The reaction of 50 mL of Cl₂gas with 50 mL of CH₄gas via the equation:
Cl₂(g) + CH₄(g) - HCl (g) + CH₃Cl (g)
Will produce a total of mL of products if pressure and temperature are kept constant.

Question

Quizplus · Accepted Answer

According to the balanced chemical equation, the reaction will produce 1 mole of HCl and 1 mole of CHCl3 for every 1 mole of Cl2 and 1 mole of CH4 consumed. Since the volumes are the same for both reactants, we can assume that they have the same number of moles. Therefore, we can calculate the total moles of products formed as follows:

Total moles of products = (moles of HCl) + (moles of CHCl3)
= 1 mole HCl + 1 mole CHCl3
= 2 moles of products

Since we know the total moles of products formed and the volume of each reactant used, we can use the ideal gas law to calculate the volume of products formed:

PV = nRT

Assuming constant pressure and temperature, we can solve for the volume (V):

V = nRT/P

where n is the total moles of products, R is the ideal gas constant, T is the temperature in Kelvin, and P is the pressure.

Since the pressure and temperature are not given in the problem, we cannot calculate the actual volume of products formed. However, we can use the given answer choices to determine the best choice.

- Choice A: 150 mL. This answer assumes that each reactant will produce 75 mL of products, which is not necessarily true since the stoichiometry of the reaction must be considered. Therefore, this choice is not the best option.
- Choice B: 250 mL. This answer assumes that the volume of products formed is equal to the sum of the volumes of the two reactants, which is not correct since the reactants will be consumed during the reaction. Therefore, this choice is not the best option.
- Choice C: 100 mL. This answer assumes that the total volume of products formed is equal to the volume of one of the reactants. Since the stoichiometry of the reaction indicates that 2 moles of products are formed for each mole of reactant, this answer choice is the best option.
- Choice D: 200 mL. This answer assumes that each reactant will produce 100 mL of products, which is not necessarily true since the stoichiometry of the reaction must be considered. Therefore, this choice is not the best option.
- Choice E: 50 mL. This answer assumes that none of the reactants will react, which is not true since the balanced chemical equation indicates that both reactants will be consumed during the reaction. Therefore, this choice is not the best option.

Therefore, the best choice is C.

The Reaction of 50 ML of Cl2 gas with 50

The Reaction of 50 ML of Cl₂gas with 50