I did a lab collecting hydrogen gas. The amount of gas i collected was 45.4 ml. The temp was 295.65 Kelvins and the pressure 101.68 kPa. We used 6Molarity and 10ml of Hydrochloric reacted with 4.9cm of Magnesium.
well, the ideal gas law states
PV=nRT
so, volume = ((1 mol)(8.31 kPa L/mol K)(295.65K))/101.68kPa
= 24.16L
Note: I suspect you first need to determine the moles of hydrogen you created from the reaction, then you will know the volume of this amount of hydrogen (under the T & P conditions you listed), then you can find the volume of one mole at these conditions and finally normalize to one mole @ STP to get the answer.
The problem is you list magnesium in cm, not grams, so I don’t know how much you used (by weight).
![p389sml[1]](http://farm4.staticflickr.com/3119/2665437479_e1a40381b8_t.jpg)
Recent Comments