Hey guys I'm stuck on this one question.
The fuel tank of one type of hydrogen-powered car holds 70kg of magnesiumhydride. Calculate the volume of hydrogen gas, measured at room temperature and pressure,which would be produced if this amount of magnesium hydride reacted with water.
MgH2(s) + 2H2O(I) -----> Mg(OH)2(s) + 2H2(g)
The marking scheme says this :
Moles MgH2 = 70000 = 2659.6 (2660) (1)
26.32Moles H2 = 5319.2 (5320) (1) I've gotten to here, but I just cant figure out what to do to get the next answer.
Volume H2 = 1.28 × 105dm3(1)
Thanks for any help!