Question
A) Balance the following equation:NH, + -- -NO -Mo + B) How many moles of water would be produced in a reaction that consumes 10 mol NH,? C) What volume of nitrogen monoxide, in liters, could be produced if 50 g of oxygen are consumed (assume excess ammonia)? 9) Salicylic acid reacts with acetic anhydride to form aspirin according to the balanced equation below. What mass of salicylic acid is required to produce 150 g of aspirin, if the percent yield of this reaction is 78.5%? salicylic acid acetic anhydride Calculate the molar mass of each reactant/s and product/s in the above reaction first aspirin 10) The thermite reaction is performed using 8.6g Fe,O, and 1.8g Al powder Fe,O, + Al Al,O, + Fe a) Type of reaction: b) Will this reaction occur? Yes/NO; Justfy. c) Identify the limiting reagent. d) Calculate the theoretical yield of Fe produced in grams. e) If the reaction produced 2.8 g of Fe, what is the percent yield of this reaction? f) How much of the excess reagent will be left over at the end of the reaction? (You may give your answer in either moles or grams.) 11) A sample of gas initially at 1.00 atm was compressed from 12.0 L to 2.00 L at constant temperature. After the compression, the gas pressure was atm. 9) A) 2.00 B) 6.00 C) 10.0 D) 24.0 13) Consider the following reaction: 2NO Now? " 25.0 mL of No, gas is ompletely converted to N,O. gas at the same conditions, what volume will the NO, occupy? C) 125 ml D) 12.5 ml h) A) 25.0 ml B) 250 ml 14) Calcium chloride reacts with sodium carbonate to produce calcium carbonate and sodium chloride. a) Complete the balanced equation:
Explanation / Answer
A) NH3 + O3 = NO + H2O
Balance all the atoms on each sides to get equal number of stoichiometry.
Hence, the balanced chemical equation is 6 NH3 + 5 O3 = 6 NO + 9 H2O
B) 6 mole NH3 produces 9 moles H2O
10 moles NH3 produces 9/6 x 10 = 15moles H2O
C) no. of moles of O3 present = mass taken/ molar mass = 50g/48g/mol = 1.04moles
So, 5 moles O3 produces moles of NO = 6
1.04 moles O3 produces moles of NO = 6/5 x 1.04 = 1.25moles
mass of NO produced = moles x molar mass = 1.25 moles x 30g/mol = 37.5g
