The fuel used to power the booster rockets on the space shuttle is a mixture of aluminum metal and ammonium perchlorate. The following balanced equation represents the reaction of these two ingredients:

$$3 \mathrm { Al } ( s ) + 3 \mathrm { NH } _ { 4 } \mathrm { ClO } _ { 4 } ( s ) \longrightarrow \mathrm { Al } _ { 2 } \mathrm { O } _ { 3 } ( s ) + \mathrm { AlCl } _ { 3 } ( g ) + 3 \mathrm { NO } ( g ) + 6 \mathrm { H } _ { 2 } \mathrm { O } ( g )$$

.a If

$$1.50 \times 10 ^ { 5 } g$$

of Al react, what mass of

$$\mathrm { NH } _ { 4 } \mathrm { ClO } _ { 4 }$$

, in grams, is required? b. If aluminum reacts with 620 kg of

$$\mathrm { NH } _ { 4 } \mathrm { ClO } _ { 4 }$$

, what mass of nitrogen monoxide is produced?

Calcium carbonate found in limestone and marble reacts with hydrochloric acid to form calcium chloride, carbon dioxide, and water according to the following equation:

$$\mathrm { CaCO } _ { 3 } ( s ) + 2 \mathrm { HCl } ( a q ) \longrightarrow \mathrm { CaCl } _ { 2 } ( a q ) + \mathrm { CO } _ { 2 } ( g ) + \mathrm { H } _ { 2 } \mathrm { O } ( l )$$

a. What mass of HCl will be needed to produce

$$5.00 \times 10 ^ { 3 } \mathrm { kg }$$

of

$$\mathrm { CaCl } _ { 2 } ?$$

b. What mass of

$$CO_2$$

could be produced from the reaction of 750 g of

$$\mathrm { CaCO } _ { 3 } ?$$

Phosphoric acid is typically produced by the action of sulfuric acid on rock that has a high content of calcium phosphate according to the following equation:

$$3 \mathrm { H } _ { 2 } \mathrm { SO } _ { 4 } + \mathrm { Ca } _ { 3 } \left( \mathrm { PO } _ { 4 } \right) _ { 2 } + 6 \mathrm { H } _ { 2 } \mathrm { O } \rightarrow 3 \left[ \mathrm { CaSO } _ { 4 } \cdot 2 \mathrm { H } _ { 2 } \mathrm { O } \right] + 2 \mathrm { H } _ { 3 } \mathrm { PO } _ { 4 }$$

a. If

$$2.50 \times 10 ^ { 5 } \mathrm { kg }$$

of

$$H_2SO_4$$

react, how many moles of

$$\mathrm { H } _ { 3 } \mathrm { PO } _ { 4 }$$

can be made? b. What mass of calcium sulfate dihydrate is produced by the reaction of 400. kg of calcium phosphate? c. If the rock being used contains 78.8%

$$\mathrm { Ca } _ { 3 } \left( \mathrm { PO } _ { 4 } \right) _ { 2 }$$

, how many metric tons of

$$H_3PO_4$$

can be produced from 68 metric tons of rock?

Potassium permanganate and glycerin react explosively according to the following equation:

$$14 \mathrm { KMnO } _ { 4 } + 4 \mathrm { C } _ { 3 } \mathrm { H } _ { 5 } ( \mathrm { OH } ) _ { 3 } \longrightarrow \mathrm { 7K } _ { 2 } \mathrm { CO } _ { 3 } + 7 \mathrm { Mn } _ { 2 } \mathrm { O } _ { 3 } + 5 \mathrm { CO } _ { 2 } + 16 \mathrm { H } _ { 2 } \mathrm { O }$$

a. How many moles of carbon dioxide can be produced from 4.44 mol of

$$\mathrm { KMnO } _ { 4 } ?$$

b. If 5.21 g of

$$H_2O$$

are produced, how many moles of glycerin,

$$\mathrm { C } _ { 3 } \mathrm { H } _ { 5 } \left( \mathrm { OH } _ { 3 } \right)$$

, were used? c. If 3.39 mol of potassium carbonate are made, how many grams of manganese(III) oxide are also made? d. How many grams of glycerin will be needed to react with 50.0 g of

$$\mathrm { KMnO } _ { 4 } ? \mathrm { H }$$

How many grams of

$$CO_2$$

will be produced in the same reaction?

Ammonium hydrogen phosphate,

$$\left( \mathrm { NH } _ { 4 } \right) _ { 2 } \mathrm { HPO } _ { 4 }$$

, a common fertilizer; is made from reacting phosphoric acid,

$$\mathrm { H } _ { 3 } \mathrm { PO } _ { 4 }$$

, with ammonia. a. Write the equation for this reaction. b. If 10.00 g of ammonia react, how many moles of fertilizer will be produced? c. What mass of ammonia will react with 2800 kg of

$$\mathrm { H } _ { 3 } \mathrm { PO } _ { 4 } ?$$

Sodium sulfide and cadmium nitrate undergo a double-displacement reaction as shown by the following equation:

$$\mathrm { Na } _ { 2 } \mathrm { S } + \mathrm { Cd } \left( \mathrm { NO } _ { 3 } \right) _ { 2 } \rightarrow 2 \mathrm { NaNO } _ { 3 } + \mathrm { CdS }$$

What is the mass, in milligrams, of cadmium sulfide that can be made from 5.00 mg of sodium sulfide?

Rusting of iron occurs in the presence of moisture according to the following equation:

$$4 \mathrm { Fe } ( s ) + 3 \mathrm { O } _ { 2 } ( g ) \longrightarrow 2 \mathrm { Fe } _ { 2 } \mathrm { O } _ { 3 } ( s )$$

Suppose that 3.19% of a heap of steel scrap with a mass of 1650 kg rusts in a year. What mass will the heap have after one year of rusting?

Which expression is equivalent to

$$( - 9 ) ^ { 6 }$$

? (A)

$$( - 9 ) ^ { 2 } ( - 9 ) ^ { 3 }$$

(B)

$$( - 9 ) ( - 9 ) ^ { 5 }$$

(C)

$$\left[ ( - 9 ) ^ { 4 } \right] ^ { 2 }$$

(D)

$$\left[ ( - 9 ) ^ { 3 } \right] ^ { 3 }$$

Joseph Priestley is credited with the discovery of oxygen. He produced

$$O_2$$

by heating mercury(II) oxide, HgO, to decompose it into its elements. How many moles of oxygen could Priestley have produced if he had decomposed 517.84 g of mercury oxide?

193. Iron(III) chloride,

$$\mathrm { FeCl } _ { 3 }$$

, can be made by the reaction of iron with chlorine gas. How much iron, in grams, will be needed to completely react with 58.0 g of

$$\mathrm { Cl } _ { 2 } ?$$

Lead(II) nitrate reacts with potassium iodide to produce lead(II) iodide and potassium nitrate. If 1.23 mg of lead nitrate are consumed, what is the mass of the potassium nitrate produced?

Write an equation to show how sulfuric acids in acid rain reacts with marble and limestone. (Both marble and limestone are primarily calcium carbonate.)

The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel. A possible reaction is

$$3 \mathrm { Al } ( s ) + 3 \mathrm { NH } _ { 4 } \mathrm { ClO } _ { 4 } ( s ) \longrightarrow \mathrm { Al } _ { 2 } \mathrm { O } _ { 3 } ( s ) + \mathrm { AlCl } _ { 3 } ( s ) + 3 \mathrm { NO } ( g ) + 6 \mathrm { H } _ { 2 } \mathrm { O } ( g )$$

Calculate $\Delta H ^ { \circ }$ for this reaction.

Solve the equation.

$$3^x+4=6^2x-5$$