2.14 2H2(g)+ 0(g) +2H200) If 100g of hydrogen is burnt how many grams of water a
ID: 1029629 • Letter: 2
Question
2.14 2H2(g)+ 0(g) +2H200) If 100g of hydrogen is burnt how many grams of water are produced? b How many moles of methane must have reacted if D.2 mole of CO2 gas are produced when the methane reacts with excess oxygen in the combustion reaction according to the following equation If 17 6 of CO; is produced how many grams of methane must have been burnt? c How many moles of Ha gas are produced when 0.1 mole of Mg reacts with excess HCI in the single displacement reaction according to the folowing equation If 2 4g of magnesium have reacted, haw many grams of hydrogen gas must have been produced? d How many moles of Cuso4 solution must have reacted with excess Zn if 3.2g of copper were produced in the single displacement reaction according to the follawing equation If 3 2g of copper were produced how many grams of copper suifate must have been reacted? How many males of oxygen are formed when 6 moles of KCIO, react in the decomposition reaction acoording to the following equation? e If 12.4g of KCIO, has decomposed how many grams of axygen gas must have been produced? How many moles of CaCO, must have reacted if 3 moles of carbon dioxide were produced in the decomposition reaction according to the following equation? fExplanation / Answer
Solutions:- a)
2H2(g) + O2(g) -----> 2H2O(l)
From the balanced equation, there is 2:2 mol ratio between H2 and H2O.
100 g H2 x (1mol H2/2.02 g H2) x (2mol H2O/2 mol H2) x (18.02 g H2O/1mol H2O) = 892 g H2O
b) The balanced equation given for the combustion of methane is...
CH4(g) + 2O2(g) -----> CO2(g) + 2H2O(l)
0.2 mol CO2 x (1 mol CH4/1mol CO2) = 0.2 mol CH4
Now when 17,6 g of CO2 are produced then grams of CH4 could be calculated as...
17.6 g CO2 x (1 mol CO2/44.01 g CO2) x (1 mol CH4/1mol CO2) x (16.05 g CH4/1mol CH4) = 6.42 g CH4
c) Mg(s) + 2HCl(aq) -----> MgCl2(aq) + H2(g)
0.1 mol Mg x (1 mol H2/1mol Mg) = 0.1 mol H2
When 2.4 g of Mg were reacted...
2.4 g Mg x (1mol Mg/24.305 g Mg) x (1 mol H2/1mol Mg) x (2.02 g H2/1mol H2) = 0.199 g H2
d) Zn(s) + CuSO4(aq) -----> ZnSO4(aq) + Cu(s)
3.2 g Cu x (1mol Cu/63.546 g Cu) x (1mol CuSO4/1mol Cu) x (159.6 g CuSO4/1mol CuSO4) = 8.04 g CuSO4
e) 2KClO3(s) ------> 2KCl(s) + 3O2(g)
6 mol KClO3 x (3 m ol O2/2mol KClO3) = 9 mol O2
When 12.4 g of KClO3 are decomposed then...
12.4 g KClO3 x (1mol KClO3/122.55 g KClO3) x (3 mol O2/2mol KClO3) x (32 g O2/1mol O2) = 4.86 g O2
f) CaCO3(s) ------> CaO(s) + CO2(g)
3 mol CO2 x (1mol CaCO3/1mol CO2) = 3 mol CaCO3
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