(1) Which of the following statements is correct for the equation shown here?
4NH3(g) + 5O2(g) ⟶ 4NO(g) + 6H2O(g)
(a) 6 g of H2O are produced for every 4 g of NH3 reacted. (b) 1 mole of NO is produced per mole of NH3 reacted. (c) 2 moles of NO are produced for every 3 moles of O2 reacted.
(2) Silicon reacts with chromium(III) oxide according to the equation
3Si(s) + 2Cr2O3(s) ⟶ 3SiO2(s) + 4Cr(s)
If 59.4 g of silicon is consumed in the reaction, what is the mass of SiO2 produced?
1)
Coefficient in stoichiometric equation represent ratio of mol or volume or number of particles. They do not represent ratio of mass.
So, a is wrong
From reaction,
Ratio of NH3 / NO = 4/4 = 1/1
So, b is correct
Ratio of O2/N2 = 5/4 = 1.25
In option c, ratio is 3/2 = 1.5
Hence this is not correct
Answer: b
2)
Molar mass of Si = 28.09 g/mol
mass of Si = 59.4 g
mol of Si = (mass)/(molar mass)
= 59.4/28.09
= 2.115 mol
According to balanced equation
mol of SiO2 formed = moles of Si
= 2.115 mol
Molar mass of SiO2,
MM = 1*MM(Si) + 2*MM(O)
= 1*28.09 + 2*16.0
= 60.09 g/mol
mass of SiO2 = number of mol * molar mass
= 2.115*60.09
= 127 g
Answer: 127 g
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