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In: Chemistry
Phosphine (PH3) decomposes into phosphorus and molecular hydrogen: 4PH3(g) → P4(g) + 6H2(g) Experiments show that...
Phosphine (PH3) decomposes into phosphorus and molecular hydrogen: 4PH3(g) → P4(g) + 6H2(g) Experiments show that this is a first-order reaction, with a rate constant of 0.0173 s-1 at 650°C. Identify each of the following statements about this reaction as true or false. (Use the drop-down menu and select "True" or "False" for each. You must get all 4 correct.)
The reaction PH3 → PH2 + H might be the rate-determining step in the mechanism of this reaction.
The rate constant would be greater than 0.0173 s-1 at 340°C.
The overall reaction could occur as a single elementary step.
The activation energy for the reaction cannot be determined without additional data.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
Phosphine (PH3) decomposes into phosphorus and molecular hydrogen: 4PH3(g) → P4(g) + 6H2(g) Experiments show that...
Phosphine (PH3) decomposes into phosphorus and
molecular hydrogen:
4PH3(g) → P4(g) + 6H2(g)
Experiments show that this is a first-order reaction, with a rate
constant of 0.0173 s-1 at 650°C. Identify each of the
following statements about this reaction as true or false. (Use the
drop-down menu and select "True" or "False" for each. You must get
all 4 correct.)
True/False The mechanism for this reaction must involve
two or more elementary steps.
True/False The activation energy for the reaction cannot
be...
How many grams of phosphine (PH3) can form when 44.4 g of phosphorus and 98.8 L...
How many grams of phosphine
(PH3) can form when 44.4 g of
phosphorus and 98.8 L of hydrogen gas react at
STP?
P4(s) + H2(g) →
PH3(g) (Unbalanced)
Calculate ΔS°(universe) for the decomposition of 1 mol of gaseous phosphine (PH3) to form white phosphorus...
Calculate ΔS°(universe) for the decomposition of 1 mol of
gaseous phosphine (PH3) to form white phosphorus and gaseous
hydrogen at 25 °C.
Gaseous phosphorus pentachloride decomposes according to the reaction PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)...
Gaseous phosphorus pentachloride decomposes according to the
reaction
PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)
The equilibrium system was analyzed at a particular temperature,
and the concentration of the substances present were determined to
be [PCl5] = 1.1 x10-2 M, [PCl3] = 0.325 M, and [Cl2] = 3.9 x 10-3
M. Calculate the value of K for the reaction.
Phosphine decomposes by the following reaction: COCl2(g) <---> CO(g) + Cl2(g) Kc = 8.3 x 10-4...
Phosphine decomposes by the following reaction:
COCl2(g) <---> CO(g) +
Cl2(g) Kc = 8.3 x 10-4
Calculate the concentration of each component when 2.55 g of
phosphine decomposes in a 25.0mL flask.
30.00mg of phosphorus (P4) is added to a 2.00Lcontaining only molecular oxygen, PO2= 352 mmHg, and...
30.00mg of phosphorus (P4) is added to a 2.00Lcontaining only
molecular oxygen, PO2= 352 mmHg, and Argon, PAr= 489 mmH, at 80.2
degrees C.
A) Calculate amount of heat consumed or produced if only
Phosphorus and oxygen react according to the following reaction:
P4(s)+5O2(g) --->P4O10(s) ΔH= -2940 kJ
B) Mole fractions and partial pressures of remaining gases?
Phosphorus pentachloride decomposes according to the chemical equation PCI5 (g) <---> PCI3 (g) + Cl2(g) Kc=...
Phosphorus pentachloride decomposes according to the chemical
equation PCI5 (g) <---> PCI3 (g) + Cl2(g) Kc= 1.80 at
250°C
A 0.244 mol sample of PCl5(g) is injected into an empty 2.65 L
reaction vessel held at 250 °C. Calculate the concentrations of
PCl5(g) and PCl3(g) at equilibrium.
Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) - PCl3(g) + Cl2(g) A 0.213 mol...
Phosphorus pentachloride decomposes according to the chemical
equation PCl5(g) - PCl3(g) + Cl2(g) A 0.213 mol sample of PCl5(g)
is injected into an empty 3.40 L reaction vessel held at 250
degrees C. Calculate the concentrations of PCl5(g) and PCl3(g) at
equilibrium.
Phosphorus pentachloride decomposes at higher temperatures. PCl5(g) ⇄ PCl3(g) + Cl2(g) An equilibrium mixture at some...
Phosphorus pentachloride decomposes at higher temperatures.
PCl5(g) ⇄ PCl3(g) + Cl2(g)
An equilibrium mixture at some temperature consists of
3.03 g PCl5, 208.23 g/mol
4.86 g PCl3, 137.33 g/mol
3.59 g Cl2, 70.91 g/mol
in a 1.00-L flask.
If you add 1.31 g of Cl2, how will the equilibrium be
affected and what will the concentration of PCl5 be when
equilibrium is reestablished?
shift left
shift right
no shift will occur
[PCl5] = mol/L
Phosphorus pentachloride decomposes at higher temperatures. PCl5(g) ⇄ PCl3(g) + Cl2(g) An equilibrium mixture at some...
Phosphorus pentachloride decomposes at higher
temperatures.
PCl5(g) ⇄ PCl3(g) + Cl2(g)
An equilibrium mixture at some temperature consists of
5.93 g PCl5, 208.23 g/mol
4.86 g PCl3, 137.33 g/mol
3.59 g Cl2, 70.91 g/mol
in a 1.00-L flask.
If you add 1.31 g of Cl2, how will the equilibrium be affected
and what will the concentration of PCl5 be when equilibrium is
reestablished?
shift left
shift right
no shift will occur
[PCl5] = mol/L
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