13.How many grams of phosphorus (P4) are needed to completely consume 79.2 L of chlorine gas according to the following reaction
1 answer:
Answer:
73.2g
Explanation:
The reaction expression is given as:
P₄ + 6Cl₂ → 4PCl₃
Given parameters:
Volume of chlorine gas = 79.2L
Unknown:
Mass of Phosphorus needed = ?
Solution:
To solve this problem, let us find the number of moles of the chlorine gas.
Since the condition of the reaction is at STP;
22.4L of gas is contained in 1 mole
79.2L of chlorine gas will contain = 3.54mole
From the reaction expression;
6 moles of chlorine gas will react with 1 mole of P₄
3.54 mole of chlorine gas will completely react with = 0.59mole of P₄
Mass of P₄ = number of moles x molar mass
Molar mass of P₄ = 4 x 31 = 124g/mol
Mass of P₄ = 0.59 x 124 = 73.2g
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<u>Answer: </u>The volume of the solution is 85.7 mL
<u>Explanation:</u>
Molarity is defined as the amount of solute expressed in the number of moles present per liter of solution. The units of molarity are mol/L. The formula used to calculate molarity:
.....(1)
We are given:
Molarity of solution = 0.600 M
Given mass of = 12.00 g
We know, molar mass of
Putting values in equation 1, we get:
The rule of significant number that is applied for the problems having multiplication and division:
The least number of significant figures in any number of the problem determines the number of significant figures in the answer.
Here, the least number of significant figures is 3 that is determined by the number, 0.600. Thus, the answer must have these many significant figures only.
Hence, the volume of the solution is 85.7 mL