A Balancing Act
H2O2 ⟶ H2O + O2
2H2O2 ⟶ 2H2O + O2
How many atoms are in a 3.56 g sample of Cu?
3.37 x 1022 Cu atoms
From the reaction: B2H6 + O2 -> HBO2 + H2O
How many moles of water are produced from 19.2 g of B2H6?
1.39 moles H2O
MnO2 + HBr → MnBr2 + Br2 + H2O
MnO2 + 4HBr → MnBr2 + Br2 + 2H2O
How many molecules of HCl are in 4.91 L of HCl acid at 25°C if the density equals 1.096 g/mL?
8.88 x 1025 molecules
From the reaction: B2H6 + O2 -> HBO2 + H2O
What mass of O2 will be needed to burn 36.1 g of B2H6?
125 g O2
PaI5 ⟶ Pa + I2
2 PaI5 ⟶ 2 Pa + 5 I2
How many g of CaCO3 are present in a sample if there are 4.52 x 1024 atoms of carbon in that sample?
751 g CaCO3
The Deacon process is one way to recover Cl2 on-site in industrial plants where the chlorination of hydrocarbons produces HCl. The reaction uses oxygen to oxidize HCl to chlorine, as shown.
HCl + O2 → Cl2 + H2O
a) Balance the chemical equation.
b) If 26 kg of HCl reacts with an excess of oxygen, how many kilograms of water would result from the Deacon process?
a) 4 HCl + O2 → 2 Cl2 + 2 H2O b) 6.4 kg
C7H14 + O2 --> CO2 + H2O
2C7H14 + 21O2 --> 14CO2 + 14H2O
What mass of Ni has as many atoms as there are N atoms in 63.0 g of NO2?
80.4 g Ni
a) Balance the following equation for the combustion of octane, C8H18,
using the lowest possible whole-number coefficients:
C8H18 + O2 ⟶ CO2 + H2O
b) How many grams of O2 are consumed during the combustion of 2.00 grams of octane?
a) 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
b) 7.02 g
Lead(II) sulfide and hydrogen peroxide react to form lead(II) sulfate and water
PbS + 4 H2O2 → PbSO4 + 4 H2O
How many carbon atoms are contained in a 1.30 x 104 mL sample of dimethylmercury? The density of Hg(CH3)2 is 15.5 g/mL.
1.05 x 1027 C atoms
Balance the following equation for the decomposition of glucose using the lowest possible whole-number coefficients:
C6H12O6 ⟶ CO2 + C2H5OH
The density of liquid ethanol, C2H5OH, is 0.789 g/mL. If 505 grams of glucose decomposes, how many liters of liquid ethanol will be produced?
a) C6H12O6 → 2 CO2 + 2 C2H5OH
b) 0.327 L