Determine the number of moles of flourine gas that are required to react with 35.45 g of chlorine gas.
What is 1.50 mol
100
Determine the pressure in a sealed 24.1 L flask at 45 degrees C, if it contains a mixture of 20.0 g He and 20.0 g Ne
What is 6.49 atm
100
Write and balance the chemical equation for the reaction between titanium (IV) chloride and water to form titanium (IV) oxide and hydrochloric acid. What is the coefficient in front of HCl?
What is 4
100
How many moles of NaCl form when 1.50 moles of FeCl3 react with 3.00 moles of NaOH, according to the following reaction
FeCl3(aq) + 3NaOH(aq) ---> Fe(OH)3(s) + 3 NaCl(aq)
What is 3.00 mol NaCl
100
A gas mixture contains 25.5 percent Ar. if the total pressure of the gas mixture is 850.0 mm Hg, what is the partial pressure of Ar?
What is 217 mm Hg
200
Determine the mass of S that forms when 4.22 moles of H2S and 2.55 x 10^23 molecules of SO2 react
2H2S(g) + SO2(g) ---> 3S(s) + 2H2O(g)
What is 40.7 g
200
Determine the mass of a gaseous methane (CH4) sample that has a volume of 295 mL at STP.
What is 0.211 g
200
Complete the reaction, if one occurs. what are the products if any?
H2SO4(aq) + K2CO3(aq) ---->
What is H20, CO2 and K2SO4
200
A sealed, 6.70 L vessel containing CH4 has a pressure of 1.55 atm. if the temperature of the vessel is 288 K, how many moles of CH4 are within the vessel?
What is 0.439 mol CH4
200
Which of the following substances are insoluble in water?
Ag2SO4, CaS, MgSO4, PbS
What is PbS
300
Determine the percent yield if 3.50 g of B form when 1.50 moles of B2O3 react with 14.9 g of Mg.
B2O3(s) + 3Mg(s) ---> 2 B(s) + 3MgO(s)
What is 79.2 percent
300
The total pressure in a 15.5 L sealed flask is 2.75 atm at 35 degrees C. how much does the pressure in the flask rise if it is warmed to a temperature of 55 degrees C and the volume remains 15.5 L?
What is 0.18 atm
300
Determine the net ionic equation (if any) that occurs when aqueous solutions of (NH4)3PO4 and BaCl are mixed.
What is 3Ba^2+(aq) + 2PO4^3-(aq) ----> Ba3(PO4)2 (s)
300
Which of the following gas samples would have the smallest volume if they were all at the same pressure and temperature?
4.00 mol He, 20.2 mol Ne, 40.0 mol Ar, 83.8 mol Kr
What is 4.00 mol He
300
In the balanced chemical reaction between aluminum metal and fluorine gas to form aluminum fluoride, what is the coefficient in front of the aluminum?
What is 2
400
What mass of aluminum metal must react with MnO2 in order to release 3.60 x 10^3 kJ of heat, according to the equation below?
4Al(s) + 3MnO2(s) ---> 2Al2O3(s) + 3Mn(s) Hrxn=-1792kJ
What is 2.17 x 10^2 g Al
400
What volume (in L, at 25 degrees C, and 1.20 atm) of nitrogen gas is required to form 17.8 g of Li3N?
6Li(s) + N2(g) ---> 2Li3N(s)
What is 5.21 L
400
What type of reaction is this?
Fe(s) + 2HCl(g) ---> H2(g) + FeCl2(s)
What is Oxidation-reduction
400
I have a piece of potassium metal that has a mass of 18.9 g. When I fully react the potassium with excess phosphorus (P4), a white, solid product forms. What is the mass of P4 that reacted? the unbalanced chemical reation is given below.
K(s) + P4(s) ---> K3P(s)
What is 0.499 g P4
400
The reaction between iron metal and solid phosphorus to form iron(III) phosphide is an example of what type of reaction?
4Fe(s) + P4(s) ----> 4FeP(s)
What is Oxidation-Reduction
500
How many grams of solid form when 6.71 g of aq CaCl2 and 8.22 g of aq K3PO4 react?
What is 6.01 g
500
Determine the pressure (in atm) of gas that remains after 34.8 g Al reacts with 44.9 g O2 according to the following reaction. The reaction takes place in a 5.00 L sealed container at 285 K. (assume 100% yield)
What is 2.02 atm
500
Which of the following statements about the thermochemical equation below is true
N2(g) + O2(g) ---> 2NO(g) Delta Hrxn = 180.6 kJ
1) the reaction is exothermic
2) for every mole of NO gas formed, 90.3 kJ of heat are absorbed.
3)For every mole of N2 gas reacted 180.6 kJ of heat are given off.
4) For every mole of O2 gas reacted, 90.3 kJ of heat are absorbed.
What is 2
500
HCl reactis with Ni(s) to form nickle(II) chloride(aq) and H2 gas. I completely react 10.2 g of HCl some Ni metal and collect the gaseous product in a vessel (2.5 L, 313K) what is the pressure in the vessel?
What is 1.44 atm
500
Which of the following reactions is an oxidation- reduction reaction?
1) 2HBr(aq)+ Pb(s) ---> PbBr2(s) + H2(g)
2) NH4Cl(aq) + AgNO3 (aq) ---> AgCl(s) + NH4Cl (aq)
3) LiOH(aq) + HCl(aq) ---> H2O(l) + LiCl (aq)