Calculate the gas constant, r, if 25.55 ml of hydrogen gas was collected at a barometric pressure of 0.987 atm and a temperature of 295 k. the vapor pressure of water at this temperature is 0.026 atm.

This problem is providing 25.55 mL of hydrogen gas that is collected with steam at 295 K and 0.987 atm. Thus, it is asked for the calculation of the gas constant R, which is derived from the ideal gas law:

Whereas we solve for R as follows:

Nevertheless, the pressure of hydrogen will be equal to the barometric one minus waters, since the gas is composed by hydrogen and steam:

Hence, we can plug in the given variables to obtain R, however, since the moles of hydrogen are not given, we can write it for you to plug that in further:

Keep in mind that if you measured grams of hydrogen, you will need to convert them to moles by dividing by its molar mass (2.02g/mol) so that you will be able to get the correct result.

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oxygen, selenium, tellurium, and polonium.

they're all from the same group as sulfur (group 16).

a). in this case, dh> 0 and sd> 0. if t becomes larger, the term "-tds" will become more negative. at some point, it is possible that -dts will be more negative than the dh is positive, and the reaction will become spontaneous. this is probably the correct answer, but you should look at all of the other possibilities and make sure of that.