Q: How many molecules are present in 0.113 mol of glucose ($$C_6H_{12}O_6$)?

$$6.8 \times 10$$^{22}$$ molecules

Question 1

How many molecules are present in 0.113 mol of glucose ($$C_6H_{12}O_6$)?

Accepted Answer

$$6.8 	imes 10$$^{22}$$ molecules

Question 2

You have 0.0015 moles of sodium carbonate ($$Na_2CO_3). $$How many moles of sodium atoms do you have?

Accepted Answer

$$0.0030$$ moles

Question 3

A balanced equation for the formation of a s'more is: 1 cracker + 1 marshmallow + $$\frac{1}{2}$$ chocolate bar $$\rightarrow 1 s$$'more. If you have 10 crackers, 10 marshmallows, and 5 chocolate bars, what is the maximum number of s'mores you can make?

Accepted Answer

$$5 s$$'mores

Question 4

Given the reaction $$2NH_3(g) \rightarrow N_2$(g) + 3H_2(g)$$, how many moles of hydrogen gas are formed from 4 moles of ammonia, assuming complete reaction?

Accepted Answer

$$6$$ moles

Question 5

Ammonium nitrate decomposes according to $$NH_4NO_3(s) \rightarrow 2N_2(g) + O_2$(g) + 4H_2O(g). If $$you start with 2 moles of ammonium nitrate, how many moles of water are formed?

Accepted Answer

$$8$$ moles

Question 6

If you start with 5.0 g of sodium ($$Na$$), how many grams of chlorine gas ($$Cl_2) $$are needed for complete reaction to form sodium chloride ($$NaCl$$)? ($$2Na + Cl_2$ \rightarrow 2NaCl$$; $$M_{Na} = 22.99 g/$$mol, $$M_{Cl_2$} = 70.90 g/$$mol)

Accepted Answer

$$7.71 g$$

Question 7

Industrial production of hydriodic acid ($$HI) $$takes place by the reaction $$I_2 + N_2H_4$$ \rightarrow 2HI + $$N_2. $$How many grams of $$I_2$$ are needed to react with 36.7 g of $$N_2H_4$$? ($$M_{I_2$} = 254 g/$$mol, $$M_{N_2H_4} = 32 g/$$mol)

Accepted Answer

$$291 g$$

Question 8

In a reaction, 2.3 g of sodium reacts with 3.5 g of chlorine to form sodium chloride. The theoretical yield is 5.8 g, but only 5.5 g is obtained. What is the percent yield?

Accepted Answer

$$95\%$$

Question 9

What is the molarity of a solution prepared by dissolving 10.0 g of sodium chloride ($$NaCl) in $$enough water to make 0.500 L of solution? ($$M_{NaCl} = 58.44 g/$$mol)

Accepted Answer

$$0.342 M$$

Question 10

If 0.123 L of a 1.00 M NaCl solution is mixed with excess Pb(NO$$_3$$)$$_2$$, how many grams of PbCl$$_2$$ will precipitate? ($$PbCl_2$$ molar mass = 278 g/mol)

Accepted Answer

$$17.1 g$$

Question 11

A 50.0 mL sample of 0.50 M NaCl is mixed with 50.0 mL of 0.40 M AgNO$$_3. $$What mass of AgCl will precipitate? ($$M_{AgCl} = 143.32 g/$$mol)

Accepted Answer

$$2.87 g$$

Question 12

You dilute 125.0 mL of a 0.15 M NaOH solution to a final volume of 150.0 mL. What is the molarity of the diluted solution?

Accepted Answer

$$0.125 M$$

Question 13

A 10.0 mL sample of HCl is titrated with 0.10 M NaOH and requires 25.0 mL to reach the endpoint. What is the concentration of the HCl solution?

Accepted Answer

$$0.25 M$$

Question 14

A 0.55 g sample of a monoprotic acid is titrated and requires 36.2 mL of 0.10 M NaOH to reach the endpoint. What is the molar mass of the acid?

Accepted Answer

$$152 g/$$mol

Question 15

A hydrocarbon is combusted, producing 11.8 g of $$CO_2$$ and 4.729 g of $$H_2O. $$What is the empirical formula of the hydrocarbon?

Accepted Answer

$$CH_2$$

Question 16

In a precipitation reaction, 75.0 mL of 0.100 M $$Pb(NO_3$)_2 is $$mixed with 100.0 mL of 0.190 M $$KI. $$What is the limiting reagent?

Accepted Answer

$$Pb(NO_3$)_2$$

Question 17

After mixing 75.0 mL of 0.100 M $$Pb(NO_3$)_2$$ and 100.0 mL of 0.190 M $$KI$$, what is the final molarity of $$K^+$$ ions in the solution?

Accepted Answer

$$0.109 M$$

Question 18

Which of the following best describes the limiting reagent in a chemical reaction?

Accepted Answer

The reactant that is completely consumed first, limiting the amount of product formed.

Question 19

If you have 12 frames and 20 wheels, and each bicycle requires 1 frame and 2 wheels, what is the maximum number of bicycles you can build?

Accepted Answer

$$10$$

Stoichiometry, Mole Calculations, and Limiting Reagents in General Chemistry

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