How much mole of dry hydrogen at NTP is liberated on heating 0.1 mole of Mg with excess of dilute HCl? Actually what is NTP? I know the balaned equation and 1mole Mg forms 1 mole H2 , then 0.1 mole forms 1/0.1 moles of H2? Plz help
Almost. Since
Mg + 2HCl ==> H2 + MgCl2
then 0.1 mol Mg will form 0.1 mol H2. Now convert that to NTP. STP is 0 degrees C (273 kelvin) and 1 atm pressure. NTP is 20 C (293 kelvin) and 1 atm pressure.
Is this a trick question? 0.1 mol Mg metal will produce 0.1 mol dry H2 (or wet H2 for that matter but it will have water added in with it) no matter what the conditions. NTP, STP, SATP, etc will change the VOLUME of 0.1 mol gas but it won't change the amount in grams of the gas; i.e., 0.1 mol H2 will be 0.1 mol x 2g/mol = 0.2 gram no matter how you slice it.
To determine the number of moles of hydrogen gas (H2) liberated when 0.1 mole of magnesium (Mg) reacts with excess dilute hydrochloric acid (HCl), we need to use the balanced chemical equation and the concept of stoichiometry.
The balanced chemical equation for the reaction between magnesium and hydrochloric acid is:
Mg + 2HCl → MgCl2 + H2
From the equation, we can see that 1 mole of magnesium (Mg) forms 1 mole of hydrogen gas (H2). Therefore, if we have 0.1 mole of magnesium, we can expect the formation of 0.1 mole of hydrogen gas.
Now, let's define NTP (Normal Temperature and Pressure). NTP is a standard set of conditions used for experimental purposes. It is defined as a temperature of 25 degrees Celsius (298 Kelvin) and a pressure of 1 atmosphere.
Hence, at NTP, 0.1 mole of dry hydrogen gas (H2) will be liberated when 0.1 mole of magnesium reacts with excess dilute hydrochloric acid.