Questions LLC
Login
or
Sign Up
Ask a New Question
Science
Chemistry
In the reaction between ammonia and oxygen, 4.3302 g of Nitrogen oxide was produced. If only 3.9845 g of Nitrogen oxide was recovered, calculate the percentage yield. Round off your answer to three significant figures.
1 answer
100 * 3.9845 / 4.3302 = 92.0 %
You can
ask a new question
or
answer this question
.
Related Questions
If a certain oxide of nitrogen weighing 0.11g gives 56 ml of nitrogen and another oxide of nitrogen weighing 0.15 g gives the
ammonia, NH3, is a typical ingrediant in household cleaners. it is produced through a combination reaction involcing N2(g) and
When 34.5 L ammonia and 39.5 L oxygen gas at STP burn, nitrogen monoxide and water are produced. After the products return to
ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation.
N2+3H2g----- >
Nitric Acid is produced from nitric oxide, NO which in turn is prepared from ammonia by the ostwald process.
4NH3 + 5O2 ----->
18.1g of ammonia and 90.4g of copper(II) oxide are used in the reaction 2NH3+3CuO=N2+3Cu+3H3O.What is the limiting reactant? How
When ammonia was reacted to copper(ll)oxide at a high temperature, it will produce nitrogen gas, copper metal and water vapour.
Nitrogen oxide reacts with oxygen gas to form nitrogen dioxide (NO2). In one experiment 0.866 mole of NO is mixed with 0.503
What mass of nitrogen monoxide can be made by the reaction of 8.00 g ammonia and 17.0 g oxygen?
correct answer is 12.8 ± 0.1 (g)
in an attempt to establish the formula of an oxide of nitrogen , a known volume of the pure gas was mixed with hydrogen and
