Question

(Part A)

Hydrogen peroxide is unstable and decomposes readily: 2H2O2(aq) → 2H2O(l) + O2(g) This reaction is accelerated by light, heat, or a catalyst. The concentrations of aqueous hydrogen peroxide solutions are normally expressed as percent by mass. In the decomposition of hydrogen peroxide, how many liters of oxygen gas can be produced at STP from 26.8 g of a 7.50% hydrogen peroxide solution?

(Part B)

What volume of bromine (Br₂) vapor measured at 100.°C and 700. mmHg pressure would be obtained if 2.00 L of dry chlorine (Cl₂),measured at 17°C and 760. mmHg, was absorbed by a potassium bromide solution?

(Part C)

A few drops of concentrated ammonia solution added to a calcium bicarbonate solution cause a white precipitate to form. Write a balanced net ionic equation for the reaction. Include the states of each species.

(Part D)

Draw a Lewis structure, including all lone pair electrons and nonzero formal charges, for the C₂²⁻ ion.

(Part E)

Sodium amide (NaNH₂) reacts with water to produce sodium hydroxide and ammonia. Describe this reaction as a Brønsted acid-base reaction. Write the balanced net ionic equation:

Answer 1

Part A VT00840 082.1 x373 Lit 2.01 Wwte prt Part e mole o, gao volume. 2.2.4 u 224 2o PPt 34 02 34.01 x1. C2 leis sucture @c'ㄧ e() ㈠ : e= irbnd .. 2- obtaintd RT Ct e-ㅋ6 D.mmng at ½D BYpnsted acid 0 0821x290