Reactions
Balance the following equation: _FeCl3 + _NaOH --> _Fe(OH)3 + _NaCl
1, 3, 1, 3
Calculate the molar mass of Mg(NO3)2
148.31 g/mol
How many moles of HCl would be produced with 3.17 moles of CH4?
CH4 + 4Cl2 --> CCl4 +4HCl
12.7 mol HCl
If 1.0 mol NiSO4 is dissolved into 1.56 L H2O, what is the molarity of the solution?
0.64 M
In a fixed volume container if the number of collisions between the particles and the walls increases what variable of the ideal gas law is being affected directly
ideal gas law- PV=nRT
pressure
Indicate which metal could react with the following compound, then write the balanced chemical equation: Copper (II) nitrate reacts with
Gold, Zinc, or Platinum
Zn. Cu(NO3)2 + Zn --> Cu + Zn(NO3)2
How many moles are in 46.3 g of C3H4O?
0.826 mol Fe
If we have 2.11 moles of chromium metal reacting, how many grams of chromium (III) oxide (MM = 152 g/mol) will be produced?
4Cr + 3O2 --> 2Cr2O3
160. g Cr2O3
Draw Oxygen Gas's Lewis dot structure
O=O
A sample of Ne at 0.203 atm experiences a change in volume from 34.466 L to 4.756 L. What is the new pressure in atmospheres?
1.47 atm
Write the balanced chemical equation for the combustion of methane (CH4) and oxygen gas.
CH4 + 2O2 --> CO2 + 2H2O
How many atoms are in 67.0 grams of cobalt?
6.85 x 1023 particles
In an experiment, 30.0 g of solid aluminum is reacted with 35.0 g of oxygen gas, and produces 43.9 g of Al2O3. If the theoretical yield is 56.7 g of Al2O3, what is the percent yield of the reaction?
77.4%
In 74 mL of 0.60 M HBr what is the mass in grams of HBr present in the solution?
3.6 g HBr
The temperature of a sample of ClF5 is changed, causing a change in volume from an original volume of 56.3 L to a new volume of 76.64 L. If its new temperature is 1191 K, what was its original temperature in Kelvin?
875 K
Write the balanced chemical equation for the following reaction: Dinitrogen tetrahydride reacts with oxygen gas to produce nitrogen gas and water.
N2H4 + O2 --> N2 +2H2O
A compound is found to contain 23.3% magnesium, 30.7% sulfur, and 46.0% oxygen. What is the empirical formula of this compound?
MgSO3
If 2 NH3 + 3 I2 → N2 + 6 HI
275.8 grams of I2 (MM = 253.8) are reacted with 440 grams of NH3 (MM = 17.04 g/mol), how many grams of N2 (MM = 28.02 g/mol) will be produced?
10.15 g N2
How many grams of silver chromate will be produced when 150. mL of 0.500 M silver nitrate are added to potassium chromate?
2 AgNO3 (aq) + K2CrO4 (aq) --> Ag2CrO4 (s) + 2 KNO3 (aq)
(molar mass of Ag2CrO4 is 331.73 g/mol )
12.4 g Ag2CrO4
The pressure of a 7.21 mol sample of ClO2 in a 76 L container is measured to be 0.4906 atm. What is the temperature of this gas in Celsius?
-210 C
Which reaction happens? Finish it and balance it, including states of matter.
_CuCl2 (aq) + _Zn(NO3)2 (aq) --> ?
_Al2(SO4)3 (aq) + _NH4OH (aq) --> ?
Al2(SO4)3 (aq) + 6NH4OH (aq) -->
2Al(OH)3 (s) + 3(NH4)2SO4 (aq)
Find the molecular formula of a compound that is 87.4% nitrogen and 12.6% hydrogen, and has a molar mass of 32.05 g/mol.
N2H4
Take the reaction: 2 H2 + O2 --> 2 H2O
In an experiment, 68 g of H2 are allowed to react with 212 g of O2 .
How much of the excess reactant remains after the reaction?
(O2 is LR ; H2 is ER)
26.8 grams of H2 are USED
68 g - 26.8 g = 41.2 g H2 are left over
0.060 L of 0.322 M potassium iodide are combined with 0.020 L of 0.530 M lead (II) nitrate. How many grams of lead (II) iodide will be produced?
2 KI (aq) + Pb(NO3)2 (aq) -> 2 KNO3 (aq) + PbI2 (s)
(molar mass of PbI2 is 461.01 g/mol )
4.45 g PbI2
How many grams of chlorine gas must react to produce 16 L of nitrogen gas at 1.2 atm and 23 oC?
2 NH3 (g) + 3 Cl2 (g) ---> N2 (g) + 6 HCl (g)
PV = nRT ; R = 0.0821
170 g Cl2