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5. If 20 grams of C₂H, reacts with 2 moles of O; how many grams of CO, can be made?​

User EmilDo
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Answer:

The mass of CO2 produced from 20 grams of C2H2 is approximately 67.61 grams.

Step-by-step explanation:

The balanced equation for the combustion of C2H2 with O2 to produce CO2 and H2O is:

C2H2 + 2O2 → 2CO2 + H2O

From the balanced equation, we can see that the stoichiometric ratio of C2H2 to CO2 is 1:2. This means that for every 1 mole of C2H2 that reacts, 2 moles of CO2 are produced.

To determine the mass of CO2 produced from 20 grams of C2H2, we first need to calculate the number of moles of C2H2:

n(C2H2) = m/M

where:

m = mass of C2H2 (20 g)

M = molar mass of C2H2 (2 x 12.01 g/mol + 2 x 1.01 g/mol = 26.04 g/mol)

n(C2H2) = 20 g / 26.04 g/mol

n(C2H2) = 0.7686 mol

Since the stoichiometric ratio of C2H2 to CO2 is 1:2, the number of moles of CO2 produced is twice the number of moles of C2H2:

n(CO2) = 2 x n(C2H2)

n(CO2) = 2 x 0.7686 mol

n(CO2) = 1.5372 mol

Now, we can calculate the mass of CO2 produced:

m(CO2) = n x M

where:

n = number of moles of CO2 (1.5372 mol)

M = molar mass of CO2 (12.01 g/mol + 2 x 16.00 g/mol = 44.01 g/mol)

m(CO2) = 1.5372 mol x 44.01 g/mol

m(CO2) = 67.61 g

Therefore, the mass of CO2 produced from 20 grams of C2H2 is approximately 67.61 grams (to two decimal places).

User Luca Burgazzoli
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