Question 1. considering the reaction of the decomposition of n2o5 to form the products no2 and o2, calculate the average reaction rate if at 0.00s the concentration of n2o5 was 1.00 m and at 4.00s it decreases to 0.987 m?
2 n2o5 4 no2 + o2
4.97 × 10-1 mol/(l × s)
7.27 × 10-2 mol/(l × s)
6.50 × 10-3 mol/(l × s)
3.25 × 10-3 mol/(l × s)
question 2. what is the oxidation number of sulfur (s) in sulfuric acid (h2so4)?
-6
+2
+4
+6

10. translate each of the following chemical equations into a sentence. a. 2 zns(s) + 3 o2(g) -> 2 zno(s) + 2 so2(g) b. cah2(s) + 2 h2o(l) -> ca(oh)2 (aq) + 2 h2(g)

Astudent is given a sample of a blue copper sulfate hydrate. he weighs the sample in a dry covered porcelain crucible and got a mass of 23.875 g for the crucible, lid, and sample. the mass of the empty crucible and lid was found earlier to be 22.652 g. he then heats the crucible to expel the water of hydration, keeping the crucible at red heat for 10 minutes with the lid slightly ajar. on colling, he finds the mass of crucible, lid, and contents to be 23.403 g. the sample was changed in the process to very light clue anhydrous cuso4. if there are again 100.0 g of hydrate, how many grams of cuso4 are in it? how many moles of cuso4? (hint: molar mass of cuso4 = 159.6 g / mole. what per cent of the hydrate is cuso4? you may convert the mass of cuso4 to moles.)

If 1.8 l of water is added to 2.5l of a 7.0 m koh solution, what is the molarity of the new solution