Question

1. Gaseous phosphorus trifluoride is prepared by the reaction of phosphine and fluorine: 4 PH_3 (g)...

1. Gaseous phosphorus trifluoride is prepared by the reaction of phosphine and fluorine: 4 PH_3 (g) + 3 F_2 (g) --> 3 PH_4F (s) + PF_3 (g) If you mix PH_3 and F_2 in the correct stoichiometric ratio, and if the total pressure of the mixture is 0.2 atm, then what is the final total pressure in the flask? (Assume T is constant and the reactants have been completely consumed)

a) 0.029 atm

b) 0.114 atm

c) 0.200 atm

d) 1 atm

e) Not enough information

2. A flask is first evacuated so that it contains no gas at all. Then 4.4 g of carbon dioxide is introduced into the flask. On warming to 22 degrees C, the gas exerts a pressure of 0.242 atm. What is the volume of the flask? C: 12.01 g/mol; O: 16.0 g/mol; R = 0.0821 L*atm/mol*K

a) 27 L

b) 4.93 L

c) 0.34 L

d) 1.25 L

e) 10 L

Homework Answers

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
A.Calculate ΔS°(universe) for the decomposition of 1 mol of gaseous phosphine (PH3) to form white phosphorus...
A.Calculate ΔS°(universe) for the decomposition of 1 mol of gaseous phosphine (PH3) to form white phosphorus and gaseous S° (J/K · mol .) . ΔfH° (kJ/mol) O2(g) 205.07 0 H2(g) 130.7 0 H2O(ℓ) 69.95    -285.83 P4(s, white) 41.1 0 PH3(g)210.24 5.47 N2(g)191.56 0 NH3(g)192.77 -45.90 Cl2(g)223.08 0 HCl(g)186.2 -92.31 CO2(g)213.74 -393.509 C(s, graphite)0 5.6 ΔS°(universe) = J/K B.Determine whether the decomposition of gaseous phosphine (PH3) to form white phosphorus and gaseous hydrogen is spontaneous at 25 °C.
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 .
Gaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine:...
Gaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine: I2(s)+5F2(g)→2IF5(g) A 4.60 −L flask containing 9.20 g I2 is charged with 9.20 g F2, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125 ∘C. Part A What is the partial pressure of IF5 in the flask? Part B What is the mole fraction of IF5 in the flask?...
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.
Nitrogen trifluoride decomposes to form nitrogen and fluorine gases according to the following equation: 2NF3(g)   N2(g) +...
Nitrogen trifluoride decomposes to form nitrogen and fluorine gases according to the following equation: 2NF3(g)   N2(g) + 3F2(g) When 3.15 mol of NF3 is placed in a 3.00-L container and allowed to come to equilibrium at 900 K, the mixture is found to contain 0.0563 mol of N2.  What is the value of Kp at this temperature? (R = 0.0821 L⋅atm⋅mol-1⋅K-1). (Hint: Solve for Kc first, then calculate Kp) a. 1.07 x 10–5 b. 1.91 x 10–3 c. 1.8 x 10–2 d....
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...
If a gaseous mixture is made by combining 3.02 g of Ar and 2.81 g of...
If a gaseous mixture is made by combining 3.02 g of Ar and 2.81 g of Kr in an evacuated 2.50 L container at 25.0 °C, what are the partial pressures of each gas and what is the total pressure exerted by the gaseous mixture?    (All three answers must be in units of atm) PAr PKr PTotal
1. Part A A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured...
1. Part A A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 24.0 ∘C is 1.75 atm . Assuming ideal gas behavior, how many grams of ammonia are in the flask? Express your answer to three significant figures and include the appropriate units. 2. Part B If 1.00 mol of argon is placed in a 0.500-L container at 30.0 ∘C , what is the difference between the ideal pressure (as predicted by the ideal gas...
Consider the following reaction: 2AgCl(s) → 2Ag(s) + Cl2(g); ΔH° = 127.1 kJ; ΔS° = 115.7...
Consider the following reaction: 2AgCl(s) → 2Ag(s) + Cl2(g); ΔH° = 127.1 kJ; ΔS° = 115.7 J/K at 298 K Suppose 59.4 g of silver(I) chloride is placed in a 63.1 L vessel at 298 K. What is the equilibrium partial pressure of chlorine gas? (R = 0.0821 L · atm/(K · mol) = 8.31 J/(K · mol)) A.5.7 × 10-17 atm B.0.95 atm C.5.1 × 10-23 atm D.0.081 atm E.0.16 atm
1- A gas mixture is made by combining 6.9 g each of Ar, Ne, and an...
1- A gas mixture is made by combining 6.9 g each of Ar, Ne, and an unknown diatomic gas. At STP, the mixture occupies a volume of 15.60 L. 2- 1.85 g of an unknown gas at 21 °C and 1.10 atm is stored in a 1.65-L flask. -What is the density of the gas?​ -What is the molar mass of the gas? 3- An open flask sitting in a lab fridge looks empty, but we know that actually it...