If a mixture of `3` moles of `H^(2)` and one mole of `N_(2)` is completely converted into `NH_(3)`. What would be the ratio of the initial and final volume at same temperature and pressure ?

If a mixture of 3 mol of H_(2) and 1 "mole" of N_(2) is completely converted into NH_(3) , what would be the ratio of the initial and final volume at same temperature and pressure?

If a mixture of 3 mol of H_(2) and 1 "mole" of N_(2) is completely converted into NH_(3) , what would be the ratio of the initial and final volume at same temperature and pressure?

If a mixture of 3 "mole" of H_(2) and 1 "mole" of N_(2) is completely converted into NH_(3) , what would be the final volume at same P and T ?

If a mixture of 3 mole H_2 and 1 mole of N_2 is completely converted into NH_3 what would be final volume at same P and T.

40% of a mixture of 2.0 mol of N_(2) and 0.6 mol of H_(2) reacts to give NH_(3) according to the equation: N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) at constant temperature and pressure. Then the ratio of the final volume to the initial volume of gases are

40% of a mixture of 0.2 mol of N_(2) and 0.6 mol of H_(2) reacts to give NH_(3) according to the equation: N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) at constant temperature and pressure. Then the ratio of the final volume to the initial volume of gases are

40% of a mixture of 0.2 mole of N_2 and o.6 mole of H_2 react to give NH_3 according to the equation: N_ 2 ( g ) + 3 H_ 2 ( g ) ⇔ 2 N H_ 3 (g) at constant temperature and pressure. Then what is the ratio of the final volume to the initial volume of gases ?

A ballon whose volume is 5.0 L contains 7 g of N_(2) . What mass of the H_(2) gas must be added to the ballon to expand its volume to 10 L at the same temperature and pressure ? Strategy : We know the two volumes at the same temperatures and pressure. We can find the moles of N_(2) through its mass . To calculate the total moles of N_(2) and H_(2) , we apply Avogadro's law. Finally , we find the mass of H_(2) through its moles.