Atomic chlorine is produced under ozone-hole conditions by the photodissociation of Cl2. Given that Cl2 gas...

Atomic chlorine is produced under ozone-hole conditions by the photodissociation of Cl2. Given that Cl2 gas is the most stable form of the element, and that the ΔHfo for atomic chlorine is +121.7 kJ mol-1, calculate the maximum wavelength of light that can dissociate diatomic chlorine into the monoatomic form. Does this wavelength correspond to the UVA or UVB region of the wavelength spectrum?

Expert Solution

ΔHfo for atomic chlorine is +121.7 kJ mol-1

so that , DH0 dissociation of Cl2 = 121.7*2 = +243.4 Kj/mol

1 Cl2 molecule required energy = 243.4*10^3/(6.023*10^23) = 4.04*10^-19 joule

suitable wavelength (l) = hc/E = (6.625*10^-34*3*10^8)/(4.04*10^-19)

= 4.92*10^-7 m

= 492 nm

suitable light = visible region.

queen_honey_blossom answered 2 years ago

The rate constants for the reactions of atomic chlorine and of hydroxyl radical with ozone are...

The rate constants for the reactions of atomic chlorine and of hydroxyl radical with ozone are given by 3 x 10-11 e-250/T and 2 x 10-12 e-940/T, where T is the Kelvin temperature. Calculate the rate constant for ozone destruction by chlorine under conditions in the Antarctic ozone hole, when the temperature is about -80°C and the concentration of atomic chlorine increases by a factor of one hundred to about 4 x 105 molecules cm-3.

Chlorine gas (Cl2) can be produced by reaction of hydrochloride acid with manganese oxide. What is...

Chlorine gas (Cl2) can be produced by reaction of hydrochloride acid with manganese oxide. What is the volume of chlorine gas is produced by adding 1 g of MnO2 to one litre of 1 M HCl? MnO2 + 4HCl -> MnCl2 + Cl2 + 2H2O How much chlorine gas is produced when instead of 1 g MnO2 this time 50 g MnO2 is added?

Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2 (g) + 3 F2 (g)...

Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2 (g) + 3 F2 (g) → 2 ClF3 (g) A 1.65 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 741 mmHg . What is the pressure of ClF3 in the reaction vessel after the reaction? Enter your answer numerically, in terms of mmHg.

Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2(g) + 3 F2(g) --> 2...

Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2(g) + 3 F2(g) --> 2 ClF3(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 729 mmHg. Identify the limiting reactant and deter- mine the theoretical yield of ClF3 in grams. I got 4.84g ClF3 for this problem, but the textbook answer is 2.84g. Can anyone tell me where I went wrong,...

Sodium reacts with chlorine gas according to the reaction What volume of Cl2 gas, measured at...

Sodium reacts with chlorine gas according to the reaction What volume of Cl2 gas, measured at 867 torr and 55.0 °C, is required to form 42.0 g NaCl (58.44 g/mol)

Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2(g)+3F2(g)→2ClF3(g) A 2.15 L reaction vessel,...

Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2(g)+3F2(g)→2ClF3(g) A 2.15 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 882 mmHg. Identify the limiting reactant and determine the theoretical yield of ClF3 in grams.

A rigid tank contains 61.5 g of chlorine gas (Cl2) at a temperature of 77°C and...

A rigid tank contains 61.5 g of chlorine gas (Cl2) at a temperature of 77°C and an absolute pressure of 6.00 × 105 Pa. Later, the temperature of the tank has dropped to 34°C and, due to a leak, the pressure has dropped to 3.90 × 105 Pa. How many grams of chlorine gas have leaked out of the tank? (The mass per mole of Cl2 is 70.9 g/mol.)

Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas: PCl3(g)+Cl2(g)⇌PCl5(g). A 7.5-L gas...

Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas: PCl3(g)+Cl2(g)⇌PCl5(g). A 7.5-L gas vessel is charged with a mixture of PCl3(g) and Cl2(g), which is allowed to equilibrate at 450 K. At equilibrium the partial pressures of the three gases are PPCl3 = 0.127 atm , PCl2 = 0.152 atm , and PPCl5 = 1.30 atm . Part A) What is the value of Kp at this temperature? Part B) Does the equilibrium favor reactants or products?...

Consider the reaction: Cl2(g) D 2Cl(g). Exactly 1.000 mole of chlorine gas is placed into a...

Consider the reaction: Cl2(g) D 2Cl(g). Exactly 1.000 mole of chlorine gas is placed into a 1.000 L container at 298 K. Determine the number of chlorine atoms in that container at equilibrium, assuming DGof (Cl) = 105.3 kJ/mol.

Q3. Standard enthalpies of formation for atomic oxygen and for ozone are given here: O(g), ΔfH°...

Q3. Standard enthalpies of formation for atomic oxygen and for ozone are given here: O(g), ΔfH° = 249.2 kJ mol-1. O3(g), ΔfH° = 142.7 kJ mol-1 For each of the reactions below, evaluate the standard reaction enthalpy (kJ mol-1) corresponding to the dissociation threshold, and therefore calculate the wavelength (nm) and state the “colour” of a photon with the minimum energy sufficient to achieve dissociation. (a) dissociation of molecular oxygen, O2(g). {numerical ans. 240 nm} (b) dissociation of ozone, O3(g),...

Question