Question

Mass (before reaction): test tube + HCl(aq) + stir bar + capsule 26.600 g
Mass (after reaction): test tube + HCl(aq) + stir bar + capsule 25.300 g
Volume of water displaced from the squirt bottle 148 mL
Temperature of the CO2(g) 287.4 K
Pressure (atm) 1.032 atm

Using this data answer each of the questions below. Enter your answer to three significant figures and enter only the numerical value in the answer box.

Calculate the mass of CO2(g).



Calculate the number of moles of CO2(g).



Calculate the density of CO2(g) in g/L.



Calculate the molar mass of CO2 assuming a temperature of 287.4 K.



Calculate the Gas constant, R, in L*atm/K*mol.



Calculate the % error of the value of the Gas constant, R.

Answer 1

Calculate the mass of CO2(g).

<b> I don't know your set up and you didn't explain but it appears mass CO2 is 26.600-25.300 = ?</b>

Calculate the number of moles of CO2(g).

<b>mols = grams/molar mass</b>

Calculate the density of CO2(g) in g/L.

<b>At what temperature? 287.4 K. You have grams and you ave volume.</b>

Calculate the molar mass of CO2 assuming a temperature of 287.4 K.

<b>mols = grams/molar mass. You have mols and grams.</b>

Calculate the Gas constant, R, in L*atm/K*mol.

<b>PV = nRT. Substitute and solve for R.</b>


Calculate the % error of the value of the Gas constant, R.
<b> [(exp value-accepted value)/(accepted value]*100 = ?</b>

Answer 2

Calculate the number of moles of CO2
1.3/44.01+.029 This doesnt work