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Given the following data in the Determination of Molar Mass of CO2 lab : Mass (before rxn): test tube HCl(aq) stir bar capsule 26.110 g Mass (after rxn): test tube HCl(aq) stir bar capsule 25.783 g Volume of water displaced from squirt bottle 144 mL Temperature of CO2(g) 293.6 K CO2(g) pressure 0.986 atm Calculate the mass of CO2(g) produced, in grams.

Respuesta :

Answer:

.259 g

Explanation:

PV = nRT

n = PV / RT

= .986 x 0.144 / .082 x 293.6

= .005897 moles

= .005897 x 44 g

= .259 g

The mass of [tex]$CO_2$[/tex]  that is produced in the test tube is 0.327 grams.

Finding out the mass of [tex]$CO_2$[/tex] produced :

It is given that :

  • Weight of the flask before the reaction = 26.110 grams
  • Weight of the flask after the reaction = 25.783 grams

Therefore,

Mass of   [tex]$CO_2$[/tex]  produced is = mass before reaction - mass after reaction

                                            = ( 26.110 - 25.783 ) grams

                                            = 0.327 grams.

                                           

Thus, 0.327 grams of [tex]$CO_2$[/tex] is produced.

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