16. carbon tetrachloride is a solvent which is used as a refrigerant and also as a cleaning agent. today…

16. carbon tetrachloride is a solvent which is used as a refrigerant and also as a cleaning agent. today, methane and chlorine are mainly used to produce carbon tetrachloride.\n\nch₄ + 4cl₂ → ccl₄ + 4hcl\n\nhow many grams of carbon tetrachloride (ccl₄ - molar mass of 153.82 g/mol) can be produced from reacting 709.0 grams of chlorine (cl₂ - with a molar mass of 70.906 g/mol) with excess methane (ch₄)?\n\n3.845 g\n61.53 g\n384.5 g\n6153 g\nclear all

16. carbon tetrachloride is a solvent which is used as a refrigerant and also as a cleaning agent. today, methane and chlorine are mainly used to produce carbon tetrachloride.\n\nch₄ + 4cl₂ → ccl₄ + 4hcl\n\nhow many grams of carbon tetrachloride (ccl₄ - molar mass of 153.82 g/mol) can be produced from reacting 709.0 grams of chlorine (cl₂ - with a molar mass of 70.906 g/mol) with excess methane (ch₄)?\n\n3.845 g\n61.53 g\n384.5 g\n6153 g\nclear all

Answer

Answer:

615.3 g

Explanation:

Step1: Calculate moles of Cl₂

$n_{Cl_2}=\frac{m_{Cl_2}}{M_{Cl_2}}=\frac{709.0\ g}{70.906\ g/mol}=10\ mol$

Step2: Determine mole - ratio

From the balanced equation $CH_4 + 4Cl_2\rightarrow CCl_4+4HCl$, the mole - ratio of $Cl_2$ to $CCl_4$ is 4:1. So, $n_{CCl_4}=\frac{1}{4}n_{Cl_2}$.

Step3: Calculate moles of CCl₄

$n_{CCl_4}=\frac{1}{4}\times10\ mol = 2.5\ mol$

Step4: Calculate mass of CCl₄

$m_{CCl_4}=n_{CCl_4}\times M_{CCl_4}=2.5\ mol\times153.82\ g/mol = 615.3\ g$