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Chapter 13: QCYL (page 717)

Round the following to the indicated number of significant figures:

(a) 0.424 (to two significant figures)

(b) 0.0038661 (to three significant figures)

(c) 421.25 (to four significant figures)

(d) 28,683.5 (to five significant figures)

Short Answer

Expert verified

a) 0.424 rounds down to 0.42.

b) 0.0038661 rounds up to 0.00387.

c) 421.25 rounds down to 421.2.

d) 28,683.5 rounds up to 28,684.

Step by step solution

01

Significant figures

All the digits in measurement, including the uncertain last digit, are called significant figures or significant digits.

02

Rules used to determine the significant figures in a number

  • Non-zero digits are always significant.
  • Any zero between two significant digits is significant.

a) 0.424 rounds "down" to 0.42 (The removed digit, 4, is less than 5).

b) 0.0038661 rounds "up" to 0.00387 (The removed digit, 6, and the retained digit are odd).

c) 421.25 rounds "down" to 421.2 (The removed digit, 5, and the retained digit are even).

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Most popular questions from this chapter

A sample of ammonium chloride was heated in a closed container. NH4 Cl (s)鈬� NH3 (g) + HCl(g)at equilibrium, the pressure of NH3 (g)was found to be 1.75 atm. What is the value of the equilibrium constant, Kp, for the decomposition at this temperature?

A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide (\({\rm{S}}{{\rm{O}}_3}\)), from sulfur dioxide (\({\rm{S}}{{\rm{O}}_2}\)), and oxygen (\({{\rm{O}}_2}\)), shown here.

\(2{\text{S}}{{\text{O}}_2}(g) + {{\text{O}}_2}(g) \rightleftharpoons 2{\text{S}}{{\text{O}}_3}(g)\)

At high temperatures, the rate of formation of \({\rm{S}}{{\rm{O}}_3}\)is higher, but the equilibrium amount (concentration or partial pressure) of \({\rm{S}}{{\rm{O}}_3}\) is lower than it would be at lower temperatures.

(a) Does the equilibrium constant for the reaction increase, decrease, or remain about the same as the temperature increases?

(b) Is the reaction endothermic or exothermic?

Acetic acid is a weak acid that reacts with water according to this equation:

\(C{H_3}C{O_2}H(aq) + {H_2}O(aq) \rightleftharpoons {H_3}{O^ + }(aq) + C{H_3}CO_2^ - (aq)\)

Will any of the following increase the percent of acetic acid that reacts and produces \(C{H_3}CO_2^ - \)ion?

(a) Addition of \(HCl\)

(b) Addition of \(NaOH\)

(c) Addition of \(NaC{H_3}C{O_2}\)

For which of the reactions in Exercise 13.15 does\({K_c}\)(calculated using concentrations) equal\({K_p}\)(calculated using pressures)?

(a) \(C{H_4}(g) + C{l_2} \rightleftharpoons C{H_3}CI(g) + HCI(g)\)

(b) \({N_2}(g) + {O_2}(g)\rightleftharpoons 2NO(g)\)

(c) \(2S{O_2}(\;g) + {O_2}(\;g)\rightleftharpoons 2S{O_3}(\;g)\)

(d) \(BaS{O_3}(s)\rightleftharpoons BaO(s) + S{O_2}(g)\)

(e) \({P_4}(g) + 5{O_2}(g)\rightleftharpoons{P_4}{O_{10}}(s)\)

(f) \(B{r_2}(\;g)\rightleftharpoons 2Br(g)\)

(g) \(C{H_4}(g) + 2{O_2}(g)\rightleftharpoons C{O_2}(g) + 2{H_2}O(l)\)

(h)\(CuS{O_4} \times 5{H_2}O(s)\rightleftharpoons CuS{O_4}(s) + 5{H_2}O(g)\)

If you observe the following reaction at equilibrium, is it possible to tell whether the reaction stated with pure \(N{O_2}\) or with pure \({N_2}{O_4}\)? \(2N{O_2}(g) \rightleftharpoons {N_2}{O_4}(g)\)
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