Me
given the reaction, pcl3 + cl2 imported asset pcl5, if 3.00 moles of cl2 are used, then how many moles of pcl5 are made?
6.00 moles
5.00 moles
3.00 moles
1.00 mole
given the reaction, fe2o3 + 3 co imported asset 2 fe + 3 co2, if 12.0 moles of co2 are made, then how many moles of co were used?
12.0 moles
6.0 moles
4.0 moles
3.0 moles
given the reaction, 2 so2 + o2 imported asset 2 so3, if 4 moles of so2 are used, then how many moles of so3 are made?
4 moles
2 moles
1 mole
1/2 mole
using the equation, 4fe + 3o2 imported asset 2fe2o3, if 6 moles of oxygen and an excess of iron were available, how many moles of iron (iii) oxide would be produced?
3 moles
4 moles
5 moles
6 moles
how much volume would 2.00 moles of gas take up, under standard temperature and pressure conditions?
11.2 l
22.4 l
33.6 l
44.8 l
if you have 3.0 liters of an unknown gas, at standard temperature and pressure conditions, then you can calculate what about that gas?
mass
density
moles of representative particles
mass and moles of representative particles
when magnesium metal and an aqueous solution of hydrochloric acid combine, they produce an aqueous solution of magnesium chloride and hydrogen gas. using the equation, mg (s) + 2hcl (aq) imported asset mgcl2 (aq) + h2 (g), if 48.6 g of mg and 150.0 g of hcl are allowed to react, identify the limiting reagent.
mg
hcl
mgcl2
h2
when magnesium metal and an aqueous solution of hydrochloric acid combine, they produce an aqueous solution of magnesium chloride and hydrogen gas. using the equation, mg (s) + 2hcl (aq) imported asset mgcl2 (aq) + h2 (g), if 24.3 g of mg and 75.0 g of hcl are allowed to react, calculate the mass of h2 that is produced.
1.00 g
2.00 g
4.00 g
5.00 g
the limiting reagent is the reactant that is completely consumed in a chemical reaction and limits the amount of product.
true
false
ammonia gas is formed from nitrogen gas and hydrogen gas, according to the following equation: n2 (g) + 3h2 (g) imported asset 2nh3 (g). if 84.0 g of nitrogen gas is allowed to react with an excess of hydrogen gas to produce 85.0 g of ammonia, what is the percent yield of this reaction?
42.2%
65.0%
70.3%
83.3%
red mercury (ii) oxide decomposes to form mercury metal and oxygen gas according to the following equation: 2hgo (s) imported asset hg (l) + o2 (g). if 3.55 moles of hgo decompose to form 1.54 moles of o2 and 618 g of hg, what is the percent yield of this reaction?
13.2%
42.5%
56.6%
86.5%
ammonia gas is formed from nitrogen gas and hydrogen gas according to the following equation: n2 (g) + 3h2 (g) imported asset 2nh3 (g). if 112 grams of nitrogen gas is allowed to react with an excess of hydrogen gas to produce 120 grams of ammonia, what is the percent yield of this reaction?
44.1%
66.2%
88.3%
96.4%
once the percent yield has been determined for a reaction, that percent yield will never vary.
true
false
the theoretical yield for a chemical reaction can not be calculated until the reaction is completed.
true
false