Inorganic Chemistry Answers

SO2 in the atmosphere contributes to acid rain. The equation for the formation of the acid is represented by: 2SO2 (g) + O2 (g) + 2H2O (l) ------> H2SO4 (aq)
What mass of sulphuric acid will form from 50.0L of sulphur dioxide at SLC (Standard Laboratory Conditions)?

1. If an electric discharge produces 800 cm3 of ozone (O3), how many cm3 of oxygen (O2) are required?

3O2(g) ---> 2O3(g)





2. When 75.0 dm3 of O2 react with an excess of glucose (C6H12O2), according to the reaction below, what volume of carbon dioxide will be produced?

6O2(g) + C6H12O6(s) ---> 6H2O(g) + 6CO2(g)

Given H2SO4 is sulfuric acid, HNO3 is nitric acid, and H3PO4 is phosphoric acid, name the following:
HCl
H2SO3
HNO2
H3PO2
HNO4
H2SO5
HI

How many grams of nitrogen and oxygen are dissolved in 125g of water at 20.0C when the water is saturated with air, in which Pnitrogen(2) equals 593 torr and Poxygen(2) equals 159 torr? At 1.00 atm pressure, the solubility of pure oxygen in water is 0.00430g O(2)/100.0g H(2)O, and the solubility of pure nitrogen in water is 0.00190g N(2)/100.0g H(2)O.

1.'Na' is a reductant, Na - Na+ + e-
but can it act as an oxidant to become Na-? Is it stable?

2. Na^5+, Na^4+, Na^3+, Na^2+, are all possible Oxidation number....... but do all exist in real? Does it happens in the case of Halogens?

determine the mass of iron in (500Kg) of hematite (Fe2O3) if the percent of iron is 74%

Question 1:

A compound A reacts according to the following hypothetical equation and has a molecular weight of 48.36 g/mol.

3 A (s) +B (aq) ––> 2 C (aq) ∆H° = ?

A sample of A, weighing 0.152 g reacts in a flask containing 250.00 g of water and the water temperature increases from 24.85 °C to a temperature of 26.26 °C. Calculate ∆H° for the reaction as written in the equation.

Answer: -1408 kJ

Question 2:

For which of the following reactions is ∆H° = ∆H°f, the heat of formation?
i. C (s) + 2 F2(g) ––> CF4 (g) ∆H° = – 221.0 kJ
ii. H(g) + Br (g) ––> HBr (g) ∆H° = –366.2 kJ
iii. 2 C(s) + H2(g) + 3 Cl2(g) ––> 2 CHCl3 (g) ∆H° = –268.2

Could you also explain exactly what Delta H means.

a 25.0 mL sample of sodium sulfate was analyzed by adding an excess of barium chloride to produce barium sulfate crystals

Na2SO4(aq) + BaCl2(aq) -> 2NaCl(aq) + BaSO4(s)

If 5.719g of BaSO4 was obtained what was the molarity of the original Na2SO4?

7.004x10^26 molecules of CHCl3

In a titration of 20.00 mL H3PO4, 12.75 mL of 0.350 M NaOH were used. a)

Find the concentration of the acid in this experiment. b) The base solution was

not standardized. How will that affect the results? How would you standardize

such a solution?