If 4.2 g of methane reacts with excess oxygen gas to form carbon dioxide and water in the following chemical equation, how much water is produced in the reaction? CH4(g) + 2O2(g) —-> CO2(g) + 2H2O(g)
A) 9.4 g
B) 4.7 g
C) 4.2 g
D) 3.7 g
Help quick pls!?

1 mol of methane is 16 grams. Therefore, if you have 100 grams of methane, it means that you have

100

16              

=

6.25

moles of methane.

When you burn 6.25 moles of methane, you produce 6.25 moles of carbon dioxide.

When you burn 6.25 moles of methane, you need 12.5 moles of oxygen gas.

When you burn 6.25 moles of methane, you produce 6.25 moles of carbon dioxide (275 grams of

C

O      

2

) and 12.5 moles of water vapour (225 grams of

H

2

O

).

Explanation: I HOPED THAT HELPED

12 is it do you think so

the answer is 0.42 is that is an option. this question provides no info