if 6.00 g of carbon is burned completely, what volume of carbon dioxide gas is released at stp?\n6.0 l\n11.2…

Explanation:

Step1: Calculate moles of carbon

The molar mass of carbon (C) is 12.01 g/mol. The number of moles of carbon $n_{C}=\frac{m}{M}$, where $m = 6.00$ g and $M=12.01$ g/mol. So $n_{C}=\frac{6.00\ g}{12.01\ g/mol}\approx0.5$ mol.

Step2: Determine moles of carbon - dioxide

The chemical equation for the complete combustion of carbon is $C + O_{2}\rightarrow CO_{2}$. From the equation, the mole - ratio of $C$ to $CO_{2}$ is 1:1. So, if $n_{C}=0.5$ mol, then $n_{CO_{2}} = 0.5$ mol.

Step3: Calculate volume of carbon - dioxide at STP

At STP (Standard Temperature and Pressure, $T = 273$ K and $P= 1$ atm), the molar volume of any ideal gas is $V_{m}=22.4$ L/mol. The volume of $CO_{2}$, $V=n_{CO_{2}}\times V_{m}$. Substituting $n_{CO_{2}} = 0.5$ mol and $V_{m}=22.4$ L/mol, we get $V = 0.5\ mol\times22.4\ L/mol=11.2$ L.

Answer:

11.2 L