Given the equation $C_2H_6(g) + O_2(g) -> CO_2 (g) + H_2O(g)$ (not balanced), what is the number of liters of $CO_2$ formed at STP when 240.0 grams of $C_2H_6$ is burned in excess oxygen gas?

Md Ariful Islam

0 like 0 dislike
1 views
Share with your friends

1 Answers

Md Ariful Islam

Call

The first thing to do here is make sure that you have a balanced chemical equation. The equation given to you is actually unbalanced, so focus on writing a balanced version

$color(red)(2)"C"_2"H"_text(6(g]) + 7"O"_text(2(g]) -> color(purple)(4)"CO"_text(2(g]) + 6"H"_2"O"_text((g])$

Now, the problem provides you with a mass of ethane, $"C"_2"H"_6$, and asks for the volume of carbon dioxide, $"CO"_2$, formed by the reaction at STP, Standard Temperature and Pressure.

As you know, STP conditions are defined as a temperature of $0^@"C"$ and a pressure of $"100 kPa"$. Under these specific conditions, one mole of any ideal gas occupies exactly $"22.7 L"$ - this is known as the .

So, what this means is that if you know how many moles of carbon dioxide are produced by the reaction, you can use the molar volume of the gas to find the requested volume.

Use the molar mass of ethane to determine how many moles you'd get in that $"240.0-g"$ sample

$240.0 color(red)(cancel(color(black)("g"))) * ("1 mole C"_2"H"_6)/(30.07color(red)(cancel(color(black)("g")))) = "7.9814 moles C"_2"H"_6$

Now, notice that you have a $color(red)(2):color(purple)(4)$ mole ratio between ethane and carbon dioxide. Since ethane reacts with excess oxygen, you can assume that all the moles will take part in the reaction.

This means that the reaction will produce

$7.9814 color(red)(cancel(color(black)("moles C"_2"H"_6))) * (color(purple)(4)" moles CO"_2)/(color(red)(2)color(red)(cancel(color(black)("moles C"_2"H"_6)))) = "15.9628 moles CO"_2$

So, if one mole of any ideal gas occupies $"22.7 L"$ at STP, this many moles will occupy

$15.9628color(red)(cancel(color(black)("moles CO"_2))) * "22.7 L"/(1color(red)(cancel(color(black)("mole CO"_2)))) = color(green)("362.4 L")$

The answer is rounded to four , the number of sig figs you have for the mass of ethane.

0 like 0 dislike
1 views
Talk Doctor Online in Bissoy App
How would you balance this equation: $C_2H_6+O_2 -> CO_2+H_2O$?

$"C"_2"H"_6" + O"_2$$rarr$$"CO"_2" + H"_2"O"$ Balance H first. There are 6 H atoms on the left and 2 on the right. Place a coefficient of 3 in front of the...

1 Answers 1 views
When the equation $C_2H_4+O_2 -> CO_2+H_2O$ is balanced using smallest whole numbers, what is the coefficient of the $O_2$?

The answer is $3$. Is this balanced? For every reactant particle, is there a corresponding product particle? There are $2C$ reactant particles, and $2C$ product particles. You have to count...

1 Answers 1 views
Water can be formed from the stoichiometric reaction of hydrogen with oxygen: $2H_2(g) + O_2(g) + 2H_2O(g)$. A complete reaction of 5.0 g of $O_2$ with excess hydrogen produces how many grams of $H_2O$?

$2H_2(g) + O_2(g) rarr 2H_2O(g)$ We started with $(5.0*g)/(32.00*g*mol^-1)=0.156*mol" dioxygen"$. Given excess dihydrogen, this molar quantity thus gives $2xx0.156*mol$ water. And thus, $2xx0.156*molxx18.01*g*mol^-1~=6*g$ water are evolved. Is this reaction exothermic...

1 Answers 1 views
)A compound that contains just C, H and N is burned in oxygen. When 5.000 g of the compound is burned in excess oxygen, 6.019 g of $CO_2$, 4.313 g of $H_2O$, and 9.438g of $NO_2$ are the only products. What is the empirical formula of the compound?

We must calculate the masses of $"C, H"$, and $"N"$ from the masses of carbon dioxide, water, and nitrogen dioxide. $"Mass of C" = 6.019 color(red)(cancel(color(black)("g CO"_2))) × "12.01 g...

1 Answers 1 views
Hm many grams of $CO_2$ would be formed from 30 grams of $C_7H_8$ in the following reaction $C_7H_8 + O_2 -> CO_2 + H_2O$?

A balanced equation representing the complete combustion of toluene is absolutely necessary: $C_7H_8 + 9O_2 rarr 7CO_2 + 4H_2O$ This tells us that for every mole of toluene, 7 moles...

1 Answers 1 views
If 5.49 mol of ethane ($C_2H_6$) undergoes combustion according to the unbalanced equation $C_2H_6+O_2->CO_2+H_2O$, how much oxygen is required?

The balanced equation of the combustion of ethane is: $2C_2H_6+7O_2->4CO_2+6H_2O$ Then number of mole of oxygen that will be needed to completely react with $5.49mol$ of ethane could be calculated...

1 Answers 1 views
$2CO(g) + O_2(g) -> 2CO_2(g)$. How many liters of $O_2$ will react with 74.2 liters of CO? If 6.5 g of CO react, how many liters of $CO_2$ are produced?

We calculate the relative quantities from the molar ratios in the balanced reaction equation. $2CO(g)+O_2(g)→2CO_2(g)$. As a pretty good approximation, gas volumes are proportional to molar amounts. Therefore with...

1 Answers 1 views
For $CH_4 +2O_2 -> CO_2 + 2H_2O$, the molar mass of oxygen gas ($0_2$) is 32.00 g/mol. The molar mass of carbon dioxide ($CO_2$) is 44.01 g/mol. What mass of $CO_2$, in grams, will form when 8.94 g $O_2$ completely react?

The balanced chemical equation tells us unequivocally that 16 g of methane gas reacts with 32 g of dioxygen gas to give 44 g of carbon dioxide, and 36 g...

1 Answers 1 views
What is the limiting reagent and the moles of $CO_2$ formed when 11 moles $CS_2$ reacts with 18 moles $O_2$ to produce $CO_2$ gas and $SO_2$ gas at STP?

Limiting reagent problems are all about using the that exists between the reactants to determine if you have enough of each reactant to allow for their complete consumption....

1 Answers 1 views
Limiting reagent problem? For the reaction $C_2H_6+O_2 to CO_2+H_2O$

Balanced Eqn $2C_2H_6 +7O_2 =4 CO_2+6H_2O$ By the Balanced eqn 60g ethane requires 7x32= 224g oxygen here ethane is in excess.oxygen will be fully consumed hence 300g oxygen will...

1 Answers 1 views
X