Question

What mass of oxygen is needed for the complete combustion of 4.60×10−3g of methane?

Answer 1

first you should start with a chenmical equation for the combustion

Answer 2

do you know the chemical formula of oxygen and methane?

Answer 3

yea, 02 and CH4

Answer 4

that's right.

do you know what products will be formed in a complete combustion?

Answer 5

mass of O2= 7.20x10^-3g Ch4( 1mol/16.042g) x( 2 mol O2/ 1molCh4) x(32.00g/1mol O2)=0.0287g

Answer 6

got this from an earlier problem, but the only diference is the 7.20 #

Answer 7

well in this case the mass is 4.6 milligrams instead of 7.2 milligrams

Answer 8

do you know how they arrived at 0.0287g?

Answer 9

Yeah you have the working above

Answer 10

The proper way to do this is finish the combustion equation

so far we have

\[\text O_2+\text{CH}_4\longrightarrow\]

Answer 11

can you tell me what products form in a complete combustion reaction

Answer 12

you mean from oxygen and methane?

Answer 13

what do you get when you burn all the methane in the oxygen ,
what is left?

Answer 14

we get just o2

Answer 15

all of the atoms in the products should be the same as the atom in the reactants,

however, they molecules will have changed

Answer 16

yea, reactant should equal products after chemical reaction

Answer 17

What are the products ?

Answer 18

carbon dioxide and water

Answer 19

That's right!

Answer 20

so the (unballanced) reaction is\[\text O_2+\text{CH}_4\longrightarrow \text{CO}_2+\text H_2\text O\]

Answer 21

Can you ballance the equation so that the number of atoms of each element is the same on both sides of the equation ?

Answer 22

The C is already balanced, balance the H , then O