we wish to determine the moles of co₂ produced when 50.0 ml of 2.0 m hcl reacts with excess…

we wish to determine the moles of co₂ produced when 50.0 ml of 2.0 m hcl reacts with excess na₂co₃.\n2hcl(aq) + na₂co₃(aq) → 2nacl(aq) + h₂o(l) + co₂(g)\nin the previous step, you determined 0.10 mol hcl react.\nhow many moles of co₂ form during the reaction?

we wish to determine the moles of co₂ produced when 50.0 ml of 2.0 m hcl reacts with excess na₂co₃.\n2hcl(aq) + na₂co₃(aq) → 2nacl(aq) + h₂o(l) + co₂(g)\nin the previous step, you determined 0.10 mol hcl react.\nhow many moles of co₂ form during the reaction?

Answer

Explanation:

Step1: Calculate moles of HCl

Use the formula $n = M\times V$, where $M$ is molarity and $V$ is volume in liters. Given $V = 50.0\ mL=0.0500\ L$ and $M = 2.0\ M$. $n_{HCl}=2.0\ mol/L\times0.0500\ L = 0.10\ mol$

Step2: Determine mole - ratio

From the balanced chemical equation $2HCl(aq)+Na_{2}CO_{3}(aq)\rightarrow2NaCl(aq)+H_{2}O(l)+CO_{2}(g)$, the mole - ratio of $HCl$ to $CO_{2}$ is $2:1$.

Step3: Calculate moles of $CO_{2}$

Let the moles of $CO_{2}$ be $n_{CO_{2}}$. Using the mole - ratio, $n_{CO_{2}}=\frac{1}{2}n_{HCl}$. Since $n_{HCl} = 0.10\ mol$, then $n_{CO_{2}}=\frac{1}{2}\times0.10\ mol=0.05\ mol$

Answer:

$0.05\ mol$