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3 years ago

Significant Figures For 7.06 × 10^5 ÷ 5.3 × 10^-2

Chemistry

1 answer:

Kay [80]3 years ago

4 0

Answer:

$\boxed{\text{two}}$

Explanation:

In multiplication and division problems, your answer can have no more significant figures than the number with the fewest significant figures.

$\dfrac{7.06 \times 10^{5}}{5.3 \times 10^{-2}}= 1.332 075 472 \times 10^{7}$ (by my calculator)

There are three significant figures in 7.06 and two in 2.3.

You must round to $\boxed{\textbf{two}}$ significant figures and report the answer as 1.3 × 1.0⁷.

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Which of the following pairs of elements would form the covalent bond with the largest dipole moment? View Available Hint(s) Whi

LekaFEV [45]

Answer:

In-F bond has the largest dipole moment.

Explanation:

Given the electronegativities:

Ge= 2.01

O= 3.44

H= 2.20

P= 2.19

In= 1.78

F= 3.98

B= 2.04

N= 3.04

The bond between Ge and O has an electronegativity difference:

ED= 3.44 - 2.01= 1.43

The bond between H and P has an electronegativity difference:

ED= 2.20 - 2.19= 0.01

The bond between In and F has an electronegativity difference:

ED= 3.98 - 1.78= 2.20

The bond between B and N has an electronegativity difference:

ED= 3.04 - 2.04= 1.00

As In-F bond has the largest electronegativity difference, this is the covalent bond with the largest dipole moment.

6 0

3 years ago

0.052301 km significant figures

lesya [120]

Answer:

Five significant figures.

Explanation:

The given measurement have five significant figures 52301.

All non-zero digits are consider significant figures like 1, 2, 3, 4, 5, 6, 7, 8, 9.

Leading zeros are not consider as a significant figures. e.g. 0.03 in this number only one significant figure present which is 3.

Zero between the non zero digits are consider significant like 104 consist of three significant figures.

The zeros at the right side e.g 2400 are also significant. There are four significant figures are present.

3 0

3 years ago

Given the following reaction: 3D(g) + E(g) + 2F(g) → 5G(g) + 4H(g)

evablogger [386]

Answer:

Explanation:

Hello,

The law of mass action, allows us to know the required amounts, thus, for this chemical reaction it is:

$\frac{1}{-3} \frac{d[D]}{dt} =\frac{1}{-1} \frac{d[E]}{dt} =\frac{1}{-2} \frac{d[F]}{dt} =\frac{1}{5} \frac{d[G]}{dt} =\frac{1}{4} \frac{d[H]}{dt}$

Now, we answer:

(a)

$\frac{d[H]}{dt}=4*\frac{1}{-3} *(-0.12M/s)=0.16M/s$

(b)

$\frac{d[E]}{dt}=-1*\frac{1}{5} *(0.2M/s)=-0.04M/s$

$r=\frac{1}{-3} \frac{d[D]}{dt} =\frac{1}{-1} \frac{d[E]}{dt} =\frac{1}{-2} \frac{d[F]}{dt} =\frac{1}{5} \frac{d[G]}{dt} =\frac{1}{4} \frac{d[H]}{dt}$