Step one write the chemical equation for reaction
= Ag2O + 2(C10H10N4SO2)---> 2 ( AgC10H9N4SO2)
The reacting ratio of Ag2O to AgC10H9N4SO2 is 1:2 from the reaction above
step 2; find the number of moles of AgC10H9N4SO2
that is mass/molar mass
The molar mass of AgC10H9N4SO2 = 107.86 +(12 x10) + (1 x 9) + (4 x 14) +32 +(16 x2) =356.86g/mol
moles is therefore= 25g/356.86g/mol= 0.07moles
by use of mole ratio the moles of Ag2O= 0.0702=0.035moles
mass = moles x molar mass
the molar mass of Ag2O=231.72 g/mol
mass is therefore= 231.72g/mol x 0.035moles= 8.11grams
Answer:
The answer to your question is
Explanation:
Data
12.5 g of reactant
Balanced Reaction 1
TiBr₄ + 2H₂ ⇒ Ti + 4HBr
Molar mass of TiBr₄ = 48 + (4 x 80) = 368 g
Atomic mass of Ti = 48 g
Molar mass of HBr = 1 + 80 = 81
368 g of TiBr₄ ---------------- 48 g of Ti
12.5 g of TiBr₄ -------------- x
x = (12.5 x 48) / 368
x = 1.63 g of Ti
368 g of TiBr₄ ----------------4(81) g of HBr
12.5 g of TiBr₄ ------------- x
x = (12.5 x 324) / 368
x = 11 g of HBr
Balanced reaction 2
3SiH₄ + 4NH₃ ⇒ Si₃N₄ + 12H₂
Molar mass of SiH₄ = 28 + 4 = 32
Molar mass of Si₃N₄ = 28 x 3 + 14 x 4 = 84 + 56 = 140 g
Atomic mass of H₂ = 2 g
3(32) g of SiH₄ --------------- 140 g of Si₃N₄
12.5 g of SiH₄ -------------- x
x = 18.2 g of Si₃N₄
3(32) g of SiH₄ --------------- 24 g of H₂
12.5 g of SiH₄ -------------- x
x = 3.125 g of H₂
Electrons are negative protons are positive you remove or add on to the balance is shifted and the electrical charge is changed
The number of molecules of water is calculated as follows
find the moles of water= moles=mass/molar mass
moles = 69.1g/18 g/mol = 3.84 moles
by use of Avogadro law constant
that is 1 mole = 6.02 x10^23 molecules what about 3.84 moles of water
the molecules of water = (3.84 x 6.02 x10^23) = 2.312 x10^24 molecules
