given the following:

mass (before reaction) test tube +HCL + stir bar +capsule = 26.042g

mass (after reation) test tube + HCL + stir bar + capsule 25.783g

volume of water displaced from squirt bottle 144mL

temperature of CO2 (g) 293.6 K

CO2 (g) pressure = 0.986 tm

Calculate the :

mass of CO2 (g)

moles of CO2 (g)

-density of CO2 g/L

- molar mass of CO2 (g) assuming a temperature of 293.6K

## Answers (1)

a] - mass of CO2 (g) = 26.042 - 25.783g

b] moles of CO2 (g) divide answer a]by molar mass of CO2 (44g)

c]-density of CO2 g/L

density = mass/volume

mass = answer a]

volume in L = 0.144

d] - molar mass of CO2 (g) assuming a temperature of 293.6K

use P1V1/T1 = P2V2/T2 to find volume at STP [remember to convert degrees C --> K by adding 273.

find V2

V2 L weigh [answer a]

scale to quantity you want by simple proportion maths.

so 22.4L [1 mole at STP] weigh A/V2 x 22.4g

Reference:rtc