What volume of hydrogen will be produced if 100cm3 of ammonia is completely decomposed at constant temperature and pressure? The equation for reaction is 2N...
What volume of hydrogen will be produced if 100cm3 of ammonia is completely decomposed at constant temperature and pressure? The equation for reaction is 2NH3(g) → N2(g) + 3H2(g)
Answer Details
The balanced chemical equation for the reaction between ammonia and hydrogen is: 2NH3(g) → N2(g) + 3H2(g) From the equation, we can see that 2 moles of ammonia reacts to produce 3 moles of hydrogen. Therefore, the ratio of ammonia to hydrogen is 2:3. This means that for every 2 moles of ammonia, 3 moles of hydrogen will be produced. To determine the volume of hydrogen produced, we need to use the volume of ammonia given in the question. We can assume that the ammonia is measured under the same temperature and pressure as the hydrogen produced. Since we are given the volume of ammonia, we need to convert it to moles using the ideal gas law: PV = nRT Where: P = pressure (constant) V = volume of gas (in liters) n = number of moles R = ideal gas constant T = temperature (constant) Assuming constant temperature and pressure, we can simplify the equation to: V = n Therefore, the volume of ammonia (100 cm3) is equal to its number of moles. Using the ratio from the balanced equation, we can calculate the number of moles of hydrogen produced: 2 moles NH3 : 3 moles H2 100 cm3 NH3 : x cm3 H2 x = (100 cm3 NH3)(3 mol H2/2 mol NH3) = 150 cm3 H2 Therefore, the volume of hydrogen produced is 150 cm3. The correct answer is (B) 150 cm3.