Multiple Choice 1 point How many moles of oxygen gas (O_(2)) is needed to produce 18.0 liters of CO_(2) at STP? CH_(4(g))+2O_(2(g))arrow CO_(2(g))+2H_(2)O_((l))

Question

Answer 1

1.608 moles of

Answer 2

## Step 1: Identify the balanced chemical equation for the reaction. The given equation is already balanced:

## Step 2:Determine the mole ratio between

and

from the balanced equation. According to the equation, 1 mole of

is produced from 2 moles of

.## Step 3:Use the ideal gas law at STP (Standard Temperature and Pressure) to find the number of moles of

. At STP, 1 mole of any gas occupies 22.4 liters. Therefore, 18.0 liters of

corresponds to:

## Step 4:Calculate the moles of

needed using the mole ratio from Step 2. Since 1 mole of

requires 2 moles of

, 0.804 moles of

will require:

Problemas