At what temperature will 5 g of Cl2 exert a pressure of 900 mmHg at a volume of .75 L?

The temperature : 154.73 K

Further explanation

Given

mass = m = 5 g of Cl2

P = 900 mmHg = 1,18421 atm

V = 0.75 L

Required

Temperature

Solution

mol Cl2 = mass : MW = 5 : 71 = 0.07

Ideal gas law : PV = nRT

P = pressure, atm  

V = volume, liter  

n = number of moles  

R = gas constant = 0.082 L.atm / mol K  

T = temperature, Kelvin  

T = PV/nR

Input the value :

T = 1.18421 x 0.75 / 0.07 x 0.082

T = 154.73 K

Most likely a is the answer - because  you generate   38 atp's but also consume an atp.   each atp gives approx. less than 4 kcal so probably a is the closest answer.

Answerthis solution will not form a precipitateexplanationsolubility equilbrium:         pbf₂(s)  ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is    (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as    then, we can interpret  q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually  forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product:     since q = 2.7  × 10⁻⁸ < ksp =  4  ×  10⁻⁸, a precipitate will not form.