A sample of 10.5 g of nitrogen reacts with 20.2 g of hydrogen to produce ammonia. 3H2 (g) + N2 (g) → 2NH3 (g)

a. What is the theoretical yield of ammonia?

b. What is the limiting reactant?

c. What is the excess reactant?

d. How much excess reactant remains?

e. If 4.1 g of ammonia is actually produced, what is the percent yield?

Achemistry student weighs out 0.306 g of citric acid (h3c6h5o7), a triprotic acid, into a 250 ml volumetric flask and dilutes to the mark with distilled water. he plans to titrate the acid with 0.1000 m naoh solution. calculate the volume of naoh solution the student will need to add to reach the final equivalence point. be sure your answer has the correct number of significant digits.