Chapter 5-6 Test Math

Question 1

In the formation of C2H4O, how many moles of C are required to make 15 moles of C2H4O?

Answer 1

3.0 ~10 to the 1 moles C

Question 2

What is the balanced chemical equation for the combustion of C16H34?

Answer 2

2C16H34 +49O2 —> 32CO2+ 34H2O

Question 3

What is the mass of a CaCl2 sample if it contains 0.172 moles of the compound?

Answer 3

19.1g Cacl2

Question 4

How many grams are contained in a 4.51 mole sample of CO2?

Answer 4

198g CO2

Question 5

How many moles of H2CO3 are in a 125 gram sample of the compound?

Answer 5

2.02 moles H2CO3

Question 6

Nitric acid is manufactured with the following reaction: 3NO2+ H2O r —> 2HNO3 + NO
How many grams of nitrogen dioxide are required to produce 5.89x10 to the 6th kg HNO3 in excess water?

Answer 6

6.44 ~ 10 to the 4th g NO2

Question 7

Carbon tetrachloride is made according to the following reaction: CS2 + 3Cl2 —> CCl4+ S2Cl2
How much CS2 is needed to make 16 kg of CCl4?

Answer 7

1.0 ~ 10 the the 2nd moles of CS2

Question 8

Decomposition of 100.0 g of a dark green powder yields 39.7 g K, 27.9 g Mn, and an unknown
amount of oxygen. What is the empirical formula?

Answer 8

K2MNO4

Question 9

A compound has an empirical formula of CH2O. If its molecular mass is 60.0 amu, what is its
molecular formula?

Answer 9

C2H4O2

Question 10

To make a phosphorus fertilizer (CaH4P2O8), agricultural companies use the following reaction: Ca3P2O8 + 2H2SO4 + 4H2O → CaH4P2O8 + 2CaH4SO6
If 2.50x103 grams of Ca3P2O8 are reacted with excess H2SO4 and H2O, how many grams of fertilizer can be made?

Answer 10

1,890 g CaH4P2O8