General Chemistry Answers

One of the reactions used to inflate automobile air bags involves sodium azide

(NaN3). The balanced equation will be: 2NaN3(s) → 2Na(s) + 3N2(g). Determine the mass of N2

produced from the decomposition of 100.0 g of NaN3.

Learning Task 2

Write the equilibrium constant expression for each of the following reactions.

1. H2(g) + I2(g) ⇌ 2HI(g)

2. 3O2(g) ⇌ 2O3(g)

3. 2CO2(g) ⇌ 2CO(g) + O2(g)

4. CH3COOH(aq) + C2H5OH ⇌ CH3COOC2H5(aq) + H2O(l)

5. AgCl(s)

⇌

Ag+

(aq) + Cl-

(aq)

Express the concentration of solution in % w/v containing 12 g sodium chloride and 50 ml of water.

5.0 L of 0.4 M H2SO4 contains how many moles?

Good day

In a laboratory pot experiment, what is the allowed or standard weight in mg.kg-1 of each of this Cadmium, selenium, and silicon to be added to the pot experiment.

By applying solubility guidelines,state which of the following compounds will precipitate in water

1 cobalt (ll) hydroxide

2 sodium nitrate

3 Ammonium phosphate

4 potassium chloride

5 none of the above

what is the poh of a 7.2 x 10-8 m blood sample

how and why the decay of Uranium 238 and Technetium–99m are both considered spontaneous even though the time and rate of decay are different.

A 0.240g of a compound of oxygen and element X was found by analysis to contain 0.960g of X and 0.144g of oxygen

1. Calculate the percentage composition by weight

2. Calculate from the above data, three(3) possible weight for X relative to oxygen

NH4NO3(s) → N2O(g) + 2H2O(l)

In a certain experiment, 156 g of ammonium nitrate is decomposed. Find the mass of each of the products formed.