Which is correct..?

The normal boiling point of mercury (Hg) is 356.7 °C. What is the vapor pressure of mercury at 333 °C in atm? (∆Hvap = 58.51 kJ/

grigory [225]

Answer:

Here you can use the Clausis Clayperon equation: ln P1/P2=-Ea/R-(1/T1 - 1/T2)

where P1 is the pressure at standard condition: 760 mm Hg

P2 is the variable we need to solve

Ea is the activation energy, which in this case is delta H vaporisation: 56.9 kJ/mol

R is the gas constant 8.314 J/mol or 8.314 J/mol /1000 to convert to kJ

T1 is the normal boiling point 356.7 C, but converted to Kelvin: 629.85K

T2 is room temperature 25 C, but converted to Kelvin: 298.15 K

Once you plug everything in, you should get 4.29*10^-3 mmHg

Explanation:

8 0

3 years ago

What is urine made of?

Annette [7]

Answer: 90 percent water, electrolytes such as potassium and phosphorus, and chemicals called urea and uric acid

Explanation:

6 0

3 years ago

What is the oxidation state of S in so ??

Marina86 [1]

Answer:

+2

Explanation:

If a compound $SO$ existed, we would identify the oxidation state of sulfur using the following logic:

oxygen is more electronegative than sulfur, so it's more electron-withdrawing and it should have a negative oxidation state producing a positive oxidation state for sulfur;
oxygen typically has an oxidation state of -2;
we may then apply the fact that SO is expected to be a molecule with a net charge of 0;
if the net charge is 0 and the oxidation state of oxygen is -2, we may set the oxidation state of S to x;
write the equation for the net charge of 0 by adding all individual charges of the two atoms: $x + (-2) = 0$ ;
hence, x = 2.

That said, in this hypothetical compound S would have an oxidation state of +2.

6 0

3 years ago

Which term is used to describe the attraction that an oxygen atom has for the electrons in a chemical bond?

Mekhanik [1.2K]

electronegativty

It is the attraction force

8 0

3 years ago

Read 2 more answers

Assume that an exhaled breath of air consists of 74.8% N2, 15.3% O2, 3.7% CO2, and 6.2% water vapour.

Goryan [66]

Answer:

a) PN₂ = 0.733 atm

PO₂ = 0.150 atm

PCO₂ = 0.036 atm

Pwater = 0.061 atm

b) 6.44x10⁻⁴ mol

c) 0.02 g

Explanation:

a) By the Dalton's Law, in a gas mixture, the total pressure is the sum of the partial pressures, and the partial pressure is the molar fraction of the gas multiplied by the total pressure.

PN₂ = 0.748*0.980 =0.733 atm

PO₂ = 0.153*0.980 = 0.150 atm

PCO₂ = 0.037*0.980 = 0.036 atm

Pwater = 0.062*0.980 = 0.061 atm

b) The number of moles of CO₂ can be calculated by the ideal gas law:

PV = nRT, where P is the pressure, V is the volume (0.455 L), n is the number of moles, R is the gas constant (0.082 atm.L/mol.K), and T is the temperature (37°C + 273 = 310 K).

0.036*0.455 = 0.082*310*n

25.42n = 0.01638

n = 6.44x10⁻⁴ mol

c) For the combustion reaction of glucose:

C₆H₁₂O₆ + 6O₂ → 6CO₂ + 6H₂O

So, the stoichiometry is:

1 mol of glucose ------- 6 moles of CO₂

x ------- 6.44x10⁻⁴ mol of CO₂

By a simple direct three rule:

6x = 6.44x10⁻⁴

x = 1.073x10⁻⁴mol of glucose

Glucose has a molar mass equal to 180 g/mol, and its mass is the molar mass multiplied by the number of moles:

m = 180x1.073x10⁻⁴

m = 0.02 g

8 0

3 years ago