Question

1.Calculate the mass of CaCO3 that would produce ~ 40.0 ml of CO2 at STP. Hint...

1.Calculate the mass of CaCO3 that would produce ~ 40.0 ml of CO2 at STP.

Hint use molar volume of an ideal gas (22.4 L).

2. The pressure of water vapor at 23 °C is [_____] torr.

3.The difference in mass of the gas generator before and after the reaction takes place yields the mass of CO2 evolved.

true

false

Homework Answers

Answer #1

Q1

CaCO3 + 2HCl = H2O + CO2 + CaCL2

40 mL of CO2 at STP --> 40*10^-4 L

1 mol = 22.4 L at STP

x mol = 40*10^-4 L

x = (40*10^-3)/(22.4) = 0.0017857 mol of CO2

ratio is 1:1 so

0.0017857 mol of CO2 =0.0017857mol of CaCO3

mass = mol*MW= 0.0017857*100 = 0.17857 g of CaCO3 wil do

Q2

23°C the water will have a vapor pressure of --> P = 21.1 torr (from data bases)

Q3

Correct

since only CO2 is being "lost" i.e. the solid/liquyd solutoin remains with CaCO3, CaCl2 and H2O

only CO2(g) goes "out"

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
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...
Calcium carbonate is know to react to form CO2 according to the following reaction: CaCO3 +...
Calcium carbonate is know to react to form CO2 according to the following reaction: CaCO3 + 2H+ → Ca2+ + H2O + CO2 Use the Ideal Gas law to calculate the mass of CaCO3 required to generate 300 torr of pressure at standard temperature in a 50.0 mL flask
If you add 179.0 mL of C3H8 (propane) gas at STP to a 1.00L container, seal...
If you add 179.0 mL of C3H8 (propane) gas at STP to a 1.00L container, seal the container, and combust the gas with 390mL of oxygen. (Molar volume of a gas at STP=22.4L/mol) a) what is the balanced chem. equation for the reaction? b) what is the limiting reagent? what are the theoretical moles of CO2 produced? c) Use daltons law of partial pressure and the ideal gas law to determine the partial pressure of each of the gases when...
1. What is the molar mass of a gas if 0.252 g of the gas occupies...
1. What is the molar mass of a gas if 0.252 g of the gas occupies a volume of 125 mL at a temperature of 123°C and a pressure of 778 torr? 2. A mixture of 0.229 g of H2, 1.08 g of N2, and 0.836 g of Ar is stored in a closed container at STP. Find the volume (in L) of the container, assuming that the gases exhibit ideal behavior.
Using molar volume (stp) or the ideal gas law equation, determine the molar mass , g/mole,...
Using molar volume (stp) or the ideal gas law equation, determine the molar mass , g/mole, of each of the fillowin g. 1- 12.5 g of a gas that has a volume of 2.25 L at stp M = 2- 0.742 g of a gas that has a volume of 835 ml at 1.10 ATM and 19 degrees C. M=
1) 362.11 g of O2 are contained in a 3.00 L high pressure tank at a...
1) 362.11 g of O2 are contained in a 3.00 L high pressure tank at a temperature of 186°C. What is the pressure of the gas in torr? 2) A gas has a given volume. The moles of gas are doubled then the pressure is 1/3 of the original pressure. After the pressure change, the Kelvin temperature quadruples (increases 4 times of the original Kelvin temperature). By how much has the volume changed? Be specific (i.e. the volume is 1/3...
Consider the combustion reaction between 25.0mL of liquid methanol (density=0.850g/mL) and 12.5 L of oxygen gas...
Consider the combustion reaction between 25.0mL of liquid methanol (density=0.850g/mL) and 12.5 L of oxygen gas measured at STP. The products of the reaction are CO2(g) and H2O(g). Calculate the volume of liquid H2O (density= 1g/mL) formed if the reaction goes to completion and you condense the water vapor. *assume that oxygen is an ideal gas*
1. Use the molar volume to calculate each of the following at STP: A.Calculate the number...
1. Use the molar volume to calculate each of the following at STP: A.Calculate the number of moles of CO2 in 1.40 L of CO2 gas. Express your answer to three significant figures and include the appropriate units. B.Calculate the volume, in liters, occupied by 0.200 mol of He gas.Express your answer to three significant figures and include the appropriate units. C.Calculate the volume, in liters, occupied by 4.00 g of O2 gas.Express your answer to three significant figures and...
1. Hydrogen produced in the following reaction is collected over water at 23oC and 742 Torr:...
1. Hydrogen produced in the following reaction is collected over water at 23oC and 742 Torr: 2Al + 6HCl --> 2AlCl3   + 3H2 What volume (mL) of the gas will be collected in the reaction of 1.50 g Al with excess HCl? 2. Sample of O2 gas has a volume of 50.0 L at a pressure of 750. mmHg. What is the final volume, in liters, of the gas at 2.0 atm? 3. What is the mass, in grams, of...
1. Hydrogen produced in the following reaction is collected over water at 23oC and 742 Torr:...
1. Hydrogen produced in the following reaction is collected over water at 23oC and 742 Torr: 2Al + 6HCl --> 2AlCl3 + 3H2 What volume (mL) of the gas will be collected in the reaction of 1.50 g Al with excess HCl? 2. Sample of O2 gas has a volume of 50.0 L at a pressure of 750. mmHg. What is the final volume, in liters, of the gas at 2.0 atm? 3. What is the mass, in grams, of...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT