Final answer:
The student's questions relate to chemical stoichiometry, specifically calculating moles of ammonia that will react with a given amount of oxygen and the volume of NO produced from a certain volume of oxygen. By using the mole ratios from balanced chemical equations, we can determine the quantities of reactants and products.
Step-by-step explanation:
The student's questions are centered around the stoichiometry of reactions involving ammonia, NH3. Specifically, they're asking about stoichiometric calculations using balanced chemical equations. Answering the student's questions involves using the provided mole ratios from the balanced equations to calculate the amounts of reactants and products in the reactions.
To address the student's concerns:
A) They've provided the equation 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g). To find out how many moles of ammonia will react with 7.0 moles of oxygen, we would use the stoichiometric ratio from the balanced equation. Since 5 moles of oxygen react with 4 moles of ammonia, we can set up a proportion: (7 moles O2) / (5 moles O2) = (x moles NH3) / (4 moles NH3). Solving for x gives us the moles of ammonia that will react.
B) To determine how many milliliters of NO can be made by the reaction of 102 ml of oxygen, we again use the stoichiometric ratios. Since volumes of gases at constant temperature and pressure are directly proportional to moles, the mole ratio between O2 and NO is 5:4, and the volume ratio will be the same. Therefore, if 102 ml of O2 are reacted, we will produce (102 ml O2) * (4 moles NO/5 moles O2) ml of NO.
For the additional equation provided (N2 + 3 H2 → 2 NH3), the calculation will involve the mole ratios of 1:3 for N2 to H2 and the ratio 1:2 for N2 to NH3.