Question

Elemental phosphorus reacts with chlorine gas according to the equation: P4(s)+6Cl2(g)→4PCl3(l) A reaction mixture initially contains...

Elemental phosphorus reacts with chlorine gas according to the equation: P4(s)+6Cl2(g)→4PCl3(l) A reaction mixture initially contains 45.21 g P4 and 130.4 g Cl2.

Part A Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

Express your answer to three significant figures.

m =

Homework Answers

Answer #1

number of moles of P4 = 45.21g / 123.90 g.mol^-1 = 0.365 mole

number of moles of Cl2 = 130.4g / 70.9060 g.mol^-1 = 1.84 mole

from the balanced equation we can say that

1 mole of P4 requires 6 mole of Cl2 so

0.365 mole of P4 will require

= 0.365 mole of P4*(6 mole of Cl2 /1 mole of P4)

= 2.19 mole of Cl2

but we have 1.84 mole of Cl2 so Cl2 is limiting reactant

P4 is excess reactant

6 mole of Cl2 requires 1 mole of P4 so

1.84 mole of Cl2 will require 0.307 mole of P4

The number of moles of excess reactant = 0.365 - 0.307 = 0.058 mole

mass of excess reactant = 0.058 * 123.90 = 7.19g

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) A reaction mixture initially contains...
Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) A reaction mixture initially contains 22.95 g Fe2O3 and 14.26 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?
Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s)+2HCl(aq)→FeCl2(s)+H2S(g) A reaction mixture initially contains...
Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s)+2HCl(aq)→FeCl2(s)+H2S(g) A reaction mixture initially contains 0.208 mol FeS and 0.678 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant is left?
Phosphorus and chlorine react as follows: P4(s) + Cl2(g) => PCl3(l). Balance it! Assume 135 g...
Phosphorus and chlorine react as follows: P4(s) + Cl2(g) => PCl3(l). Balance it! Assume 135 g P4(s) react with 333 g of Cl2(g). a) What is the limiting reactant? b) What is the reactant in excess and the amount in excess? c) What mass of phosphorus trichloride can be formed from the reaction?
Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2(g)+3F2(g)→2ClF3(g) A 2.45 L reaction vessel,...
Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2(g)+3F2(g)→2ClF3(g) A 2.45 L reaction vessel, initially at 298 K, contains chlorine gas at a partial pressure of 337 mmHg and fluorine gas at a partial pressure of 739 mmHg .Identify the limiting reactant and determine the theoretical yield of ClF3 in grams.
Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2(g)+3F2(g)→2ClF3(g) A 1.90 L reaction vessel,...
Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2(g)+3F2(g)→2ClF3(g) A 1.90 L reaction vessel, initially at 298 K, contains chlorine gas at a partial pressure of 337 mmHg and fluorine gas at a partial pressure of 877 mmHg .
What is the enthalpy change for the first reaction? P4(s) + 6Cl2(g) → 4PCl3(l) ΔH =...
What is the enthalpy change for the first reaction? P4(s) + 6Cl2(g) → 4PCl3(l) ΔH = P4(s) + 10Cl2(g) → 4PCl5(s) ΔH = -1,779.8 PCl3(l) + Cl2 → PCl5(s) ΔH = -123.3 question 2 What is the enthalpy change for the first reaction? Fe2O3(s) → 2Fe(s) + 3/2O2(g) ΔH = 4Fe(s) + 3O2(g) → 2Fe2O3 (s) ΔH = -1,645 kJ Help me understand, please
Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2(g)+3F2(g)→2ClF3(g) A 2.00 L reaction vessel,...
Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2(g)+3F2(g)→2ClF3(g) A 2.00 L reaction vessel, initially at 298 K, contains chlorine gas at a partial pressure of 337 mmHg and fluorine gas at a partial pressure of 784 mmHg . Part A What is the pressure of ClF3 in the reaction vessel after the reaction? Part B What is the total pressure in the reaction vessel after the reaction? So, I've tried this problem, but I end up having...
Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s)+3Cl2(g)→2AlCl3(s) You are...
Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction: 2Al(s)+3Cl2(g)→2AlCl3(s) You are given 26.0 g of aluminum and 31.0 g of chlorine gas. A) If you had excess chlorine, how many moles of of aluminum chloride could be produced from 26.0 g of aluminum? B)If you had excess aluminum, how many moles of aluminum chloride could be produced from 31.0 g of chlorine gas, Cl2?
Consider the reaction between iodine gas and chlorine gas to form iodine monochloride: I2(g)+Cl2(g)⇌2ICl(g)Kp=81.9 (at 298...
Consider the reaction between iodine gas and chlorine gas to form iodine monochloride: I2(g)+Cl2(g)⇌2ICl(g)Kp=81.9 (at 298 K) A reaction mixture at 298 K initially contains PI2=0.35 atm and PCl2=0.35 atm . What is the partial pressure of iodine monochloride when the reaction reaches equilibrium?
Consider the reaction between iodine gas and chlorine gas to form iodine monochloride: I2(g)+Cl2(g)⇌2ICl(g)Kp=81.9 (at 298...
Consider the reaction between iodine gas and chlorine gas to form iodine monochloride: I2(g)+Cl2(g)⇌2ICl(g)Kp=81.9 (at 298 K) A reaction mixture at 298 K initially contains PI2=0.40 atm and PCl2=0.40 atm . What is the partial pressure of iodine monochloride when the reaction reaches equilibrium?