1. What is the molecular mass of P2Cl5 in amu?

1. What is the molecular mass of P2Cl5 in amu?

(Please give your answer to the second decimal place)

2. The molar mass of ammonium phosphate is

3. The mass of 0.94 mol of H2 is _____.

4. A mole can be defined as the number equal to the number of oxygen atoms in 32.00 g of oxygen. Is this statement true or false?

5. 38.6 g of Cr represents how many atoms?

6. What is the mass of 1.36 x 1022 molecules of HCl?

7. How many nitrogen atoms are indicated by the formula Ca(NO3)2 ?

8. How many total atoms are present in 0.140 g of HCl?

9. How many grams of O are in 3.70 moles of H2SO4?

10. Calculate the molar mass of a sample if a single molecule weighs 9.31 × 10–23 g.

11. The mass percent of hydrogen in NH4Br is _____.

12. A 10.00 g sample of a substance is found to contain 5.12 g of water. What is the percent by mass of water in the compound?

13. In which pair would both compounds have the same empirical formula?

14. A 65.2 g sample of a compound contains 32.1 g of phosphorus and the rest is oxygen. What is the empirical formula of the compound?

15. A compound contains 25.94% N and 74.06% O (by mass). What is the empirical formula?

16. The empirical formula for acetic acid is CH2O. Its molar mass is 60 g/mol. The molecular formula is

17. A certain compound is found to have the percent composition (by mass) of 85.63% C and 14.37% H. The molecular formula contains 6 carbon atoms. How many hydrogen atoms are contained in a molecular of this compound?

18. A 0.266-g sample of NaCl (molar mass = 58.44 g/mol) is dissolved in enough water to make 5.20 mL of solution. Calculate the molarity of the resulting solution.

19. What is the minimum volume of a 2.31 M NaOH solution needed to make 150.0 mL of a 0.800 M NaOH solution?

20. The total mass of a solution is 159.0 g. The solvent mass is 125.2 g. What is the mass percent of the solute?

21. What is the concentration, in ppm, if 0.683 grams of CaCl2 is dissolved in 332 ml of water.

Note: the density of water is 1 g/ml.

Please express your answer as a whole number

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