Amixture of hydrogen and argon gases is maintained in a 6.47 l flask at a pressure of 3.43 atm and a temperature of 85 °c. if the gas mixture contains 1.10 grams of hydrogen, the number of grams of argon in the mixture is g.

b) oxygen gas can be prepared by heating potassium chlorate according to the following equation:

2kclo3(s) > 2kcl(s) + 3o2(g)

the product gas, o2, is collected over water at a temperature of 25 °c and a pressure of 747 mm hg. if the wet o2 gas formed occupies a volume of 9.38l, the number of grams of o2 formed is g. the vapor pressure of water is 23.8 mm hg at 25 °c.

a. 8.37 g,

b. 11.67 g

Explanation:

A) Given:

We need to find the mass of argon.

Firstly, we need to apply the ideal gas law in order to find the total number of moles of gases present in the flask:

From here:

Substituting the variables:

Find the number of moles of hydrogen dividing its mass by the molar mass:

Now find the moles of argon:

Using the molar mass of argon, convert this number into mass:

B) Given:

Firstly, the total pressure is equal to the sum of the vapor pressure of water and the partial pressure of oxygen. Knowing this, solve for the pressure of oxygen:

Use the ideal gas law:

Rearrange the equation, so that we have moles in terms of the mass and the molar mass of oxygen:

Convert the pressure of oxygen into atm knowing that 1 atm = 760 mm Hg. Then:

Now rearrange the ideal gas law equation for mass:

Solve using the variables identified:

its first and third is your answer i did the qustion the fourth isnt right

answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error