Question

2C3H7OH + 9O2 -> 6CO2 + 8H2O

Answer 1

Answer:

Up to $18\; \rm mol$ $\rm CO_2$.

Explanation:

The equation for this reaction: $2\; \rm C_3 H_7 OH + 9\; O_2 \to 6\; CO_2 + 8\; H_2O$ is indeed balanced.

Notice that the coefficient of $\rm C_3 H_7 OH$ is $2$ while that of $\rm CO_2$ is $6$.

Therefore, each unit of this reaction would consume $2$ units of $\rm C_3H_7OH$ while producing $6$ units of $\rm CO_2$. In other words, this reaction would produce three times as much $\rm CO_2\!$ as it consumes $\rm C_3H_7OH\!$.

If all that $6\; \rm mol$ of $\rm C_3H_7OH$ molecules are actually consumed through this reaction, three times as many $\rm CO_2$ molecules would be produced. That corresponds to $3 \times 6\; \rm mol = 18\; \rm mol$ of $\rm CO_2\!$ molecules.