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Chapter 12: QCYL (page 651)

(a) Multiply 2.334 cm and 0.320 cm.(b) Divide 55.8752 m by 56.53 s.

Short Answer

Expert verified

(a) The result is 0.747cm² (rounded to three significant figures).

(b) The result is 0.9884 m/s (rounded to four significant figures).

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

Determining the significant figures in multiplication and division

2.334cm × 0.320 cm

=0.74688cm²

The result is 0.747cm² (rounded to three significant figures).

(b) $\begin{array}{l} \frac{55.8752 m}{56.53 s} \\ = 0.9884167699 m / s \\ = 0.9884 m / s \end{array}$

The result is 0.9884 m/s (rounded to four significant figures).

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Most popular questions from this chapter

In the PhET Reactions & Rates (http://openstaxcollege.org/l/16PHETreaction) interactive, use the “Many Collisions” tab to observe how multiple atoms and molecules interact under varying conditions. Select a molecule to pump into the chamber. Set the initial temperature and select the current amounts of each reactant. Select “Show bonds” under Options. How is the rate of the reaction affected by concentration and temperature?

In an experiment, a sample of NaClO₃ was 90% decomposed in 48 min. Approximately how long would this decomposition have taken if the sample had been heated 20°C higher?

A study of the rate of the reaction represented as 2A⟶ B gave the following data:

Determine the average rate of disappearance of A between 0.0 s and 10.0 s, and between 10.0 s and 20.0 s.
Estimate the instantaneous rate of disappearance of A at 15.0 s from a graph of time versus (A). What are the units of this rate?
Use the rates found in parts (a) and (b) to determine the average rate of formation of B between 0.00 s and 10.0 s, and the instantaneous rate of formation of B at 15.0 s.

Regular flights of supersonic aircraft in the stratosphere are of concern because such aircraft produce nitric oxide, NO, as a by-product in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction $N O + O_{3} \to N O_{2} + O_{2}$ is first order with respect to both NO and $O_{3}$ with a rate constant of $2 .20 \times 1 0^{7} m o l L^{- 1} s^{- 1}$ . What is the instantaneous rate of disappearance of NO when $(N O) = 3 .3 \times 1 0^{- 6} M$ and $(O_{3}) = 5 .9 \times 1 0^{- 7} M$ ?

Consider this scenario and answer the following questions: Chlorine atoms resulting from decomposition of chlorofluoromethanes, such as $C C l_{2} F_{2}$ , catalyse the decomposition of ozone in the atmosphere. One simplified mechanism for the decomposition is:

$\begin{array}{r} O_{3} \overset{s u n l i g h t}{\to} O_{2} + O \\ O_{3} + C l \to O_{2} + C l O \\ C l O + O \to C l + O_{2} \end{array}$

(a) Explain why chlorine atoms are catalysts in the gas-phase transformation:

$2 O_{3} \overset{}{} \to 3 O_{2}$

(b) Nitric oxide is also involved in the decomposition of ozone by the mechanism: Is NO a catalyst for the decomposition? Explain your answer.

$\begin{array}{r} O_{3} \overset{s u n l i g h t}{\to} O_{2} + O \\ O_{3} + N O \to N O_{2} + O_{2} \\ N O_{2} + O \to N O + O_{2} \end{array}$

See all solutions

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