A mixture of methane and hydrogen gases in a 852 l flask at...

A mixture of methane and hydrogen gases, in a 8.52 L flask at 38 °C, contains 3.02 grams of methane and 0.225 grams of hydrogen. The partial pressure of hydrogen in the flask is atm and the total pressure in the flask is atm.

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Transcript

00:01 Hi, so to solve for this, we are calculating the partial pressure of hydrogen gas and then the total pressure in the flask.

00:08 So we will solve first for partial pressure of h2 using the ideal gas equation pv is equivalent to nrt.

00:16 So for the first question, we're solving for partial pressure of hydrogen gas.

00:19 This will be equivalent to the number of moles of h2 multiplied by r, the ideal gas constant, temperature in terms of kelvin divided by the volume in terms of liters.

00:29 So plug in the information that we have.

00:31 We have 0 .225.

00:33 This is grams of hydrogen gas h2.

00:36 We need to convert this to moles and we will divide the molar mass of h2.

00:40 That's 2 .02 grams per mole of h2.

00:44 So that's the molar mass of hydrogen gas.

00:47 R is 0 .0821 liters atm per mole kelvin.

00:53 So that's the volume r.

00:54 The temperature is 38 degrees celsius.

00:56 We have to convert this to kelvin.

00:58 We'll add to 73 .15 for this to be in kelvin divided by the given volume.

01:04 We have 8 .52 liters.