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oksano4ka [1.4K]
1 year ago
8

Write the following numbers in standard notation. Use a terminal decimal point when needed.

Chemistry
1 answer:
ololo11 [35]1 year ago
5 0

The standard notation of 1.0070x10⁴ is 10070

To express enormous figures which are in standard notation like 1,300,000 or exceedingly minuscule quantities like 0.0000000000045, scientists use scientific notation. Scientific notation, also referred to as exponential form, is one of the earliest mathematical techniques. It is well regarded by practitioners. People use scientific notation to handle situations where numbers are too large or too small to be calculated easily. Scientists, engineers, and mathematicians all use this technique. where as standard notation is way writing numbers in normal decimal form. The scientific method id most convenient denoting numbers as the numbers will be either too big or too small.

To learn more about standard notation:

brainly.com/question/10253124

#SPJ4

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20 because
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mass no-electrons=neutron
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12. Calculate the hydroxide ion concentration of a solution with pH = 10.25. Show all calculations leading to an answer.
Alex787 [66]
PH= log[H3O+]
10.25=log [H3O+]
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The equilibrium constant for the following reaction: H2(g) + Br2(g) ↔ 2HBr (g) is 1.65 x 103 at a certain temperature. Find the
Aleks [24]

Answer:

6.97 atm was the equilibrium pressure of HBr .

Explanation:

The value of the equilibrium constant =K_p=1.65\times 10^3

H_2+Br_2\rightleftharpoons 2HBr

Initially:

0             0                 7.10 atm

At equilibrium

x              x                 (7.10-2x)

The expression of equilibrium constant can be written as:

K_p=\frac{p_{HBr}}{p_{H_2}\times p_{Br_2}}

1.65\times10^3=\frac{(7.10-2x)}{x^2}

Solving for x:

x = 0.065

Partial pressure of HBr at equilibrium :(7.10 - 2 × 0.065) atm = 6.97 atm

6.97 atm was the equilibrium pressure of HBr .

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Electron 

 ~~~hope this helps~~~
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What volume of carbon dioxide gas can be collected from
alisha [4.7K]

Answer:

1.22 L of carbon dioxide gas

Explanation:

The reaction that takes place is:

  • CaCO₃ + HCl → CaCl₂ + CO₂ + H₂O

First we <u>determine which reactant is limiting</u>:

  • Calcium carbonate ⇒ 10.0 g CaCO₃ ÷ 100 g/mol = 0.10 mol CaCO₃
  • Hydrochloric acid ⇒ 0.100 L * 0.50 M = 0.05 mol HCl

So HCl is the limiting reactant.

Now we calculate the moles of CO₂ produced:

  • 0.05 mol HCl * \frac{1molCO_{2}}{1molHCl} = 0.05 mol CO₂

Finally we use PV=nRT to <u>calculate the volume</u>:

  • P = 1 atm
  • n = 0.05 mol
  • T = 25 °C ⇒ 25 + 273.16 = 298.16 K

1 atm * V = 0.05 mol * 0.082 atm·L·mol⁻¹·K⁻¹ * 298.16 K

  • V = 1.22 L
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