Question

If 1.0 mole of CH4 and 2.0 moles of Cl2 are used in the reaction CH4 + 4Cl2 => CCl4 + 4HCl then which of these statements is TRUE?

A. All of the CH4 will be used up.
B. The theoretical yield of CCl4 is 1.0 mole.
C. Some Cl2 will be left over.
D. More CH4 should be added to ensure all the Cl2 will be used.
E. The theoretical yield of HCl is 2.0 moles.

Answer 1

In the reaction CH4 + 4Cl2 → CCl4 + 4HCl, some Cl2 will be left over. Hence the correct answer is option C

Step-by-step explanation:

According to the balanced chemical equation, CH4 + 4Cl2 → CCl4 + 4HCl, the stoichiometric ratio between CH4 and Cl2 is 1:4. The question states that 1.0 mole of CH4 and 2.0 moles of Cl2 are used in the reaction. Since the ratio of CH4 to Cl2 is 1:4, the limiting reactant is CH4.

Therefore, statement A is false because not all of the CH4 will be used up. Instead, some Cl2 will be left over, so statement C is true.

Answer 2

B,C,D

Step-by-step explanation:

The yield of CCl4 depends on the amount of CH4 in a 1:1 ratio. The amount of Cl2 is twice that of CH4 hence some must be left over. To ensure that all the Cl2 is used up, more CH4 must added to the system.