Other Chemistry Answers

Identify the element X in the following nuclear reactions.

(I) N^15 +H^1 ⟶ He^4 +X

(ii) H^1+Be^9 ⟶ X + n

(III) C^13 + H^1⟶ X

• Calculate the number of moles of lead (II) nitrate
• Calculate the number of moles of sodium iodide
• Calculate the number of moles of lead (II) iodide produced assuming sodium iodide is limiting and lead (II) nitrate is in excess using mole ratios between lead (II) iodide and sodium iodide.
• Calculate the number of moles of lead (II) iodide produced assuming lead (II) nitrate is limiting and sodium iodide is in excess using mole ratios between lead (II) iodide and lead (II) nitrate
• Identify which reactant is the limiting reagent based upon your calculations.
• Calculate the mass of lead (II) iodide

Balanced Equation: Pb(NO3)2 + 2 NaI = Pbl2 + 2 NaNO3

2.190 g of sodium iodide

2.282 g of lead (II) nitrate

The average amount of Lead (II) iodide: 2.9955

2. Sodium metal reacts with water to form sodium hydroxide and hydrogen gas

a. Balanced Chemical Reaction:

 b. If you have 90.0 g of sodium and 80.0 g of water which is the limiting reactant and which is the excess reactant?

c. How many grams of the excess reactant are left over when the reaction is completed?

d. How many grams of hydrogen gas are produced?

4. Calcium carbonate (CaCO3) which is found in limestone and marble reacts readily with hydrochloric acid (HCl) to produce calcium chloride (CaCl2), carbon dioxide, and water.

a. Write the balanced chemical reaction:

b. What mass of hydrochloric acid will be needed to produce 325 g of calcium chloride?

c. What mass of carbon dioxide could be produced if 750 g of calcium carbonate reacts with excess hydrochloric acid?

1. Why do you think water and oil will not mix?
2. Is the bonding between atoms of molecules is strong or weak? Why?

The equilibrium constant Kp for the oxidation of sulfur dioxide into sulfur trioxide is 5.6×10-4 at 3500°C. If the equilibrium partial pressures of SO2 and SO3 are 0.64 atm and 0.58 atm, respectively, what is the partial pressure of O2 in the system?

  2SO2(g) + O2(g) —› 2SO3 (g)

2KCLO₃→ 2KCl + 3O_2(g)

1.5 mole of KCLO₃ was decompose during an experiment in laboratory 40 dm³

of O₂ was produced find out 

percentage yield of O_2.

Arrange the following gases in increasing order of non ideality also given reason. H2, CH4, NH3

Na2CO3 + 2HCl → 2NaCl + CO2 + H2O

During an experiment 50g mass of Na2CO3 react with 0.5 mole of HCl. Calculate the actual mass of water produced.

1500cm3

of an unknown gas have a pressure of 10000 N/m2

at 30C° find out number of moles of gas present inside 

the container.