Question 6 2 pts Nitric oxide, NO, is made from the oxidation of NH3, and the...
Nitric oxide, NO, is made from the oxidation of NH3, and the reaction is represented by this equation: 4 NH3 (g) + 5 O2 (g) --> 4 NO (g) + 6 H2O (g) If 2.0 g of NH3 react in excess oxygen, how many grams of NO will be produced?
Question 3 0.6 pts Nitric oxide is made from the oxidation of ammonia. What mass of nitric oxide can be made from the reaction of 8.00 g NH3 with 17.0 g O2 4 NH3(g) +5 O2(g) 4 NO(g) 6 H20(g)
14. Nitric oxide is made from the oxidation of ammonia made from the reaction of 17.00 g NH3 with 17.00 g 02? ammonia. What mass of nitric oxide (NO) can be (FW: 02 = 32.00, NH3 = 17.03, NO = 30.01, H20 = 18.02) (5 poun 4 NH3(g) + 5 O2(g) - 4 NO(g) + 6 H2O(g) - ha aur
a) consider the following reaction CH4 +4Cl2 = CCl4+ 4HCl what mass of CCl4 is formed by the reaction of 4.80g of methane with an excess of chlorine? and why b) Nitric oxide, NO, is made from the oxidation of NH3, and the reaction is represented by the equation: 4NH3 + 5O2 = 4NO + 6H2O What mass of NO can be produced from 7.76 g of NH3? and why?
6 1 point A sample of 7.16 g NH3 on oxidation produces 2.84 g of H20. Calculate the percent yield. Reaction: 4NH3 +502-4NO + 6H20 Use the following molar masses in your calculation: NH3 = 17.03 g/mol; H2O = 18.02 g/mol Do not type the percent symbol with your answer! Type your answer... Previous
26. Ammonium chromate, (NH4)2CrO4, contains what percent nitrogen by mass? 36.8% 9.2% 18.4% 11.9% none of these E) 27. B) WPCIs + xH20 →yPOCl3 + HCI The above equation is properly balanced when: A) w= 1, x=2, y = 2, z=4 w=2, x=2, y = 2, z = 2 C) w=2, x = 2, y = 2, z= 1 w= 1, x= 1, y = 1, z = 2 none of these Nitric oxide, NO, is made from the oxidation...
9 1 point A sample of 8.18 g NH3 on oxidation produces 4.78 g of H20. Calculate the percent yield. Reaction: 4NH3 +502 4NO+6H20 Use the following molar masses in your calculation: NH3 = 17.03 g/mol; H20 = 18.02 g/mol Do not type the percent symbol with your answer! Type your answer... I
Nitric acid is produced commercially by a multi-step process, starting from the oxidation of ammonia. If the % yield of each step is as shown (Step 1.) 4NH3(g) + 502(g)-→ 4N0(g) + 6H20(1) 94.9% yield Step 272NO(g) +02(g) 2NO2(g) 85.6% yield Step 3*) 3NO2(g) + H20(I)-> 2 HNO3(l) + NO(g) 80.4%yield How much ammonia (in kg) of ammonia must be input at the start of the reaction to produce 7.0kg of nitric acid.
QUESTION 15 Consider the reaction of 35 grams of NH3 and 45 grams 02. What is the theoretical yield of H20 in grams? 4NH3 + 502 -> 4NO + 6H20 Hint: Find excess reagent. 64.5 g Click Save and Submit
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. What is the maximum mass of H, O that can be produced by combining 57.1 g of each reactant? 4 NH3(g) + 502(g) → 4NO(g) + 6H2O(g) mass: - mass: ho