What mass of carbon dioxide results from combustion of a #52*g# mass of acetylene gas?

Answer 1

We needs a stoichiometric equation, and we finally get a mass of #CO_2# under #200*g#.

And the typical rigmarole is to balance the carbons, and then the hydrogens, and then finally the oxygens.............

#HC-=CH(g) + 5/2O_2(g) rarr 2CO_2(g) +H_2O(l)#

Is this balanced? Don't trust my 'rithmetic!

And thus, moles of acetylene reactant:

#=(52*g)/(26.04*g*mol^-1)=2*mol#
Given the stoichiometry, we gets #4*mol# #CO_2(g)# given complete combustion, a mass of #4*molxx44.0*g*mol^-1=176*g# #"carbon dioxide.........."# Take that atmosphere!

Would this reaction be exothermic? Why or why not?

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Answer 2

The balanced equation for the combustion of acetylene (C2H2) is:

2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(g)

Using the stoichiometry of the equation, we find that for every 2 moles of C2H2 consumed, 4 moles of CO2 are produced.

First, convert the mass of acetylene (C2H2) to moles using its molar mass. Molar mass of C2H2 = 212.01 g/mol + 21.01 g/mol = 26.04 g/mol Number of moles of C2H2 = mass / molar mass = 52 g / 26.04 g/mol = 2 moles

Now, since 2 moles of C2H2 produce 4 moles of CO2, we use this ratio to find the moles of CO2 produced. Moles of CO2 produced = 2 moles C2H2 * (4 moles CO2 / 2 moles C2H2) = 4 moles

Finally, convert moles of CO2 to mass using its molar mass. Molar mass of CO2 = 12.01 g/mol + 2*16.00 g/mol = 44.01 g/mol Mass of CO2 produced = moles * molar mass = 4 moles * 44.01 g/mol = 176.04 g

So, the mass of carbon dioxide resulting from the combustion of a 52 g mass of acetylene gas is 176.04 g.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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