2017年8月10日 · 78.114 "g/mol" To find the molar mass of a compound, we first look at a periodic table to find the molar masses of each element in the compound: The chemical formula for benzene is ul("C"_6"H"_6 So we need only look at the values for carbon and hydrogen. We find that the molar masses are "C": 12.01 "g/mol" "H": "1.01 "g/mol" We need to multiply these …

Question: What is the molar mass of toluene if 0.85 g of toluene depresses the freezing point of 100. g of benzene by 0.47°C?

Calculate the molar mass of a compound if 0.457 moles of it has a mass of 223 grams. What is the total number of all atoms in 4.24 grams of benzene? Calculate the molar mass of Ca3(PO4)2. Calculate the number of atoms of each element present in 0.000221 g of benzene, C6H6. Calculate the molar mass of Eugenol.

When we burn (i.e., combust) 10.0 mL of benzene in air, our theoretical yield for water would be ml> (use 18.02 g/mol and 1.00 g/mL as molar mass and density for water). The molecular weight of a gas that has a density of 1.23 g/L at standard temperature and pressure is Given that R-0.08206 Latm/molk.

Question: 10. Benzene, an organic solvent, has the empirical formula CH. If the molar mass of benzene is 78.11 g/mol, what is the molecular formula of benzene?

The normal freezing point of benzene, C6H6 (molar mass = 72.12 g/mol), is 5.5 °C. What is the freezing point of a solutions prepared by dissolving 10.5 grams of biphenyl, C12H10 (molar mass = 154.22 g/mol) into 50.0 grams benzene?

2018年6月28日 · molecular formula for benzene = C_6H_6 acetylene = C_2H_2 Since the question already gave the empirical formula for both compounds, which is CH. Let's figure out the subscript, n, in (CH)_n for their molecular formulas. To do so, let's use the molar mass and divide by the formula mass of the empirical formula, CH, 12 + 1 = 13 g. For benzene: "subscript, n" = …

What is the molar mass of a nonpolar molecular compound if 3.42 grams dissolved in 41.8 grams benzene begins to freeze at 1.17 o C? The freezing point of pure benzene is 5.50 o C and the molal freezing point constant, K f,is -5.12 o C/m.

What volume of benzene (C6H6, d= 0.88 g/mL, molar mass = 78.11 g/mol) is required to produce 1.5x 103 kJ of heat according to the following reaction? 2 CyH6(1) + 15 O2(g) → 12 CO2(g) + 6 H2O(g) AH°rxn = -6278 kJ 19 mL 37 mL 75 mL 42 mL 21 mL Determine the final temperature of a gold nugget (mass = 376 g) that starts at 398 K and loses 4.85 kJ of heat to a snowbank when …

Pure benzene, C6H6, has a molar mass of 78.114 g mol-¹, a density of 0.8765 g mL-1, a freezing point of 5.45°C, and a boiling point of 80.2°C. Its freezing point depression and boiling point elevation constants are: K₁=5.07°C m¹; Kb = 2.53°C m 1.