Question

With work shown

1) How many moles of H2O will be produced if 6.80 x 1024 formula units of NH4NO3 are decomposed in the reaction given below?

NH4NO3 -------- N2O + 2H2O

2) Aspirin (C9H8O4) can be made in the laboratory by reacting salicylic acid (C7H6O3) with acetyl chloride (C2H3ClO).

C7H6O3 + C2H3ClO-------- C9H8O4 + HCl

What mass of HCl is produced by the complete reaction of 36.0 g of acetyl chloride?

3) Propane (C3H8) burns in oxygen to form CO2 and H2O according to the following equation. How many grams of O2 are required to burn 3.01 x 1023 propane molecules?

C3H8 + 5 O2-------3 CO2 + 4 H2O

Answer 1

Q1) the reaction is NH4NO3 -------> N2O +2H2O

From the stoichiometry, we observe that one ole of NH4NO3 produces two moles of water.

Taken 6.8x10²⁴ formula units of NH4NO3. =  6.8x10²⁴ /6.02x 10²³  moles

= 1.13x10 = 11.3 moles

Thus the moles of water produced = 2 x11.3 moles = 22.6 moles

Q2) The balanced equation for the reaction is

C9H6O3 + C2H3ClO ---------> C9H8O4 + HCl

from this equation , one mole of acetyl chloride (C2H3ClO) [= 78.5g/mol ] can produce one mole of HCl[36.5g/mol]

Thus 36.0 g of acetyl chloride can produce = 36.0x36.5 / 78.5 =16.74 g of HCl

Q3) Combustion of propane is given the balanced equation

C3H8 + 5O2 -------> 3CO2 + 4H2O

thus one mole of propane requires 5 moles of oxygen to burn.

3.01x10²³ moleculesare equal to 3.01x10²³/ 6.02x10²³ = 0.5 moles

Thus the moles of O2 required to burn 0.5 moles of propane = 5/2 moles

Thus mass of O2 required to burn = moles x molar mass

= (5/2 )molesx32g/mole

= 80 g