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...

The balanced chemical equation for the reaction between ammonia and hydrogen is: 2NH_3(g) → N_2(g) + 3H_2(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.