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Chapter 7: Q. 7.96 (page 255)

How many moles are in $4.00$ gof each of the following compounds? ( $7.3$ )
a. ${NH}_{3}$
b. $Ca {({NO}_{3})}_{2}$
c. ${SO}_{3}$

Short Answer

Expert verified

(a) The no. of moles of ${NH}_{3}$ in localid="1653468385200">4.00gare localid="1653468399534" $0.235$ mole

(b) The no. of moles of $Ca {({NO}_{3})}_{2}$ in localid="1653468422965" $4.00$ gare localid="1653468436007">0.024mole

(c) The no. of moles of ${SO}_{3}$ inlocalid="1653468450392" $4.00$ gare localid="1653468463717" $0.05$ mole

Step by step solution

01

Part (a) Step 1: Given information

We need to find no. of moles in given compound i.e. $N H_{3}$

02

Part (a) Step 2: Explanation

We know that

Molar mass of ${NH}_{3}$ is localid="1653484364686" $17 g / mole$

And molar mass is equal to a mole

Therefore,

localid="1653484377668" $17 g = 1 mole 4.00 g = \frac{1 mole}{17 g} 脳 4 g = 0.235 mole$

03

Part (b) Step 1: Given information

We need to find no. of moles in given compound i.e. $Ca {({NO}_{3})}_{2}$

04

Part (b) Step 2: Explanation

We know that

Molar mass of $Ca {({NO}_{3})}_{2}$ islocalid="1653484404438" $164 g / mole$

And molar mass is equal to a mole

Therefore,

localid="1653484416853" $164 g = 1 mole 4.00 g = \frac{1 mole}{164 g} 脳 4 g = 0.024 mole$

05

Part (c) Step 1: Given information

We need to find no. of moles in given compound i.e. ${SO}_{3}$

06

Part (c) Step 2: Explanation

We know that

Molar mass of ${SO}_{3}$ is localid="1653484445634" $80 g / mole$

And molar mass is equal to a mole

Therefore,

localid="1653484459957" $80 g = 1 mole 4.00 g = \frac{1 mole}{80 g} 脳 4.00 g = 0.05 mole$

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Most popular questions from this chapter

a. Why do chemical reactions require energy of activation ?

b. In an exothermic reaction, is the energy of the products higher or lower than that of the reactants?

c. Draw an energy diagram for an exothermic reaction.

When ammonia ( ${NH}_{3}$ ) gas reacts with fluorine gas, the gaseous products are dinitrogen tetrafluoride ( $N_{2} F_{4}$ ) and hydrogen fluoride ( $HF$ ). ( $7.4, 7.7, 7.8$ )

a. Write the balanced chemical equation.

b. How many moles of each reactant are needed to produce localid="1653469855463" $4.00$ moleof $HF$ ?

c. How many grams of $F_{2}$ are needed to react with localid="1653469902894" $25.5$ gof ${NH}_{3}$ ?

d. How many grams of $N_{2} F_{4}$ can be produced when localid="1653469925977" $3.40$ gof ${NH}_{3}$ reacts?

Balance each of the following chemical equations, and identify the type of reaction: ( $7.4, 7.5$ )

a. ${Si}_{3} N_{4} (s) 鈫� Si (s) + N_{2} (g)$

b. $Mg (s) + N_{2} (g) 鈫� {Mg}_{3} N_{2} (s)$

c. $Al (s) + H_{2} {PO}_{4} (aq) 鈫� H_{2} (g) + {AIPO}_{4} (aq)$

d. $C_{3} H_{4} (g) + O_{2} (g) 鈫� {CO}_{2} (g) + H_{2} O (g)$

e. ${Cr}_{2} O_{3} (s) + H_{2} (g) 鈫� Cr (s) + H_{2} O (g)$

f. $Al (s) + {Cl}_{2} (g) 鈫� {AlCl}_{3} (s)$

g. ${MgCl}_{2} (aq) + {AgNO}_{3} (aq) 鈫� AgCl (s) + Mg {({NO}_{3})}_{2} (aq)$

When solid lead(II) sulfide reacts with oxygen gas, the products are solid lead(II) oxide and sulfur dioxide gas.

a. Write the balanced chemical equation for the reaction.

b. How many grams of oxygen are required to react with $29.9 g$ of lead(II) sulfide?

c. How many grams of sulfur dioxide can be produced when $65.0 g$ of lead(II) sulfide reacts?

d. How many grams of lead(II) sulfide are used to produce $128 g$ of lead(II) oxide?

Determine whether each of the following chemical equations are balanced or not balanced:

a. $P C l_{3} (s) + C l_{2} (g) 鈫� P C l_{5} (s)$

b. $C O (g) + 2 H_{2} (g) 鈫� C H_{4} O (g)$

c. $2 K C l O_{3} (s) 鈫� 2 K C l (s) + O_{2} (g)$

d. $M g (s) + N_{2} (g) 鈫� M g_{3} N_{2} (s)$

See all solutions

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