Question

how many liters of H2O is produced by tge complete combustion of 2.00 mol of C4H10 assuming STP conditions

Answer 1

Combustion of Butane can be signified with following reaction :

$2C_4H_{10}(g) +13 O_2(g)\to 8CO_2(g)+10H_2O(g)$

As evident from the above balanced reaction,

2 moles of $C_4H_{10}$ reacts to form $10$ moles of $H_2O$ at STP.

1 mole of gas occupies $22.4\ L$ of volume.

So, $10$ moles of $H_2O$ will occupy $22.4\times 10=224\ L$ of volume.