Interpretation:
Given the molar mass of
Concept Introduction:
Sum of atomic masses of all the atoms that are represented in chemical formula of substance is known as formula mass. If
Molar mass is the mass that is expressed in grams of a substance that is equal to the formula mass of the substance numerically. Molar mass of an element is unique for the particular element. Two natural elements can never have the same molar mass.
Mole is defined as the amount of substance that has as many elementary particles as there are atoms in exactly 12 grams of
The relationship between the atomic mass unit and grams unit is,
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General, Organic, and Biological Chemistry
- The problem How many grams of O2 are needed to produce 2.00 moles of H2O via the chemical reaction 2H2 + O2 2H2O? is characterized as a a. moles of A to grams of A problem b. grams of A to moles of B problem c. moles of A to grams of B problem d. no correct responsearrow_forwardWhich of the following is the correct conversion factor setup for the problem How many grams of H2O can be produced from 3.2 moles of O2 and an excess of H2S via chemical reaction 2H2S + 3O2 2H2O + 2SO2? a. 3.2molesO2(32.00gO21moleO2)(18.02gH2O32.00gO2) b. 3.2molesO2(2molesH2O3MolesO2)(18.02gH2O1moleH2O) c. 3.2molesO2(32.00gO21moleO2)(2molesH2O3MolesO2) d. no correct responsearrow_forwardWhich of the following chemical formulas fits the description number of elements present and number of atoms present are the same? a. HClO2 b. C2H2Cl2 c. H2O2 d. no correct responsearrow_forward
- The number of atoms present in 1 mole of P atoms is a. 6.02 1021 b. 6.02 1023 c. 6.02 1025 d. no correct responsearrow_forwardercise 9.1 Calculate the moles of CO2formed when 4.30 moles of C3H8reacts with the required 21.5 moles of O2. NT Use the moles of C3H8, and obtain the mole ratio between C3H8and CO2from the balanced equation.arrow_forwardHow many conversion factors are needed in solving a particles of A to grams of B problem? a. one b. two c. three d. no correct responsearrow_forward
- Answer key show work #35i 1.85 moles H2SO4 #35j 0.00836 moles of Ca3(PO4)2 molecules #35k 1.3333 moles H3PO4 (answer corrected 10/9/19) #35l 130.67 g H3PO4 (answer corrected 10/9/19)arrow_forwardTrial #1: A piece of magnesium with a mass of 0.330 grams was placed into a solution of hydrochloric acid. 335 mL of hydrogen gas were produce when this reaction occurred at 22.0 °C and a pressure of 747.0 mmHg. Mg(s) + 2HCl(aq) ⟶⟶ H2(g) + MgCl2(aq) Calculate the molar volume (liters/mole) of hydrogen for Trial #1?arrow_forward
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