If 7.5 g of carbon is burned completely, what volume of carbon dioxide gas is released at stp?

include work, !

The volume of carbon dioxide produced is 14L

Explanation:

Step 1: Data given

Mass of carbon = 7.5 grams

Molar mass of Carbon = 12 g/mol

STP = 1 mole of any gas occupies 22.4 liters

This means 12 grams of carbon occupies 22.4 liters

Step 2: The equation

C + O2 → CO2

For 1 mole Carbon consumed, we need 1 mole oxygen to produce 1 mole CO2. This is a 1:1 mol ratio.

7.5 grams of carbon will occupy (7.5/12)*22.4L = 14 liters

7.5 g of carbon is burned completely, 14 liters of carbon dioxide are released.

This is because at STP, 1 mole of any gas occupies 22.4 liters of volume and 7.5 grams of carbon is 0.6 mole of carbon. Since carbon produces carbon dioxide in a 1:1 ratio when burned, it means that 0.6 mole of carbon dioxide will be produced.

The volume of carbon dioxide produced is 14L

first, consult an activity series chart to determine if al is more reactive than fe. it is, so it will replace the fe. now, one can continue with the problem.

next, make sure you have a correctly balanced equation.

3feo + 2al ==> 3fe + al2o3

now, determine which reactant (feo or al) is in limiting supply.

moles feo present = 125 g x 1 mole/71.8 g = 1.74 moles

moles al present = 25.0 g x 1 mole/26.98 g = 0.927 moles

since from the balanced equation, it take 3 mol feo for every 2 mol al, al will be limiting.

you can determine this simply by dividing moles of each by their coefficient in the balanced equation. for example: 1.74/3 = 0.58 and 0.927/2 = 0.464. al is less, so it is limiting.

finally, using the stoichiometry in the balanced eq. determine mass of fe that can be produced from 0.927 moles of al.

0.927 moles al x 3 moles fe/2 moles al x 55.8 g/mole = 77.6 g

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !