Chemistry Chapter 11 Test Review

Ms. Sharma

molar mass

the mass of one mole of a substance calculated by adding up the total mass of all elements present in the compound

excess reagent

reactant that isn't used up in a chemical reaction

STP

0°C and 1 atm

reactants

the starting materials in a chemical reaction

product

the final products in a chemical reaction

theoretical yield

amount of product that you would expect for a reaction to yield based on stiochiometric calculations

percent yield

a measure of the efficiency of a reaction performed in the laboratotory

actual yield

amount of product that was collected at the end of an experiment

stoichiometry

the calculation of chemical quantities in chemical equations and is based on law of conservation of mass

mole ratio

determines moles from the coefficients in a balanced chemical equation

molar volume

22.4 L of a gas at STP

1 moles / molar mass

which of the following conversion factors would you use to convert grams to moles

percent yield = actual yield x 100% / theoretical yield

which of the following equations is used to calculate the percentage yield

22.4 L

the molar volume of gas is _____

6.02 x 10^23

1 mole is equivalent to _________ representative particles

coefficients

in a balanced equation the numbers of individual particles and the number of moles of particles are represented by the _____

Zn is the limiting reagent

Given the reaction: Zn + 2HCl → ZnCl2 + H2 

        If  2.0 mol Zn and 5.0 mol HCl are allowed to react ________________________.

4.4 mol

3Cu + 8HNO3 → 3Cu(NO3)2 + 2NO + 4H2O 

Calculate the number of moles of water produced when 3.3 mol of   Cu(NO3)2 are formed in the reaction. 

mass and the number of atoms

In any chemical reaction, the quantities that are conserved are:

0.60 L

How many liters of oxygen are required to react completely with 1.2 L of hydrogen to form water?

2 g S + 3 g O2 - 2 g SO3

Which of these expressions is an incorrect interpretation of the   balanced equation below? 

  

2S(g) + 3O2(g) → 2SO3(g)

83.3%

A reaction that has been calculated to produce 60.0g of CuCl2 actually produces 50.0g of CuCl2. What is the percent yield?

4.0 × 10^ 20

How many molecules of NO2 are produced when 2.0 x 10²⁰  molecules of N2O4 are decomposed according to the following   equation? 

N2O4 → 2 NO2 

is equal to the embassy of the reactants

In a chemical reaction, the mass of the products: