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BlueSky06
Used the Ideal gas law to get the grams of carbon dioxide

PV=nRT  Where p is pressure, v is volume, n is a number of moles, t is temperature and r is the ideal gas constant. The value of R is 0.0821.

Solution
First, find the mole of carbon dioxide

n= PV/RT
  = 1 x 1.0 / 0.081 x (2.73 x 102)
  = 1 / 0.081 x 278.46
  = 1 / 22.56
  = 0.045 mol

Convert the moles into grams
Grams of CO2 = 0.045 mol x 44 g/mol = 1.98 g

So the grams of CO2 is 1.98g
mahima6824soni

The grams of carbon dioxide gas is in a 1.0-l balloon at stp is 1.98 g.

What is the ideal gas law?

It is also known as the general gas equation. It is a hypothetical ideal gas's equation of state.

By the law

PV = nRT

[tex]n= \dfrac{PV}{RT}\\\\n = \dfrac{1 \times 1.0 }{0.081 \times (2.73 \times 102)} \\\\n = \dfrac{1}{0.081 \times 278.46} \\\\n = \dfrac{1}{22.56} = 0.045\; mol[/tex]

Now, convert the moles into grams

moles are multiplied by the molar mass

[tex]0.045 mol \times 44 g/mol = 1.98 g[/tex]

Thus, the grams of carbon dioxide are 1.98 g.

Learn more about ideal gas law

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