Calculate the molar mass of tetraphosphorus decaoxide, P4O10, a corrosive substance which can be used as a drying agent. 469.73 g/mol 139.88 g/mol 190.97 g/mol 283.89 g/mol
If 119.3 g of PCl5 are formed from the reaction of 61.3 gCl2 with excess PCl3, what is the percent yield? PCl3(g) + Cl2(g) → PCl5(g) 66.3% 48.6% 57.3% 94.6% 51.3%
How many grams of water could be made from 5.0 mol H2 and 3.0 mol O2? 42 g 45 g 36 g 90. g 108 g
For the equation below: Mg(s) + 2HCl(aq) ⟶ MgCl2(aq) + H2(g) (a) How many moles of hydrogen will be liberated from 177.6 mL of 4.94 M HCl reacting with an excess of magnesium? mol H2 (b) How many liters of hydrogen gas (H2) measured at 24∘C and 733 torr will be obtained? L H2
Calculate the number of moles of an ideal gas if it has a pressure of 1.453 atm, a volume of 14.9 L, and a temperature of 84.2∘C a. The number of moles is 0.00840 mol b. The number of moles is 0.0309 mol c. The number of moles is 0.00729 mol d. The number of moles is 3.13 mol e. The number of moles is 0.738 mol
A 4.30 L container had 33.40 moles of N2O4 added to it. When equilibrium was established, the concentration of NO2 was found to be 2.67 M. What is Kc for the following reaction N2O4(g) ↔ 2NO2(g) 0.997 M 0.415 M 0.942 M 0.374 M 0.353 M 1.108 M
3 Cd + 2 Al(NO3)3 → 3 Cd(NO3)2 + 2 AI If 1.638 moles of Cd(NO3)2 are produced, how many grams of AI(NO3)3 (molar mass 213 g/mol) were reacted?
Consider the balanced reaction: 2H2S + SO2 −− > 3S + 2H2O How many moles of H2S are needed to produce 10.5 g of elemental sulfur (S) from the above reaction? You can assume 100% of the H2S will react as described by the reaction above. ×10^ moles of H2S
A 5.3644 g sample of an unknown hydrate of cobalt(II) bromide is heated until all the water of How many moles of CoBr2 are in the sample? mol How many grams of water were lost in the dehydration? g How many moles of water were lost? (mol) What is the value of "n" in the formula CoBr2⋅nH2O? (1, 2, 3, 4…).
A fuel oil is analyzed and found to contain 83.86 wt% carbon, 13.82% elemental hydrogen (H), 1.57% sulfur, and the remainder noncombustible matter. The oil is burned with 7.5% excess air, based on complete combustion of the carbon to CO2, the hydrogen to H2O, and the sulfur to SO2. The oil is burned completely, but 8.00% of the carbon forms CO. Calculate the molar composition of the stack gas. You may take the composition of air to be 79.0 mole% N2 and 21.0 mole% O2. yN2 = yO2 = yH2O = yCO = yCO2 = ySO2 =