Stochiometry

___NH3 + ___O2 → ___NO2 + ___H2O

The balanced equation shows that 1.00 mole of NH3 requires ___ mole(s) of O2

• 0.57

• 1.25

• 1.33

• 1.75

Write a balanced equation for the combustion of acetaldehyde. The equation indicates that ___ mole(s) of O2 are required for each mole of it.

• 1

• 2

• 2.5

• 3

• 5

What is the total mass of products formed when 16 grams of CH4 is burned with excess oxygen?

• 32 g

• 36 g

• 44 g

• 62 g

• 80 g

Balance the following equation with the SMALLEST WHOLE NUMBER COEFFICIENTS possible. Select the number that is the sum of the coefficients in the balanced equation: ___KClO3 → ___KCl + ___O2

• 3

• 5

• 6

• 7

• 8

Calculate the mass of hydrogen formed when 27 g of aluminum reacts with excess hydrochloric acid according to the balanced equation below. 2Al + 6HCl → 2 AlCl3 + 3 H2

• 1.5 g

• 2.0 g

• 3.0 g

• 6.0 g

• 12 g

Tags

NGSS.HS-PS1-7

How many grams of nitric acid, HNO3, can be prepared from the reaction of 138 g of NO2 with 54.0 g H2O according to the equation below?

3NO2 + H2O → 2HNO3 + NO

• 92

• 108

• 126

• 189

• 279

Which of the following statements is true?

• I. The molar mass of CaCO3 is 100.1 g mol−1.

• II. 50 g of CaCO3 contains 9 ×1023 oxygen atoms.

• III. A 200 g sample of CaCO3 contains 2 moles of CaCO3

• None of them

The reaction of 7.8 g benzene, C6H6, with excess HNO3 resulted in 0.90 g of H2O. What is the percentage yield? Molar Mass (g/mol):

C6H6=78 HNO3=63 C6H5NO2=123 H2O=18

C6H6 + HNO3 → C6H5NO2 + H2O

• 100%

• 90%

• 50%

• 12%

• 2%

How many grams of H2O will be formed when 32.0 g H2 is allowed to react with 16.0 g O2 according to

2 H2 + O2 → 2 H2O

• 9.00 g

• 16.0 g

• 18.0 g

• 32.0 g

• 36.0 g

When 2.00 g of H2 reacts with 32.0 g of O2 in an explosion, the final gas mixture will contain:

• H2, H2O, and O2

• H2 and H2O only

• O2 and H2O only

• H2 and O2 only

• H2O only