Question

16. According to the following balanced chemical equation 1 AICI, (m + 3 AgNO.( 3 AgCl.. + Al(NO), w, how many moles of AgCl can be formed from the complete reaction of 0.15 moles of AICI.? A. 0.45 B. 0.90 C. 1.20 D. 1.35 E. 1.50 17. Consider the following balanced chemical equation: 1Al:(CO),.. + heat 2A1,0, - + 3CO. . How many liters of CO, could be formed from the complete decomposition of 1 moles of Al:(CO) at STP? A. 3 B. 22.4 C. 44.8 D. 67.2 E. 134.4 , 8. How many grams of water vapor could be formed by the complete combustion of 48.15 grams of methane, CH., according to the following chemical equation? 1 CH.. + 2 0.0 1 CO:. + 2 H,O.. A. 54 B. 76 C. 108 D. 162 E. 216

Answer 1

Question 16

One mole of AlCl3 will afford 3 moles of AgNO3.

Hence moles of AgCl formed = 0.15 x 3 = 0.45 Moles

0.45 Moles of AgCl will be formed.

Option A is correct answer

Question 17

1 mole of Al2(CO3)3 can produce 3 moles of CO2

Volume of 1 mole gas at STP = 22.4 Liters

Volume of 3 mole CO2 at STP = 22.4 Liters x 3 = 67.2 Liters

Option D is correct answer

Question 18

Mass of Methane = 48.15 gm

Moles of Methane = 48.15 gm / 16 gm/mol = 3.009 Moles

Moles of water produced = 3.0 x 2 = 6.0 moles

Mass of water produced = 6 mole x 18 g/mol = 108 gm

Option C is correct answer

Balanced equation: CH4 +2 02 = CO2 + 2 H20 Reaction type: combustion Reaction stoichiometry Limiting reagent Compound Coefficient Molar Mass Moles Weight CH4 16.04246 3.001410 48.15 31.9988 6.002820 192.0830 CO2 44.0095 3.001410 132.0906 H2O 18.01528 6.002820 108.1425 Units: molar mass - g/mol, weight - g.