ChemistryWiki | RecentChanges | Preferences
Difference (from prior author revision)
(major diff, minor diff)
Changed: 35c35
Removed: 85,88d84
Part III Answer the following question showing all work
a. A compound consists of 17.6% sodium (Na), 39.7% chromium (Cr), and 42.7% oxygen (O). What is the empirical formula (EF)?
|
Added: 91a88
Added: 93a91
Part III Answer the following questions showing all work.
|
Added: 94a93
a) How many liters (@STP) do I have if I mass out 42.7 grams of elemental nitrogen gas (N2)?
|
Added: 100a100
Added: 105a106
Removed: 111d111
b. A molecular compound consists of 54.5% C, 13.6% H and 31.8% N. The molar mass of the compound is 176g/mole. What is the empirical formula (EF) and molecular formula (MF).
|
Added: 114a115
b) How many molecules in 94.5 grams of carbon dioxide?
|
Added: 121a123
Added: 127a130
Added: 130a134
Removed: 137d140
Part IV Answer the following questions showing all work.
|
Removed: 139d141
a) How many grams in 23.7 liters of chlorine gas (Cl2) @ STP?
|
Added: 140a143
c) How many atoms of Ne do I have if I have 61.5 L @ STP of this gas?
|
Added: 151a155
Changed: 161c165
b) How many molecules in 24.5 grams of water?
|
d) How many f.u. (formula units) of Barium nitrite do I have if I massed out 82.1g of this compound?
|
Added: 179a184,187
Removed: 183d190
c) How many f.u. do I have if I have 14.5grams of aluminum chloride?
|
Added: 185a193
Added: 187a196
Changed: 189c198,200
Part IV Answer the following question showing all work
a. A compound consists of 17.6% sodium (Na), 39.7% chromium (Cr), and 42.7% oxygen (O). What is the empirical formula (EF)?
|
Removed: 196d206
Removed: 205d214
d) How many liters of N2 in 3.4E24 molecules of this gas.
(The element N is not found alone in nature but instead as in two's so it is actually a molecule)
|
Changed: 213c222,229
b. A molecular compound consists of 54.5% C, 13.6% H and 31.8% N. The molar mass of the compound is 176g/mole. What is the empirical formula (EF) and molecular formula (MF).
|
Removed: 220d235
Removed: 224d238
Removed: 226,227d239
Answer: Part III a. Na2(Cr2O7)1, b. {C8H24N4,C2H6N1}
Part IV a. 75.1g Cl2 @STP, b. 8.19E23 molecules H2O, c. 6.51E22 f.u. Al1Cl3, d. 130L (or 1.3E2L) N2 @STP
|
Added: 228a241,261
Answer:
Part I : Can't show without giving answer
Part II : Can't show without giving answer
Part III :
a. 34.2 L N2 @STP
b. 1.29E24 molecules C1O2
c. 1.65E24 atom Ne
d. 2.16E23 f.u. Ba1(NO2)2
Part IV :
a. Na2(Cr2O7)1
b. C8H24N4 and C2H6N1
|
Part I Please write the appropriate chemical formula or chemical name for the following. Make sure to give symbols & charges of each ion before writing correct chemical formula.
a) Trichlorine octabromide
b) Fe2(H1P1O3)3
c) Ammonium carbonate
d) Silicon monophosphide
e) O1Br5
f) Cobalt (III) sulfate
g) Cu1(C2O4)1
h) Silver nitrate
i) Zn3(P1O4)2
j) N2Cl2
Part II Show the symbol and charge for each ion, correct chemical formula and LDS for the following Ionic Compound
a. Potassium sulfide
b. Aluminum chloride
c. Calcium phosphide
Part III Answer the following questions showing all work.
a) How many liters (@STP) do I have if I mass out 42.7 grams of elemental nitrogen gas (N2)?
b) How many molecules in 94.5 grams of carbon dioxide?
c) How many atoms of Ne do I have if I have 61.5 L @ STP of this gas?
d) How many f.u. (formula units) of Barium nitrite do I have if I massed out 82.1g of this compound?
Part IV Answer the following question showing all work
a. A compound consists of 17.6% sodium (Na), 39.7% chromium (Cr), and 42.7% oxygen (O). What is the empirical formula (EF)?
b. A molecular compound consists of 54.5% C, 13.6% H and 31.8% N. The molar mass of the compound is 176g/mole. What is the empirical formula (EF) and molecular formula (MF).
Answer:
Part I : Can't show without giving answer
Part II : Can't show without giving answer
Part III :
a. 34.2 L N2 @STP
b. 1.29E24 molecules C1O2
c. 1.65E24 atom Ne
d. 2.16E23 f.u. Ba1(NO2)2
Part IV :
a. Na2(Cr2O7)1
b. C8H24N4 and C2H6N1