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3 years ago

Match each decimal number to the correct scientific notation.

Chemistry

2 answers:

Effectus [21]3 years ago

5 0

3.07 × 10^4=30,700

3.07 × 10^-4=0.000307

3.07 × 10^-6=0.00000307

3.07 × 10^6=3,070,000

GREYUIT [131]3 years ago

4 0

Answers are:

3.07 × 10^4 = 30,700.

3.07 × 10^-4 = 0.000307.

3.07 × 10^-6 = 0.00000307.

3.07 × 10^6 = 3,070,000.

1) 10^4 = 10 × 10 × 10 × 10.

10^4 = 10,000.

3.07 × 10^4 = 3.07 × 10,000.

3.07 × 10^4 = 30,700.

2) 10^-4 = 1 ÷ (10 × 10 × 10 × 10).

10^-4 = 1 ÷ 10,000.

10^-4 = 0.0001.

3.07 × 10^-4 = 3.07 × 0.0001.

3.07 × 10^-4 = 0.000307.

3) 10^-6 = 1 ÷ (10 × 10 × 10 × 10 × 10 × 10).

10^-6 = 1 ÷ 1,000,000.

10^-6 = 0.000001.

3.07 × 10^-6 = 3.07 × 0.000001.

3.07 × 10^-6 = 0.00000307.

4) 10^6 = 10 × 10 × 10 × 10 × 10 × 10.

10^6 = 1,000,000.

3.07 × 10^6 = 3.07 × 1,000,000.

3.07 × 10^6 = 3,070,000.

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Answer: The molecular formula for the compound is $C_6H_6$

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Moles of Hydrogen = $\frac{\text{Given mass of Hydrogen}}{\text{Molar mass of Hydrogen}}=\frac{7.74g}{1g/mole}=7.74moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 7.68 moles.

For Carbon = $\frac{7.68}{7.68}=1$

For Hydrogen = $\frac{7.74}{7.68}=1$

Step 3: Taking the mole ratio as their subscripts.

The ratio of C : H = 1 : 1

The empirical formula for the given compound is $CH$

Calculating the molar mass of the compound:

To calculate the molecular mass, we use the equation given by ideal gas equation:

PV = nRT

Or,

$PV=\frac{m}{M}RT$

where,

P = pressure of the gas = 820 torr

V = Volume of gas = 250 mL = 0.250 L (Conversion factor: 1 L = 1000 mL )

m = mass of gas = 0.6883 g

M = Molar mass of gas = ?

R = Gas constant = $62.3637\text{ L. torr }mol^{-1}K^{-1}$

T = temperature of the gas = $100^oC=(100+273)K=373K$

Putting values in above equation, we get:

$820torr\times 0.250L=\frac{0.6883g}{M}\times 62.3637\text{ L torr }mol^{-1}K^{-1}\times 373K\\\\M=\frac{0.6883\times 62.3637\times 373}{820\times 0.250}=78.10g/mol$