Write the balanced equation, then outline the steps necessary determine the information equation in each of the following:
(a) the number of moles than the mass of the chlorine cl2 required to react with 10.0 g of sodium metal na to produce sodium chloride nacl
(b) the number of moles and the mass of the oxygen formed by the decomposition of 1.252 gram of mercury (ii) oxide
(c)the number of the moles and the mass of the sodium nitrate nano3 required to produce 128 gram of oxygen (nano2 is the other product)
(d)the number of moles and the mass of the carbon dioxide formed by the combustion of 20.0 kg of carbon in excess of oxygen
(e)the number of moles and the mass of the copper(ii) carbonate needed to produce 1.500 kg of copper ii oxide (co2 is the other product)

a) The reaction requires 0.218 moles or 15.45 grams of Chlorine Cl2

b) There are 0.00289 moles or 92.49 mg of oxygen formed

c) The reaction requires 8 moles or 679.96 grams of NaNO3

d) There are 1666.67 moles or 73.35 kg of CO2 formed

e) The reaction requires 18.857 moles or 2.32978 kg of CuCO3 formed

Explanation:

a) Step 1: Balance reaction

1 Cl2 + 2 Na → 2 NaCl

So for 2 moles Na ( and also for 2 moles NaCl) we have 1 mole Cl2

Step 2: Calculate moles Cl2

⇒Moles Na = mass Na / Molar mass Na

⇒Moles Na = 10g / (22.89g/mole) = 0.43687 moles

⇒ for 2 moles Na  we have 1 mole Cl2

moles Cl2 = 0.43687/2 = 0.218 moles

Step 3: Calculate mass Cl2

mass Cl2 = moles Cl2 x Molar mass Cl2

mass Cl2 = 0.218 moles x (70.90 g/moles) = 15.45g Cl2

b) Step 1: Balance reaction

2 HgO  → 2 Hg + O2

So for 2 moles HgO  we have 1 mole O2

Step 2: Calculate moles O2

⇒Moles HgO = mass HgO / Molar mass HgO

⇒Moles Na = 1.252g / (216.59g/mole) = 0.0057805 moles

⇒ for 2 moles HgO  we have 1 mole O2

moles O2 = 0.0057805/2 = 0.00289 moles

Step 3: Calculate mass O2

mass O2 = moles O2 x Molar mass O2

mass O2 = 0.00289 moles x (32 g/moles) = 0.09248g O2 = 92.48 mg O2

c) Step 1: Balance reaction

2 NaNO3  → 2 NaNO2 + O2

So for 1 mole O2  we have 2 moles NaNO3

Step 2: Calculate moles NaNO3

⇒Moles O2 = mass O2 / Molar mass O2

⇒Moles O2 = 128g / (32g/mole) = 4 moles

⇒ for 1 mole O2  we have 2 mole NaNO3

moles NaNO3 = 4 x 2 = 8 moles

Step 3: Calculate mass NaNO3

mass NaNO3 = moles NaNO3 x Molar mass NaNO3

mass NaNO3 = 8 moles x (84.9947 g/moles) = 679.96 g NaNO3

d) Step 1: Balance reaction

C + O2 → CO2

So for 1 mole Carbon  we have 1 mole CO2

Step 2: Calculate moles CO2

⇒Moles C = mass C / Molar mass C

⇒Moles C = 20000g / (12g/mole) = 1666.67 moles

⇒ for 1 mole C  we have 1 mole CO2

moles CO2 = 1666.67 moles

Step 3: Calculate mass CO2

mass CO2 = moles CO2 x Molar mass CO2

mass O2 = 1666.67 moles x (44.01 g/moles) = 73350 grams CO2 = 73.350 kg CO2

e) Step 1: Balance reaction

CuCO3 → CuO + CO2

So for 1 mole CuO we have 1 mole CuCO3

Step 2: Calculate moles CuCO3

⇒Moles CuO = mass CuO / Molar mass CuO

⇒Moles CuO = 1500g / (79.545g/mole) = 18.857 moles

⇒ for 1 moles CuO  we have 1 mole CuCO3

moles CuCO3 = 18.857 moles

Step 3: Calculate mass CuCO3

mass CuCO3= moles CuCO3 x Molar mass CuCO3

mass CuCO3= 18.857 moles x (123.55  g/moles) = 2329.78g CuCO3 = 2.32978 kg CuCO3

"record the time to complete a chemical reaction" would most likely be part of a lab procedure.