# Chemistry

In the reaction: P4 (S) +Cl2 (g)PCl5(s),
1. If you have 10.00 grams of Phosphorus to react with 220 grams of Chlorine
gas, what would be the theoretical yield of PCl5(s), in grams?

2. Why was there condensation of the beaker of cold water when a blue flame
was passes underneath?
(A) the product of carbon dioxide from combustion
(B) the product of hydrogen dioxide from combustion
(C) left over unburned oxygen
(D) left over unburned methane
(E) melting of the glass

3. The reaction of hydrogen peroxide in the presence of manganese dioxide produces:
(A) carbon dioxide
(B) oxygen
(C) hydrogen gas
(D) nitrogen dioxide
(E) methane

4. A 21.18 mL of 0.250 M NaOH is titrated with a H2SO4 solution. The initial volume of H2SO4 was 13.28 and the final volume of H2SO4 was 28.29 mL when the solution turned very slightly pink. What is the concentration of Ca(OH)2?

5. You know the solution forms a precipitate when:
(A) when it changes color
(B) when you can’t see through it
(C) because it bubbles
(D) you have stirred it for more than 5 minutes
(E) the solution thickens

1. 👍 0
2. 👎 0
3. 👁 510
1. 1. Write the equation and balance it.
P4 + 10Cl2 ==> 4PCl5

2a. Convert grams P to moles. mole = grams/molar mass
2b. Convert g Cl2 to mole. Same process.

3a. Using the coefficients in the balanced equation, convert moles P to moles product.
3b. Same procedure, convert moles Cl2 to moles product.
3c. It is likely that moles product from 3a and 3b will not agree which means one of them is wrong. The correct value, in limiting reagent problems, is ALWAYS the smaller one and the reagent producing that value is the limiting regent.

4. Now use the smaller value from 3c and convert to grams. g = moles x molar mass. This is the theoretical yield.

#2. I have no idea what you are talking about in #2.
#3.oxygen
#4. You need to read #3 and make changes. M Ca(OH)2 is zero the way I see it; you didn't start with any.
#5. I don't know what you are doing in the experiment.
#4.

1. 👍 0
2. 👎 0
posted by DrBob222

## Similar Questions

1. ### Chemistry - Answer Check

The two common chlorides of Phosphorus, PCl3 and PCl5, both important in the production of other phosphorous compounds, coexist in equilibrium as shown in the balanced chemical reaction below: PCl3 (g) + Cl2 (g) PCl5 (g) At 250 C,

asked by Anonymous on May 17, 2016
2. ### Chem 2

Phosphorus pentachloride decomposes according to the chemical equation PCl5PCl3 +Cl2 A 0.260 mol sample of PCl5(g) is injected into an empty 2.75 L reaction vessel held at 250 °C. Calculate the concentrations of PCl5(g) and

asked by Anonymous!! on March 31, 2014
3. ### chem sorry the last one did not have the question

A sample of PCl5 weighing 2.69 grams is placed in a 1.000 liter flask and vaporized completely at 250 o C. The final pressure observed at this temperature is 1.000 atmospheres. Note that some, but not all of the PCl5 decomposes

asked by laura on December 6, 2011
4. ### chem

A sample of PCl5 weighing 2.69 grams is placed in a 1.000 liter flask and vaporized completely at 250 o C. The final pressure observed at this temperature is 1.000 atmospheres. Note that some, but not all of the PCl5 decomposes

asked by laura on December 5, 2011
5. ### Chemistry

Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) ⇌ PCl3(g) + Cl2(g) A 0.304 mol sample of PCl5(g) is injected into an empty 4.75 L reaction vessel held at 250 °C. Calculate the concentrations of

asked by Dee on April 2, 2013
6. ### Chemistry

Phosphorus pentachloride decomposes according to the chemical equation: PCl5(g) PCl3(g)+Cl2(g) Kc = 1.80 at 250 degrees Celsius A 0.352 mol sample of PCl5(g) is injected into an empty 4.45 L reaction vessel held at 250 °C.

asked by Laura on March 8, 2013
7. ### Chemistry

When a sample of PCl5(g) (0.02087 mol/L) is placed in 83.00 L reaction vessel at 491.0 °C and allowed to come to equilibrium the mixture contains 103.0 grams of PCl3(g). What is the equilibrium concentration (mol/L) of Cl2(g)?

asked by Drew on April 15, 2010
8. ### Chemistry

Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) PCl3(g)+Cl2(g) Kc=1.80 at 250 degrees Celsius A 0.222 mol sample of PCl5(g) is injected into an empty 3.25 L reaction vessel held at 250 °C. Calculate

asked by J on March 3, 2013
9. ### Chemistry

Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) -----> PCl3 (g)+ Cl2(g) Kc= 1.80 at 250 degrees C A 0.206 mol sample of PCl5(g) is injected into an empty 3.30 L reaction vessel held at 250 °C.

asked by Katherine on September 30, 2013
10. ### chemistry

Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) -----> PCl3 (g)+ Cl2(g) Kc= 1.80 at 250 degrees C A 0.463 mol sample of PCl5(g) is injected into an empty 4.80 L reaction vessel held at 250 °C.

asked by Sarah on March 9, 2012
11. ### chemistry equilibriums

At a certain temperature, 2.00 moles of phosphorus(V) chloride, PCl5, was placed in a 1.0 L vessel and permitted to react as shown: PCl5 (g) PCl3 (g) + Cl2(g) At equilibrium, the container held 0.40 PCl5. What is the numerical

asked by chem on December 29, 2010

More Similar Questions