1.) Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide

Question

1.) Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation:        3NO2(g)+H2O(l)?2HNO3(l)+NO(g)

Suppose that 3.7mol NO2 and 1.2mol H2O combine and react completely. Which reactant is in excess?

2.) For the reaction Ti(s)+2F2(g)?TiF4(s).

Compute the theoretical yield of the product (in grams) for each of the following initial amounts of reactants.

2a) 4.0g Ti, 4.0g F2

2b) 2.4g Ti, 1.7g F2

2c) 0.236g Ti, 0.285g F2

3.) Nitrogen and hydrogen gas react to form ammonia according to the reaction: N2(g)+3H2(g)?2NH3(g)

What is the limiting reactant?

Which reactant is in excess?

4.) A chemist wants to make 5.5L of a 0.320M CaCl2 solution.

What mass of CaCl2 (in g) should the chemist use?

5.) If 3.0L of a 5.0M SrCl2 solution is diluted to 40L , what is the molarity of the diluted solution?

Explanation / Answer

1)

3NO2(g)+H2O(l)--> 2HNO3(l)+NO(g)

Each mole of water will be reacting with three moles of N02

Since there are 1.2 moles of water-> hence moles of NO2 required are 3.6

Since there are 3.7 moles of NO2, hence the NO2 is an excess reagent since after rxn 0.1 mole of NO2 will be left unused

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