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Chapter 11: Q11.1-08P (page 441)

Some water dissolves in liquid methane at 1610Cto give a solution in which the mole fraction of water is6.0×10-5. Determine the mass of water dissolved in 1.00Lof this solution if the density of the solution is0.78gcm-3.

Short Answer

Expert verified

The mass of water dissolved in 1.00L of the solution of liquid methane is 0.0263g.

Step by step solution

01

The concept of mole fraction

02

Methane mass calculation

03

Calculate the number of moles of methane and water 

04

Calculate the mass of water

05

Determine the actual mass of water that can dissolve in given liquid methane solution

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Most popular questions from this chapter

The amount of ozone in a mixture of gases can be determined by passing the mixture through an acidic aqueous solution of potassium iodide, where the ozone reacts according to

O3(g)+3I-(aq)+H2O(ℓ)→O2(g)+I3-(aq)+2OH-(aq)

to form the triiodide ionI3-. The amount of triiodide produced is then determined by titrating with thiosulfate solution:

I3-(aq)+2S2O32-(aq)→3I-(aq)+S4O62-(aq)

The solution requires 26.2 mL of a 0.1359-M solution of thiosulfate ion to titrate to the endpoint. Calculate the mole fraction of ozone in the original gas sample. A small amount of starch solution is added as an indicator because it forms a deep-blue complex with the triiodide solution. Disappearance of the blue color thus signals the completion of the titration. Suppose 53.2 L of a gas mixture at a temperature of18°Cand a total pressure of 0.993 atm is passed through a solution of potassium iodide until the ozone in the mixture has reacted completely. The solution requires 26.2 mL of a 0.1359-M solution of thiosulfate ion to titrate to the endpoint. Calculate the mole fraction of ozone in the original gas sample.

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(b) 0.385gAis just neutralized by15.7mL of0.490M NaOH .

What can you conclude about the molecular weight of A from (a), from (b), and from both considered together?

Suppose 150 mL of a 10.00% by mass solution of sodium chloride (density =1.0726gcm-3) is acidified with sulfuric acid and then treated with an excess ofMnO2(s). Under these conditions, all the chlorine is liberated as Cl2(g). The chlorine is collected without loss and reacts with excessH2(g)to form HCl (g). The HCl (g) is dissolved in enough water to make 250 mL of solution. Compute the molarity of this solution.

The Henry's law constant at 250Cfor carbon dioxide dissolved in water is1.65×103atm . If a carbonated beverage is bottled under a CO2pressure of 5.0 atm .

(a) Calculate the number of moles of carbon dioxide dissolved per liter of water under these conditions, using1.00gcm-3 as the density of water.

(b) Explain what happens on a microscopic level after the bottle cap is removed.

Selenic acid (H2SeO4) is a powerful oxidizing acid that dissolves not only silver (as does the related acid H2SO4)but gold through the following reaction:

2 Au(s)+ 6H2SeO4(aq)→Au2(SeO4)3(aq)+ 3 H2SeO3(aq)+ 3 H2O(l)

Determine the oxidation numbers of the atoms in this equation. Which species is oxidized and which is reduced?
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