any, will the equilibrium shift if the amount of CaCO3 is increased?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT